Understanding and Polymer Structure
Polymers - Definition, Structure, Properties, Classification, Formation, Uses, Benefits, Example: Polymers are repeating chains of long atoms, formed from binders in the form of identical molecules called monomers. Although most are organic compounds (having carbon chains), there are also many inorganic polymers.
Definition of Polymers
Polymer is a macromolecule or also called a giant molecule composed of several monomers (simple small molecules). Polymers are large molecules (macromolecules) consisting of small, simple, and recurring chemical structures composed of covalent bonds. This repeating unit is usually equivalent or almost equivalent to a monomer, the starting material of a polymer.
Currently, polymers are widely used in meeting daily needs. Polymers are usually produced in many developing countries and are cheap. Examples of uses of polymers are to make bottles, drums, pipes, home furniture and so on. Therefore, in this paper we will discuss about polymers and their applications so that we understand more about polymers and their development in meeting daily needs.
Understanding Monomers
A monomer is any substance that can be converted into a polymer. For example, ethylene is a monomer that can be polymerized into polyethylene (see reaction below). Amino acids include monomers too, which can be polymerized to polypeptides by the release of water.
monomer example
Polymer Examples
carbohydrate,
protein,
fat, natural rubber,
and a number of plastics such as polyethylene (PE),
PP polypropylene plastic,
PET polyethylene terephthalate plastic,
PVC polyvinyl chloride plastic,
PS polystyrene plastic,
Teflon, and Nylon.
Polymer Structure
Based on the structure of the polymer is divided into:
Linear polymer
Linear polymers consist of long chains of skeletal atoms that can bind to substituent groups. These polymers can usually dissolve in several solvents, and are solid at normal temperatures. This polymer exists as an elastomer, a flexible (flexible) or thermoplastic material such as glass).
Linear polymer
Examples: Polyethylene, polyvinyl chloride (PVC), polymethyl methacrylate (PMMA), Lucite, Plexiglas, or perspex), polyacrylonitrile (orlon or creslan) and nylon 66.
Branched polymer
The branched polymer can be visualized as a linear polymer with a branching on the same basic structure as the main chain.
Three-dimensional network polymer
Three-dimensional tissue polymers are polymers with chemical bonds present between chains. This material is usually swelled (inflated) by the solvent but not until it dissolves. This irregularity can be used as a criterion of network structure. The greater the percentage of cross-links (cross-links) the smaller the amount of swelling. If the degree of crosslinking is high enough, the polymer can become rigid, high melting point, solid that cannot be inflated, for example diamond (diamond).
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Sulfur Oxides are the Result of Burning Fossil Fuels
Sulfur Oxides are the Result of Burning Fossil Fuels
Acid rain
Rainwater is usually acidic with a pH of around 6. This is because rainwater mixes with carbon dioxide in the air to produce carbonic acid. Well, if the pH of rainwater is less than 5.6 ... this phenomenon is called acid rain.
Acid rain occurs because the air is polluted by substances (oxides) that are acidic, especially sulfur oxides (SO2 and SO3) and nitrogen oxides (NO2).
Sulfur oxides are the result of burning fossil fuels, especially coal, and the metal processing industry. whereas nitrogen oxides come from motor vehicle fumes and industrial fumes.
Acid rain causes losses because it can disturb the balance of the ecosystem, reduce soil fertility, damage buildings especially those made of metal and carbonate rock (marble), kill living things in water, and damage forests because soil pH is too acidic and can cause plants to die. Soil pH ranges from 4 to 8, but mostly between 6.5 and 7.5. In lime soils are usually more alkaline, whereas in sandy or peat (swamps) and clay soils are usually more acidic. Fertile soils are usually in the range of 6.5 to 7.5.
Acid in the Laboratory
very many types of acids used in laboratories, both school laboratories, campuses, as well as company and research laboratories. Among others are..
Bases in the Human Body
Guess what! where is the presence of acid in our body? If you say it's in the stomach, your answer is correct! Yay ... stomach acid is the same HCl (hydrochloric acid) that you used for the lab yesterday. The pH is 1-2 ... strong acid! why does our body need stomach acid with a strong pH?
Remember, how can HCl be able to aluminum plate until it runs out? It's scary if our stomach becomes perforated.
Normally, stomach acid works to kill bacteria that enter the food you eat. God is good, we know that we often eat carelessly. Forgot to wash your hands ... eat along the road a lot of dust ... what ... there must be a lot of bacteria that enter the stomach through these foods. Well ... this stomach acid (HCl) will neutralize everything ... kill the incoming bacteria! Especially if zinc ketek * God forbid * ... but calm ... stomach acid will neutralize it
Gastric acid can also create conditions suitable for protein digestion. So in the process of protein digestion, the enzyme that works on this process only wants if the acidic conditions in the stomach are already right, then he wants to work digesting protein.
You've all used NaOH in practicum right? actually the benefits of NaOH in everyday life are very many. NaOH is known as fire soda. NaOH is the raw material in making soap because it can dissolve fat into soap compounds. This reaction to making soap is called saponification.
Fire soda is also used to wash the sink and open the toilet drain which is clogged with paper or tissue material, because the soda can destroy cellulose which is the basic material of paper and tissue. Soda fire is also commonly used to clean ovens (grills). Fire soda in the industry is also widely used in making paper and rayon as a bleach.
Next is calcium hydroxide Ca (OH) 2 or lime. Lime is usually used by grandmothers for betel and cement mixed building materials. Come on you try to find out, why do grandmothers like betel ?? Hehehe. Lime is also used to neutralize soil polluted by acid rain.
Another example is ammonia (NH3) which is often used in facial cleansers or glass cleaners. Why? because the ammonia base is a weak base. Remember the nature of bases that can dissolve fat.
Acid rain
Rainwater is usually acidic with a pH of around 6. This is because rainwater mixes with carbon dioxide in the air to produce carbonic acid. Well, if the pH of rainwater is less than 5.6 ... this phenomenon is called acid rain.
Acid rain occurs because the air is polluted by substances (oxides) that are acidic, especially sulfur oxides (SO2 and SO3) and nitrogen oxides (NO2).
