Strong acid calculations are really easy if you learn them the right way. This post gives you notes on how to do the calculations for A-level chemistry and includes worked examples for both monoprotic/monobasic and diprotic/dibasic strong acids.

[convertkit form=1956159]

## Strong acid calculations for A level Chemistry

For all pH calculations, learn these equations and symbols:

**pH = -log[H+ ]** (remember to give pH to 2 d.p.) and **[H+ ] = 10- pH[H+ ]** = the concentration of protons

**[HA]**= the concentration of the acid

**[A- ]** = the concentration of the conjugate base

**Monoprotic strong acids**: Fully dissociate in aqueous solution

∴ [H+ ] = [HA] + –

e.g. HCl → H + Cl

If the concentration of HCl is 0.5 mol dm- 3 the concentration of H+ will also be 0.5 mol dm -3.

**How to calculate the pH of a strong acid:**

Because [H +] = [HA], the calculation becomes **pH = -log[HA]**e.g. Calculate the pH of a solution of HCl with a concentration of 0.250 mol dm -3

pH = -log 0.250 = 0.60 (2 dp)

**How to calculate the concentration [HA] of a strong acid:**

Because [H +] = [HA], the calculation becomes **[** **HA] = 10 ****-pH**e.g. Calculate the concentration of a solution of HCl with a pH of 0.89.

[HA] = 10- 0.89 = 0.129 mol dm -3

**Diprotic Strong acids**

Fully dissociate in aqueous solution. 1 mol of acid dissociates to give 2 moles of protons. ∴ [ H + ] = 2[HA]

e.g. H_{2}SO_{4} → 2H + + SO_{4}^{2-}

If the concentration of H_{2}SO_{4} is 0.5 mol dm-3 the concentration of H+ will be

1.0 mol dm- 3 .

**How to calculate the pH of a dibasic strong acid**

**pH = -log[H****+**** ]**** **, so first you need to calculate [H + ]: **[** **H****+**** ]**** ****= 2 x [HA]**e.g Calculate the pH of a solution of H2 SO4 with a concentration of 0.400 mol dm- 3 [H+ ] = 2 x 0.400 = 0.800 mol dm -3

Then, pH = -log 0.800 = 0.10 (2 dp)

**How to calculate the concentration of a dibasic strong acid:**

You’ll be given pH, so calculate [H + ]: **[H ****+****]**** ****= 10****–**** ****pH **Then, since [H+ ] = 2[HA], **[HA] = [H ****+****]**** ** ** ****2**

e.g. Calculate the concentration of a solution of H2 SO4 w ith a pH of 0.75. [H+ ] = 10 -0.75 = 0.179 mol dm -3

Then, [HA] = 0.179 ** **0.0895 mol dm- 3

## Test your knowledge

Take the acids, bases and buffers multiple choice questions quiz to test your knowledge of the strong acid calculations for A level chemistry.