IB Chemistry SL 3.1.5 Ion Product of Water Kw Questions

Use real SL exam questions to calculate hydroxide concentration from Kw and classify solutions as acidic, neutral or basic.

Exam points

Use Kw = [H3O+][OH−] to calculate hydroxide concentration from pH or hydronium concentration, retaining powers of ten and mol dm−3 units.
Recognize acidic, neutral and basic solutions by comparing [H+] and [OH−] at the stated temperature, including pure-water conditions.

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Study 3.1.5—Ion product of water (Kw) conceptsOpen the corresponding Concept lesson for explanations, examples and exam connections.

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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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IB Chemistry SL 3.1.5 Ion Product of Water Kw Questions question 1