Sulfur oxides are the result of burning fossil fuels, especially coal, and the metal processing industry. whereas nitrogen oxides come from motor vehicle fumes and industrial fumes.
Acid rain causes losses because it can disturb the balance of the ecosystem, reduce soil fertility, damage buildings especially those made of metal and carbonate rock (marble), kill living things in water, and damage forests because soil pH is too acidic and can cause plants to die. Soil pH ranges from 4 to 8, but mostly between 6.5 and 7.5. In lime soils are usually more alkaline, whereas in sandy or peat (swamps) and clay soils are usually more acidic. Fertile soils are usually in the range of 6.5 to 7.5.
Acid in the Laboratory
very many types of acids used in laboratories, both school laboratories, campuses, as well as company and research laboratories. Among others are..
Bases in the Human Body
Guess what! where is the presence of acid in our body? If you say it's in the stomach, your answer is correct! Yay ... stomach acid is the same HCl (hydrochloric acid) that you used for the lab yesterday. The pH is 1-2 ... strong acid! why does our body need stomach acid with a strong pH?
Remember, how can HCl be able to aluminum plate until it runs out? It's scary if our stomach becomes perforated.
Normally, stomach acid works to kill bacteria that enter the food you eat. God is good, we know that we often eat carelessly. Forgot to wash your hands ... eat along the road a lot of dust ... what ... there must be a lot of bacteria that enter the stomach through these foods. Well ... this stomach acid (HCl) will neutralize everything ... kill the incoming bacteria! Especially if zinc ketek * God forbid * ... but calm ... stomach acid will neutralize it
Gastric acid can also create conditions suitable for protein digestion. So in the process of protein digestion, the enzyme that works on this process only wants if the acidic conditions in the stomach are already right, then he wants to work digesting protein.
You've all used NaOH in practicum right? actually the benefits of NaOH in everyday life are very many. NaOH is known as fire soda. NaOH is the raw material in making soap because it can dissolve fat into soap compounds. This reaction to making soap is called saponification.
Fire soda is also used to wash the sink and open the toilet drain which is clogged with paper or tissue material, because the soda can destroy cellulose which is the basic material of paper and tissue. Soda fire is also commonly used to clean ovens (grills). Fire soda in the industry is also widely used in making paper and rayon as a bleach.
Next is calcium hydroxide Ca (OH) 2 or lime. Lime is usually used by grandmothers for betel and cement mixed building materials. Come on you try to find out, why do grandmothers like betel ?? Hehehe. Lime is also used to neutralize soil polluted by acid rain.
Another example is ammonia (NH3) which is often used in facial cleansers or glass cleaners. Why? because the ammonia base is a weak base. Remember the nature of bases that can dissolve fat.
Feature Base Solution
Feature Base Solution
Bases are substances that can neutralize acids. Chemically acids and bases contradict each other. Water-soluble bases are called alkalis.
based on their strength, bases are divided into weak bases and strong bases. The smaller the pH value, the stronger the base. I corrected this one too .. A weak base has a pH of around 9-11, whereas a strong base has a pH from 12 to 14.
The PH is more than 7
Making red litmus paper into blue litmus paper (change color)
Bitter
Corrosive to skin
Example:
KOH + H2O K + + OH–
CaOH + H2O Ca ++ OH–
Some bases that we can find in everyday life are:
Chemical Base Formula Name Example Material
Aluminum hydroxide
Calcium hydroxide
Sodium hydroxide
Potassium hydroxide
Magnesium hydroxide
AlOH3
CaOH2
NaOH
KOH
Mg (OH) 2
Deodorant
Plaster
Soap ingredients, cleaning drains
Soap ingredients
Heartburn medication
The Nature of Base Solutions
Basa (alkali) comes from Arabic which means ash. One definition of a base is a substance which, if dissolved in water, will produce hydroxide ions (OH-).
Initial indicators were obtained from plants, but now they are made in factories. Litmus, for example, is obtained from lycen, a symbiosis of fungi and algae. Apart from lichens, various colored plants can be used as indicators of acid-base. For example petals, red cabbage, and beets.
Acidity (pH)
Acid solutions have different levels of acidity. Differences in acidity can occur due to differences in concentrations. The acidity level is commonly expressed on a pH scale. The pH scale ranges from 0 to 14 with the following conditions:
Acid solutions have a pH <7
Base solution has a pH> 7
Neutral solutions have pH = 7
So the more acidic a solution is, the smaller the pH. Solutions with pH = 1 have 10 times more acidic properties than solutions with pH = 2.
The hydroxide ion has a negative charge (so it's given a minus sign (-) next to the back of OH). Bases are the opposite of acids. In general, Bases have the following properties:
Bitter taste when dissolved in water (only for weak bases)
Touch: feels slippery like soap when touched (only for weak bases)
Caustic (can damage skin tissue / irritation)
Electric conductivity: can conduct electricity (an electrolyte solution)
The degree of acidity (pH) is greater than 7
Change the litmus color to blue
In its pure state it is generally in the form of solid crystals
can emulsify oil
Also Read Articles That May Be Associated: Compounds: Understanding, Characteristics, Properties, And Kinds With Complete Examples
Examples of Base Solutions
Some examples of bases used in daily life are as follows:
Soda fire (sodium hydroxide NaOH) functions to dissolve fats and oils so that it can be used to open clogged sinks.
Calcium hydroxide or lime (Ca (OH) 2) is used for whiting and as a building material, which is a mixture of cement mortar
Ammonia (NH3 solution) is used in facial cleansers or glass cleaners
Acid in the Body
Everyday life bases
Fire soda (sodium hydroxide, NaOh), functions to:
- Dissolve fats and oils
- clean the oven
- destroy seloluse
Calcium hydroxide or lime (Ca (OH)
Ammonia (NH3 solution) is used as a glass cleaner.
Indicator
The way to find out whether a substance is classified as acidic or basic is to use an indicator.
Indicator is a substance that can be paid for colors when inserted into acidic or basic compounds. Indicator can be paper or solution, indicator in the form of paper is litmus paper.
There are two kinds of litmus paper, namely red litmus and blue litmus. How to use is litmus paper inserted into the compound, then see the color change.
