IB Chemistry SL Reactivity 3.1.5 Ion Product of Water

Practise applying Kw = [H⁺][OH⁻] to aqueous solutions at a stated temperature. Calculate the missing ion concentration, compare [H⁺] with [OH⁻] to classify the solution and avoid…

Exam points

use Kw to calculate [H⁺] or [OH⁻] from the other aqueous ion concentration
classify a solution by comparing hydrogen- and hydroxide-ion concentrations
calculate neutral pH from equal ion concentrations using the stated temperature-dependent Kw

[Maximum number: 1]

Soluble acids and bases ionize in water.

A solution containing 0.510 g of an unknown monoprotic acid, HA , was titrated with $0.100 \mathrm{~mol} \mathrm{dm}^{-3} \mathrm{NaOH}(\mathrm{aq}) .25 .0 \mathrm{~cm}^{3}$ was required to reach the equivalence point.

Calculate $\left[\mathrm{H}^{+}\right]$ in the NaOH solution.

$1.00\times10^{-14}=[\mathrm{H^+}]\times0.100$ $[\mathrm{H^+}]=1.00\times10^{-13}\ \mathrm{mol\ dm^{-3}}$

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3.1.5—Ion product of water (Kw) question 1