Intext problems II — task. Science State Board, Class 10.

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What would be the pH of an aqueous solution of sulphuric acid which is $5\times10^{–5}$ $mol$ $litre^{–1}$ in concentration?

Sulphuric acid dissociates in water as:

Each mole of sulphuric acid gives of

$H^+$ ions in the solution. One litre of

$H_2SO_4$ solution contains

$5\times10^{–5}$ moles of

$H_2SO_4$ which would give

$2×5×10^{–5}=10×10^{–5}$ or

$1.0×10^{–4}$ moles of

$H^+$ ion in one litre of the solution.

Therefore,

$[H^+]=1.0×10^{–4}$

$mol$

$litre^{–1}$

$pH=–log_{10}[H^+]$

$= –log_{10}10^{–4}$

Did you find an error?

24. Intext problems II