A compound is acidic if the blue litmus paper turns red, but the red litmus paper does not change color ... while if the base group compound is red the litmus paper turns blue, but the blue litmus paper does not change color. If the compound does not change the color of litmus paper, it is classified as not an acid or base or a neutral compound.
Bases are substances that can neutralize acids. Chemically acids and bases contradict each other. Water-soluble bases are called alkalis.
based on their strength, bases are divided into weak bases and strong bases. The smaller the pH value, the stronger the base. I corrected this one too .. A weak base has a pH of around 9-11, whereas a strong base has a pH from 12 to 14.
The PH is more than 7
Making red litmus paper into blue litmus paper (change color)
Bitter
Corrosive to skin
Example:
KOH + H2O K + + OH–
CaOH + H2O Ca ++ OH–
Some bases that we can find in everyday life are:
Chemical Base Formula Name Example Material
Aluminum hydroxide
Calcium hydroxide
Sodium hydroxide
Potassium hydroxide
Magnesium hydroxide
AlOH3
CaOH2
NaOH
KOH
Mg (OH) 2
Deodorant
Plaster
Soap ingredients, cleaning drains
Soap ingredients
Heartburn medication
The Nature of Base Solutions
Basa (alkali) comes from Arabic which means ash. One definition of a base is a substance which, if dissolved in water, will produce hydroxide ions (OH-).
Initial indicators were obtained from plants, but now they are made in factories. Litmus, for example, is obtained from lycen, a symbiosis of fungi and algae. Apart from lichens, various colored plants can be used as indicators of acid-base. For example petals, red cabbage, and beets.
Acidity (pH)
Acid solutions have different levels of acidity. Differences in acidity can occur due to differences in concentrations. The acidity level is commonly expressed on a pH scale. The pH scale ranges from 0 to 14 with the following conditions:
Acid solutions have a pH <7
Base solution has a pH> 7
Neutral solutions have pH = 7
So the more acidic a solution is, the smaller the pH. Solutions with pH = 1 have 10 times more acidic properties than solutions with pH = 2.
The hydroxide ion has a negative charge (so it's given a minus sign (-) next to the back of OH). Bases are the opposite of acids. In general, Bases have the following properties:
Bitter taste when dissolved in water (only for weak bases)
Touch: feels slippery like soap when touched (only for weak bases)
Caustic (can damage skin tissue / irritation)
Electric conductivity: can conduct electricity (an electrolyte solution)
The degree of acidity (pH) is greater than 7
Change the litmus color to blue
In its pure state it is generally in the form of solid crystals
can emulsify oil
Also Read Articles That May Be Associated: Compounds: Understanding, Characteristics, Properties, And Kinds With Complete Examples
Examples of Base Solutions
Some examples of bases used in daily life are as follows:
Soda fire (sodium hydroxide NaOH) functions to dissolve fats and oils so that it can be used to open clogged sinks.
Calcium hydroxide or lime (Ca (OH) 2) is used for whiting and as a building material, which is a mixture of cement mortar
Ammonia (NH3 solution) is used in facial cleansers or glass cleaners
Acid in the Body
Everyday life bases
Fire soda (sodium hydroxide, NaOh), functions to:
- Dissolve fats and oils
- clean the oven
- destroy seloluse
Calcium hydroxide or lime (Ca (OH)
Ammonia (NH3 solution) is used as a glass cleaner.
Indicator
The way to find out whether a substance is classified as acidic or basic is to use an indicator.
Indicator is a substance that can be paid for colors when inserted into acidic or basic compounds. Indicator can be paper or solution, indicator in the form of paper is litmus paper.
There are two kinds of litmus paper, namely red litmus and blue litmus. How to use is litmus paper inserted into the compound, then see the color change.
A compound is acidic if the blue litmus paper turns red, but the red litmus paper does not change color ... while if the base group compound is red the litmus paper turns blue, but the blue litmus paper does not change color. If the compound does not change the color of litmus paper, it is classified as not an acid or base or a neutral compound.
Strong Acidic Acid Base
Strong Acidic Acid Base
Weak base solution
Ie, a base where only some of its molecules are broken down into OH- ions. The concept of salt solutions derived from strong acids and weak bases are acidic. An example is NH4Cl, this salt is formed from the results of a neutralization reaction between NH3 and HCl and in fully ionized water produces NH4 + and Cl ions.
NH3 (aq) + HCl (aq) = NH4Cl (aq)
Strong acidic acid base
Weak
NH4Cl (aq) = NH4 (aq) + Cl (aq)
Ion Cl comes from strong acids, is a weak Bronsted-Lowry base so it does not react with water (unable to attract H + ions), whereas NH + ions come from weak bases, so it is a strong Bronsted-Lowry acid so that it can react with water (hydrolyzed) or give H + ions to water.
NH4 + (aq) + H2O === NH3 (aq) H3O + (l)
Because NH4 + ions can give H + ions to water, the solution becomes acidic and it is known that the Ka value from the equilibrium above is 5.6 x 10-10. Determination of pH
Example
If it is known that 0.1 M NH4Cl and Kb NH3 = 1.8x 10-5, then in the salt water NH4Cl is fully ionized with the following reaction equation:
NH4Cl (aq) = NH4 + (aq) + Cl- (aq)
Because the coefficients of NH4Cl and NH4 + are the same then [NH4 +] = [NH4Cl] = 0.1 M ions of NH4 + undergo hydrolysis as follows,
NH4 (aq) + + H2O (l) === NH3 (aq) + H3O + (aq)
The equation for the hydolysis constant is as follows,
Kh = [NH3] [H3O +]
[NH4 +]
Various Kinds of Bases
The strength of a base is influenced by the number of OH ions produced by the base compound in the solution. Based on how much OH ions are produced, base solutions are also divided into two types as follows.
Strong bases
A strong base is a base compound which ionizes entirely into its ions. The strong base ionization reaction is an end reaction.
In general, strong base ionisations are formulated as follows.
M (OH) x (aq) ⎯⎯ → Mx + (aq) + x OH– (aq)
Strong bases
Weak base
Weak bases are base compounds in which the solution is only slightly ionized into ions.
The weak base ionization reaction is also an equilibrium reaction.
In general, weak valence one ionization bases can be formulated as follows.
