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)