Acid Base Formulas

Evaluate the reactions involving Acid Base in a short span of time by accessing the Acid Base Formulae Collection. Have a grip on the fundamentals by making the most out of Acid Base Formula Sheet & Tables provided. You will feel the concept much more simple after applying these Formulae as a part of your work.

1. Basicity of Acid:

2. Water:
According to Arhenius & Bronsted-Lowry concept it is amphoteric, (Lewis base)

3. (a) Lewis Acid (electron pair acceptor):
CO₂, BF₃, AlCl₃, ZnCl₂, FeCl₃, PCl₃, PCl₅, SiCl₄, SF₆, normal cation

(b) Lewis Base (electron pair donor) :
NH₃, ROH, ROR, H₂O, RNH₂, R₂NH, R₃N, normal anion

4. Dissociation of weak Acid & Weak Base:
(a) Weak Acid:

(i) K_a = Cx²/(1 – x)
or K_a = Cx²

(ii) [H⁺] = basicity CX (C → M)
[H⁺] = CX (C → N)
[H⁺] = \(\sqrt{\mathrm{K}_{\mathrm{a}} \mathrm{C}}\) (C → M)

(b) Weak Base:
(i) K_b = Cx²/(1 – x)
or K_b = Cx²

(ii) [OH^–] = Acidity CX (C → M)
[OH^–] = CX (C → N)
[OH^–] = \(\sqrt{\mathrm{K}_{\mathrm{b}} \mathrm{C}}\) (C → M)
Note: For strong Acid & Strong Base X = 1

5. Other Formulas:

• Relative strength = \(\frac{\left[\mathrm{H}^{+}\right]_{1}}{\left[\mathrm{H}^{+}\right]_{2}}=\frac{\mathrm{Cx}_{1}}{\mathrm{Cx}_{2}}=\sqrt{\frac{\mathrm{K}_{\mathrm{a}_{1}}}{\mathrm{K}_{\mathrm{a}_{2}}}}\) (C → same)
• pH = – log [H⁺] = log \(\frac{1}{\left[\mathrm{H}^{+}\right]}\), [H⁺] = 10^-pH
• pOH = – log [OH^–] = log \(\frac{1}{\left[\mathrm{OH}^{-}\right]}\)
  & [OH^–] = 10^-pOH
• pH + pOH = 14
• Normality = Molarity × {Acidity or Basicity}

6. (a) Semi Normal = \(\frac{N}{2}\)
(b) Deci Normal = \(\frac{N}{10}\)
(c) Centi Normal = \(\frac{N}{100}\)
(d) Milli Normal = \(\frac{N}{1000}\)
(e) Penti Normal = \(\frac{N}{5}\)
(f) Penta Normal = 5N Deca Normal = 10 N
(g) Deca Normal = 10N

7. Buffer Solution:
(a) Acidic:

for Maximum Buffer Action

pH Range of Buffer

(b) Alkaline:

for max. buffer action

(c) Butter Capacity = \(\frac{\text { Mole/lit of Acid or Base Mixed }}{\text { change in } \mathrm{pH}}\)

8. Suitable Indicator for various type of titrations:

9. Important points:
(a) For conjugate acid – base pair
K_a.K_b = K_w
K_a.K_h = K_w
PK_a + pK_b = 14
PK_a + pK_h = 14

(b) In HF solvent even strong acid (eg. HNO₃) doen’t shows acidic behaviour because it has no tendency to accept protons.

(c) Necessary condidition for showing neutral colour of Indicator
pH = pKIn
or [HIn] = [In^–]
or [InOH] = [In⁺]

(d) Aqua Regia = 3HCl + HNO₃

(e) pH of Blood & Tears =7.4

(f) In acid rain there is a – SO₂

(g) pH of gasteric juice = 2 (of stomach)

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