M (OH) (aq) ← ⎯⎯⎯⎯ → M + (aq) + OH– (aq)
Weak base
The stronger the base, the base equilibrium reaction is leaning to the right, as a result, the Kb increases.
Therefore, the price of Kb is a measure of base strength, the greater the Kb the stronger the base.
Based on the above equation, because on a weak base [M +] = [OH–], the above equation can be changed to:
Weak Acid 1
Examples of strong bases:
Lithium hydroxide (LiOH)
Sodium hydroxide (NaOH)
Potassium hydroxide (KOH)
Calcium hydroxide (Ca (OH) 2)
Rubidium hydroxide (RbOH)
Strontium hydroxide (Sr (OH) 2)
Sesium hydroxide (CsOH)
Barium hydroxide (Ba (OH) 2)
Magnesium hydroxide (Mg (OH) 2)
Beryllium hydroxide Be (OH) 2)
Examples of weak bases:
Ammonium hydroxide (NH4OH)
Aluminum hydroxide (Al (OH) 3)
Iron (III) hydroxide (Fe (OH) 3)
Ammonia (NH3)
Iron (II) hydroxide (Fe (OH) 2)
Carboxy hydroxide (CA (OH) 3)
Nickel hydroxide (Ni (OH) 2)
Zinc hydroxide (Zn (OH) 2)
Cadmium hydroxide (Cd (OH) 2)
Bismuth hydroxide (Bi (OH) 3)
Silver hydroxide (Ag (OH))
Gold (I) hydroxide (Au (OH))
Gold (III) hydroxide (Au (OH) 3)
Copper (I) hydroxide (Cu (OH) 2)
Copper (II) hydroxide (Cu (OH))
Mercury (I) hydroxide (Hg (OH))
Mercury (II) hydroxide (Hg (OH) 2)
Tin (II) hydroxide (Sn (OH) 2)
Tin (IV) hydroxide (Sn (OH) 4)
Lead (II) hydroxide (Pb (OH) 2)
Manganese hydroxide (Mn (OH) 2)
Cobalt (III) hydroxide (Co (OH) 3)
Cobalt (II) hydroxide (Co (OH) 2)
Anilia (C6H5NH2)
Dimethylamine ((CH3) 2NH)
Hydrasim (H2NNH2)
Hydroxylamide (HONH2)
Methylamine (CH3NH2)
Urea (H2NCONH2)
Glucose (C6H2O6)
Methyl hydroxide (CH3OH)
Weak base solution
Ie, a base where only some of its molecules are broken down into OH- ions. The concept of salt solutions derived from strong acids and weak bases are acidic. An example is NH4Cl, this salt is formed from the results of a neutralization reaction between NH3 and HCl and in fully ionized water produces NH4 + and Cl ions.
NH3 (aq) + HCl (aq) = NH4Cl (aq)
Strong acidic acid base
Weak
NH4Cl (aq) = NH4 (aq) + Cl (aq)
Ion Cl comes from strong acids, is a weak Bronsted-Lowry base so it does not react with water (unable to attract H + ions), whereas NH + ions come from weak bases, so it is a strong Bronsted-Lowry acid so that it can react with water (hydrolyzed) or give H + ions to water.
NH4 + (aq) + H2O === NH3 (aq) H3O + (l)
Because NH4 + ions can give H + ions to water, the solution becomes acidic and it is known that the Ka value from the equilibrium above is 5.6 x 10-10. Determination of pH
Example
If it is known that 0.1 M NH4Cl and Kb NH3 = 1.8x 10-5, then in the salt water NH4Cl is fully ionized with the following reaction equation:
NH4Cl (aq) = NH4 + (aq) + Cl- (aq)
Because the coefficients of NH4Cl and NH4 + are the same then [NH4 +] = [NH4Cl] = 0.1 M ions of NH4 + undergo hydrolysis as follows,
NH4 (aq) + + H2O (l) === NH3 (aq) + H3O + (aq)
The equation for the hydolysis constant is as follows,
Kh = [NH3] [H3O +]
[NH4 +]
Various Kinds of Bases
The strength of a base is influenced by the number of OH ions produced by the base compound in the solution. Based on how much OH ions are produced, base solutions are also divided into two types as follows.
Strong bases
A strong base is a base compound which ionizes entirely into its ions. The strong base ionization reaction is an end reaction.
In general, strong base ionisations are formulated as follows.
M (OH) x (aq) ⎯⎯ → Mx + (aq) + x OH– (aq)
Strong bases
Weak base
Weak bases are base compounds in which the solution is only slightly ionized into ions.
The weak base ionization reaction is also an equilibrium reaction.
In general, weak valence one ionization bases can be formulated as follows.
M (OH) (aq) ← ⎯⎯⎯⎯ → M + (aq) + OH– (aq)
Weak base
The stronger the base, the base equilibrium reaction is leaning to the right, as a result, the Kb increases.
Therefore, the price of Kb is a measure of base strength, the greater the Kb the stronger the base.
Based on the above equation, because on a weak base [M +] = [OH–], the above equation can be changed to:
Weak Acid 1
Examples of strong bases:
Lithium hydroxide (LiOH)
Sodium hydroxide (NaOH)
Potassium hydroxide (KOH)
Calcium hydroxide (Ca (OH) 2)
Rubidium hydroxide (RbOH)
Strontium hydroxide (Sr (OH) 2)
Sesium hydroxide (CsOH)
Barium hydroxide (Ba (OH) 2)
Magnesium hydroxide (Mg (OH) 2)
Beryllium hydroxide Be (OH) 2)
Examples of weak bases:
Ammonium hydroxide (NH4OH)
Aluminum hydroxide (Al (OH) 3)
Iron (III) hydroxide (Fe (OH) 3)
Ammonia (NH3)
Iron (II) hydroxide (Fe (OH) 2)
Carboxy hydroxide (CA (OH) 3)
Nickel hydroxide (Ni (OH) 2)
Zinc hydroxide (Zn (OH) 2)
Cadmium hydroxide (Cd (OH) 2)
Bismuth hydroxide (Bi (OH) 3)
Silver hydroxide (Ag (OH))
Gold (I) hydroxide (Au (OH))
Gold (III) hydroxide (Au (OH) 3)
Copper (I) hydroxide (Cu (OH) 2)
Copper (II) hydroxide (Cu (OH))
Mercury (I) hydroxide (Hg (OH))
Mercury (II) hydroxide (Hg (OH) 2)
Tin (II) hydroxide (Sn (OH) 2)
Tin (IV) hydroxide (Sn (OH) 4)
Lead (II) hydroxide (Pb (OH) 2)
Manganese hydroxide (Mn (OH) 2)
Cobalt (III) hydroxide (Co (OH) 3)
Cobalt (II) hydroxide (Co (OH) 2)
Anilia (C6H5NH2)
Dimethylamine ((CH3) 2NH)
Hydrasim (H2NNH2)
Hydroxylamide (HONH2)
Methylamine (CH3NH2)
Urea (H2NCONH2)
Glucose (C6H2O6)
Methyl hydroxide (CH3OH)
Base Solution Classification
Base Solution Classification
As with acids, alkaline substances can also be easily found in our daily lives. Its slippery nature and bitter taste are easy ways to recognize alkaline substances. Some examples of alkaline substances that are often used are:
Sodium hydroxide / caustic soda / soda ash and potassium hydroxide, as raw material for cleaning in the household, for example bath soap, washing soap, detergent, bleach and floor cleaner
Magnesium hydroxide and aluminum hydroxide, contained in stomach pain medications (antacids)
Ammonia, for disinfecting solvents (preventing infection) and urea fertilizer raw materials
Just like acids, bases are also divided into strong bases and weak bases. The strength of a base can be determined from its ability to release negatively charged hydroxide ions (OH- ions) when dissolved in water. The more OH ions released, the stronger the basic properties. All basic chemical formulas generally contain the OH– group.
some examples of strong bases and weak bases
As is the case with acid solutions, based on their ability to break down into OH-ions in water, basic solutions can be divided into two types namely, Strong Base Solutions and Weak Base Solutions
Titration of strong acid strong base is a method of determining the level of strong acid solution with a peniter (penitration) of a strong base solution, or determination of the level of a strong base solution with a peniter (penitrating) a solution of strong acid. The end point of the titration is the condition when the color changes of the indicator. The endpoint of the titration is expected to be close to the equivalent point of the titration, ie the condition when the strong acid solution precisely reacts with the strong base solution.
In the titration process of strong acids with strong bases and vice versa, both solutions can be ionized completely. This is because the solution of strong acids and strong bases is included in the strong electrolyte solution which can be ionized completely in water. Thus, the salt created in this reaction has neutral properties.
Therefore, in the titration process of strong acids with strong bases the equivalent point is when the pH of the mixture is equal to 7 (neutral).
Strong base solution
is a base when dissolved in partially or water. all the molecules ionize into OH- ions.
The concept of Salt from strong acids and strong bases
This salt solution is neutral. For example, the neutralization reaction between NaOH and HCl produces a salt of NaCl. In water, fully ionized NaCl produces Na + and Cl- ions
NaOH (aq) + HCl (aq) = NaCl (aq) + H2O (l)
Neutral acid base
Strong strong
NaCl = Na + + Cl-
The Na + ion comes from a strong base and the Cl- ion also comes from a strong acid, so both of these ions are acidic and the Bronsted-Lowry base is weak so that both do not react with water (not hydrolyzed). Therefore the solution is neutral or pH = 7
As with acids, alkaline substances can also be easily found in our daily lives. Its slippery nature and bitter taste are easy ways to recognize alkaline substances. Some examples of alkaline substances that are often used are:
Sodium hydroxide / caustic soda / soda ash and potassium hydroxide, as raw material for cleaning in the household, for example bath soap, washing soap, detergent, bleach and floor cleaner
Magnesium hydroxide and aluminum hydroxide, contained in stomach pain medications (antacids)
Ammonia, for disinfecting solvents (preventing infection) and urea fertilizer raw materials
Just like acids, bases are also divided into strong bases and weak bases. The strength of a base can be determined from its ability to release negatively charged hydroxide ions (OH- ions) when dissolved in water. The more OH ions released, the stronger the basic properties. All basic chemical formulas generally contain the OH– group.
some examples of strong bases and weak bases
As is the case with acid solutions, based on their ability to break down into OH-ions in water, basic solutions can be divided into two types namely, Strong Base Solutions and Weak Base Solutions
Titration of strong acid strong base is a method of determining the level of strong acid solution with a peniter (penitration) of a strong base solution, or determination of the level of a strong base solution with a peniter (penitrating) a solution of strong acid. The end point of the titration is the condition when the color changes of the indicator. The endpoint of the titration is expected to be close to the equivalent point of the titration, ie the condition when the strong acid solution precisely reacts with the strong base solution.
In the titration process of strong acids with strong bases and vice versa, both solutions can be ionized completely. This is because the solution of strong acids and strong bases is included in the strong electrolyte solution which can be ionized completely in water. Thus, the salt created in this reaction has neutral properties.
Therefore, in the titration process of strong acids with strong bases the equivalent point is when the pH of the mixture is equal to 7 (neutral).
Strong base solution
is a base when dissolved in partially or water. all the molecules ionize into OH- ions.
The concept of Salt from strong acids and strong bases
This salt solution is neutral. For example, the neutralization reaction between NaOH and HCl produces a salt of NaCl. In water, fully ionized NaCl produces Na + and Cl- ions
NaOH (aq) + HCl (aq) = NaCl (aq) + H2O (l)
Neutral acid base
Strong strong
NaCl = Na + + Cl-
The Na + ion comes from a strong base and the Cl- ion also comes from a strong acid, so both of these ions are acidic and the Bronsted-Lowry base is weak so that both do not react with water (not hydrolyzed). Therefore the solution is neutral or pH = 7
Theory According to Bronsted-Lowry
Theory According to Bronsted-Lowry
Acids are donor protons, while bases are proton acceptors.
The acid-base theory from Arrhenius apparently cannot apply to all solvents, because it is specifically for water solvents. Likewise it is not suitable with the salting reaction because not all salts are neutral, but some are acidic and some are alkaline.
The concept of acid base is more commonly proposed by Johannes Bronsted, base is a substance that can receive protons. Ionization of hydrochloric acid in water is seen as the transfer of protons from acids to bases.
HCl + H 2 O -> H 3 O + + Cl -
Likewise the reaction between hydrochloric acid and ammonia, involves the transfer of protons from HCl to NH 3.
HCl + NH 3 ⇄ NH 4 + + Cl -
Ionization of weak acids can be described in the same way.
HOAc + H 2 O ⇄ H 3 O + + OAc -
In 1923 a British chemist named T.M. Lowry also proposed the same thing with Bronsted so his acid-base theory was called Bronsted-Lowry. It should be noted here that H + from acids combine with water molecules to form polyatomic ions H 3 O + called Hydronium ions. Common reactions that occur when acid is dissolved in water are:
HA + H 2 O ⇄ H 3 O + + A -
This presentation shows the great role of polar water molecules in attracting protons from acids.
Note that conjugate acids are formed if the proton still remains after the acid has lost one proton. Both are conjugate acid-base pairs consisting of two substances that are related to each other because of the proton administration or proton reception. However, acid-base dissociation is still used in Arrhenius, but the true meaning we must understand
Johannes N. Bronsted and Thomas M. Lowry prove that not all acids contain H + ions and not all bases contain OH - ions.
Bronsted - Lowry put forward the theory that acids are species that give H + (donor protons) and bases are species that accept H + (proton acceptors). If an acid gives an H + to a base molecule, then the rest will be the conjugate base of the original acid. Likewise, if the base receives H +, then the rest is the conjugate acid from the original base. Bronsted - Lowry's theory clearly shows the presence of Hydronium ions (H 3 O +) significantly.
HF is a pair of F - and H 2 O is a pair of H 3 O +. Water has ampiprotic properties because it can be as a base and can be as an acid.
HCl + H 2 O -> H 3 O + + Cl -
Alkaline Acid
NH 3 + H 2 O ⇄ NH 4 + + OH -
The benefits of the acid-base theory according to Bronsted - Lowry are as follows:
1. The application is not limited to water solvents, but to all solvents containing Hydrogen atoms and even without solvents.
2. Acids and bases are not only molecular, but can also be anions and cations.
Another example:
HAc (aq) + H 2 O (l) -> H 3 O + (aq) + Ac - (aq)
acid-1 base-2 acid-2 base-1
HAc with Ac - is a conjugate acid-base pair.
H 3 O + with H 2 O is the conjugate acid-base pair.
H 2 O (l) + NH 3 (aq) -> NH 4 + (aq) + OH - (aq)
acid-1 base-2 acid-2 base-1
H 2 O with OH - is a conjugate acid-base pair. NH 4 + with NH 3 is the conjugate acid-base pair.
In the example above it appears that water can be both acidic (donor proton) and basic (proton acceptor). Substances or ions or species like this are ampiprotic (amphoteric).
Acids are donor protons, while bases are proton acceptors.
The acid-base theory from Arrhenius apparently cannot apply to all solvents, because it is specifically for water solvents. Likewise it is not suitable with the salting reaction because not all salts are neutral, but some are acidic and some are alkaline.
The concept of acid base is more commonly proposed by Johannes Bronsted, base is a substance that can receive protons. Ionization of hydrochloric acid in water is seen as the transfer of protons from acids to bases.
HCl + H 2 O -> H 3 O + + Cl -
Likewise the reaction between hydrochloric acid and ammonia, involves the transfer of protons from HCl to NH 3.
HCl + NH 3 ⇄ NH 4 + + Cl -
Ionization of weak acids can be described in the same way.
HOAc + H 2 O ⇄ H 3 O + + OAc -
In 1923 a British chemist named T.M. Lowry also proposed the same thing with Bronsted so his acid-base theory was called Bronsted-Lowry. It should be noted here that H + from acids combine with water molecules to form polyatomic ions H 3 O + called Hydronium ions. Common reactions that occur when acid is dissolved in water are:
HA + H 2 O ⇄ H 3 O + + A -
This presentation shows the great role of polar water molecules in attracting protons from acids.
Note that conjugate acids are formed if the proton still remains after the acid has lost one proton. Both are conjugate acid-base pairs consisting of two substances that are related to each other because of the proton administration or proton reception. However, acid-base dissociation is still used in Arrhenius, but the true meaning we must understand
Johannes N. Bronsted and Thomas M. Lowry prove that not all acids contain H + ions and not all bases contain OH - ions.
Bronsted - Lowry put forward the theory that acids are species that give H + (donor protons) and bases are species that accept H + (proton acceptors). If an acid gives an H + to a base molecule, then the rest will be the conjugate base of the original acid. Likewise, if the base receives H +, then the rest is the conjugate acid from the original base. Bronsted - Lowry's theory clearly shows the presence of Hydronium ions (H 3 O +) significantly.
HF is a pair of F - and H 2 O is a pair of H 3 O +. Water has ampiprotic properties because it can be as a base and can be as an acid.
HCl + H 2 O -> H 3 O + + Cl -
Alkaline Acid
NH 3 + H 2 O ⇄ NH 4 + + OH -
The benefits of the acid-base theory according to Bronsted - Lowry are as follows:
1. The application is not limited to water solvents, but to all solvents containing Hydrogen atoms and even without solvents.
2. Acids and bases are not only molecular, but can also be anions and cations.
Another example:
HAc (aq) + H 2 O (l) -> H 3 O + (aq) + Ac - (aq)
acid-1 base-2 acid-2 base-1
HAc with Ac - is a conjugate acid-base pair.
H 3 O + with H 2 O is the conjugate acid-base pair.
H 2 O (l) + NH 3 (aq) -> NH 4 + (aq) + OH - (aq)
acid-1 base-2 acid-2 base-1
H 2 O with OH - is a conjugate acid-base pair. NH 4 + with NH 3 is the conjugate acid-base pair.
In the example above it appears that water can be both acidic (donor proton) and basic (proton acceptor). Substances or ions or species like this are ampiprotic (amphoteric).
Salt from Weak Acid with Strong Base
Salt from Weak Acid with Strong Base
Weak acids with weak bases can form total (perfect) hydrolyzed salts in water. Both cations and anions can be hydrolyzed in water. This salt solution can be acidic, basic, or neutral. This depends on the ratio of the strength of cations to anions in reaction with water.
Example
A weak HCN acid is mixed with a weak base, NH 3 will form NH 4 CN salt. HCN is partially ionized in water to form H + and CN - whereas NH 3 in water is partially ionized to form NH4 + and OH-. CN - base anions and NH 4 + acid cations can be hydrolyzed in water.
NH 4 CN (aq) → NH 4 + (aq) + CN - (aq)
NH 4 + (aq) + H 2 O → NH 3 (aq) + H 3 O (aq) +
CN - (aq) + H 2 O (e) → HCN (aq) + OH - (aq)
Salt from Weak Acid with Weak Bases
The nature of the solution depends on the relative strength of acids and their constituent bases (Ka and Kb)
If Ka <Kb (acid is weaker than base) the anion will be hydrolyzed more and the solution is basic.
if Ka> Kb (the acid is stronger than the base) the cation will be hydrolyzed more in an acidic solution.
If Ka = Kb (acid is as weak as base) the solution is neutral.
Examples of Salt Solution
Everyday life
salt and its use
Example Problem 1
The following are some examples along with solving problems related to salt hydrolysis that we have just studied together:
1. What is the pH of the solution of 100 mL 0.01 M sodium cyanide solution? (Head of HCN = 10-10)
Solution and Answers:
Sodium cyanide solution is formed from a mixture of strong bases (NaOH) with weak acids (HCN). Thus, the salt solution undergoes partial hydrolysis and is basic.
NaCN (aq) → Na + (aq) + CN– (aq)
Hydrolyzed ions are CN- ions. The concentration of CN ions is 0.01 M. Thus, the pH of the salt solution can be obtained through the following equation:
[OH-] = {(Kw / Ka) ([hydrolyzed ion])} 1/2
[OH-] = {(10-14 / 10-10) (0.01)} 1/2
[OH-] = 10-3 B
Thus, the pOH of the solution is 3. So, the pH of the salt solution is 11.
2. What is the pH of the solution of 200 mL of 0.1 M barium acetate solution? (Head CH3COOH = 2.10-5)
Solution and Answers:
Barium acetate solution is formed from a mixture of strong bases (Ba (OH) 2) with weak acids (CH3COOH). Thus, the salt solution undergoes partial hydrolysis and is basic.
BA (CH3COO) 2 (aq) → Ba + 2 (aq) + 2 CH3COO– (aq)
Hydrolyzed ions are CH3COO- ions. The CH3COO- ion concentration is 0.2 M. Thus, the pH of the salt solution can be obtained through the following equation:
[OH-] = {(Kw / Ka) ([hydrolyzed ion])} 1/2
[OH-] = {(10-14 / 2.10-5) (0.2)} 1/2
[OH-] = 10-5 billion
Thus, the pOH of the solution is 5. So, the pH of the salt solution is 9.
3. Calculate the pH of the NH4Cl 0.42 M solution! (NH4OH KB = 1.8.10-5)
Solution and Answers:
Ammonium chloride solution is formed from a mixture of weak bases (NH4OH) with strong acids (HCl). Thus, the salt solution undergoes partial hydrolysis and is acidic.
NH4Cl (aq) → NH4 + (aq) + Cl– (aq)
Hydrolyzed ions are NH4 + ions. The concentration of the NH4 + ion is 0.42 M. Thus, the pH of the salt solution can be obtained through the following equation:
[H +] = {(Kw / Kb) ([hydrolyzed ion])} 1/2
[H +] = {(10-14 / 1.8.10-5) (0.42)} 1/2
[H +] = 1,53.10-5 M
Thus, the pH of the salt solution is 4.82.
Example Problem 2
a.First try
Weigh 5.58 grams of table salt (NaCl)
Put salt in a beaker containing ml water, then stir
Put the kitchen salt solution into the measuring flask
Add water until the volume reaches 100 ml, then stir
b. Second try
Put the 3M HCl solution + water into the beaker
Then mix the HCL solution with 100 ml of 1M HCL
After that measure until the volume reaches 100 ml, then stir
Answers a & b
Conclusion
a. First conclusion
From observations and laboratory practices, our group was able to find out that, making a 100 ml NaCl 1M salt solution by dissolving 5.85 grams of salt + water to 100 ml volume. While from the results of this chemical practice, our group obtained concentration data from NaCl solution of 1M
b. Second conclusion
From laboratory observations and practices, our group was able to find out that, making a 100 ml 1M HCL solution by diluting a 33.33 ml HCL 3M + water solution to reach a 100 ml volume.
Suggestion
In practicing the making of salt solutions must be done seriously and thoroughly. Because, if the practicum is not careful or incorrect in calculating the mass, it will affect the process of making the solution. Therefore, in this practicum, it must be careful and thorough.
Example Problem 3
One way to obtain salt compounds is by reacting acids with alkaline substances. This reaction is known as a salting reaction or also called a neutralization reaction. In everyday life salt that is often used include: table salt (NaCl), English salt (MgSO4) as a laxative, baking soda (NaHCO3) as a bread developer, monosodium glutamate (MSG) as a flavor enhancer.
The nature of salt depends on the acid and base forming it. Salt that comes from the reaction between acid and base can be acidic, basic or neutral.
Salt that is acidic, has a pH <7, comes from the reaction between strong acids and weak bases. Example: NH4Cl (ammonium chloride / salmoniac), and NH4NO3 (ammonium nitrate).
Salt that is basic, has a pH> 7, comes from the reaction between a weak acid and a strong base. Examples: KNO2 (potassium nitrite), NaHCO3 (sodium bicarbonate / baking soda), NaCH3COO (sodium acetate), KCN (potassium cyanide / potassium), and KF (potassium phosphate).
Salt that is neutral, has a pH = 7, comes from strong acids and strong bases.
Example: NaCl (sodium chloride), KI (potassium iodide), and KNO3 (potassium nitrate).
salt, NaCl → Na + + Cl-
iron sulfate, Fe2 (SO4) 3 → 2Fe3 + + 3SO3-4
Weak acids with weak bases can form total (perfect) hydrolyzed salts in water. Both cations and anions can be hydrolyzed in water. This salt solution can be acidic, basic, or neutral. This depends on the ratio of the strength of cations to anions in reaction with water.
Example
A weak HCN acid is mixed with a weak base, NH 3 will form NH 4 CN salt. HCN is partially ionized in water to form H + and CN - whereas NH 3 in water is partially ionized to form NH4 + and OH-. CN - base anions and NH 4 + acid cations can be hydrolyzed in water.
NH 4 CN (aq) → NH 4 + (aq) + CN - (aq)
NH 4 + (aq) + H 2 O → NH 3 (aq) + H 3 O (aq) +
CN - (aq) + H 2 O (e) → HCN (aq) + OH - (aq)
Salt from Weak Acid with Weak Bases
The nature of the solution depends on the relative strength of acids and their constituent bases (Ka and Kb)
If Ka <Kb (acid is weaker than base) the anion will be hydrolyzed more and the solution is basic.
if Ka> Kb (the acid is stronger than the base) the cation will be hydrolyzed more in an acidic solution.
If Ka = Kb (acid is as weak as base) the solution is neutral.
Examples of Salt Solution
Everyday life
salt and its use
Example Problem 1
The following are some examples along with solving problems related to salt hydrolysis that we have just studied together:
1. What is the pH of the solution of 100 mL 0.01 M sodium cyanide solution? (Head of HCN = 10-10)
Solution and Answers:
Sodium cyanide solution is formed from a mixture of strong bases (NaOH) with weak acids (HCN). Thus, the salt solution undergoes partial hydrolysis and is basic.
NaCN (aq) → Na + (aq) + CN– (aq)
Hydrolyzed ions are CN- ions. The concentration of CN ions is 0.01 M. Thus, the pH of the salt solution can be obtained through the following equation:
[OH-] = {(Kw / Ka) ([hydrolyzed ion])} 1/2
[OH-] = {(10-14 / 10-10) (0.01)} 1/2
[OH-] = 10-3 B
Thus, the pOH of the solution is 3. So, the pH of the salt solution is 11.
2. What is the pH of the solution of 200 mL of 0.1 M barium acetate solution? (Head CH3COOH = 2.10-5)
Solution and Answers:
Barium acetate solution is formed from a mixture of strong bases (Ba (OH) 2) with weak acids (CH3COOH). Thus, the salt solution undergoes partial hydrolysis and is basic.
BA (CH3COO) 2 (aq) → Ba + 2 (aq) + 2 CH3COO– (aq)
Hydrolyzed ions are CH3COO- ions. The CH3COO- ion concentration is 0.2 M. Thus, the pH of the salt solution can be obtained through the following equation:
[OH-] = {(Kw / Ka) ([hydrolyzed ion])} 1/2
[OH-] = {(10-14 / 2.10-5) (0.2)} 1/2
[OH-] = 10-5 billion
Thus, the pOH of the solution is 5. So, the pH of the salt solution is 9.
3. Calculate the pH of the NH4Cl 0.42 M solution! (NH4OH KB = 1.8.10-5)
Solution and Answers:
Ammonium chloride solution is formed from a mixture of weak bases (NH4OH) with strong acids (HCl). Thus, the salt solution undergoes partial hydrolysis and is acidic.
NH4Cl (aq) → NH4 + (aq) + Cl– (aq)
Hydrolyzed ions are NH4 + ions. The concentration of the NH4 + ion is 0.42 M. Thus, the pH of the salt solution can be obtained through the following equation:
[H +] = {(Kw / Kb) ([hydrolyzed ion])} 1/2
[H +] = {(10-14 / 1.8.10-5) (0.42)} 1/2
[H +] = 1,53.10-5 M
Thus, the pH of the salt solution is 4.82.
Example Problem 2
a.First try
Weigh 5.58 grams of table salt (NaCl)
Put salt in a beaker containing ml water, then stir
Put the kitchen salt solution into the measuring flask
Add water until the volume reaches 100 ml, then stir
b. Second try
Put the 3M HCl solution + water into the beaker
Then mix the HCL solution with 100 ml of 1M HCL
After that measure until the volume reaches 100 ml, then stir
Answers a & b
Conclusion
a. First conclusion
From observations and laboratory practices, our group was able to find out that, making a 100 ml NaCl 1M salt solution by dissolving 5.85 grams of salt + water to 100 ml volume. While from the results of this chemical practice, our group obtained concentration data from NaCl solution of 1M
b. Second conclusion
From laboratory observations and practices, our group was able to find out that, making a 100 ml 1M HCL solution by diluting a 33.33 ml HCL 3M + water solution to reach a 100 ml volume.
Suggestion
In practicing the making of salt solutions must be done seriously and thoroughly. Because, if the practicum is not careful or incorrect in calculating the mass, it will affect the process of making the solution. Therefore, in this practicum, it must be careful and thorough.
Example Problem 3
One way to obtain salt compounds is by reacting acids with alkaline substances. This reaction is known as a salting reaction or also called a neutralization reaction. In everyday life salt that is often used include: table salt (NaCl), English salt (MgSO4) as a laxative, baking soda (NaHCO3) as a bread developer, monosodium glutamate (MSG) as a flavor enhancer.
The nature of salt depends on the acid and base forming it. Salt that comes from the reaction between acid and base can be acidic, basic or neutral.
Salt that is acidic, has a pH <7, comes from the reaction between strong acids and weak bases. Example: NH4Cl (ammonium chloride / salmoniac), and NH4NO3 (ammonium nitrate).
Salt that is basic, has a pH> 7, comes from the reaction between a weak acid and a strong base. Examples: KNO2 (potassium nitrite), NaHCO3 (sodium bicarbonate / baking soda), NaCH3COO (sodium acetate), KCN (potassium cyanide / potassium), and KF (potassium phosphate).
Salt that is neutral, has a pH = 7, comes from strong acids and strong bases.
Example: NaCl (sodium chloride), KI (potassium iodide), and KNO3 (potassium nitrate).
salt, NaCl → Na + + Cl-
iron sulfate, Fe2 (SO4) 3 → 2Fe3 + + 3SO3-4
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