Which statement regarding the pH of aqueous solutions is correct?
At 318 K318\text{ K}318 K (where Kw=4.0×10−14 mol2 dm−6K_w = 4.0 \times 10^{-14}\text{ mol}^2\text{ dm}^{-6}Kw=4.0×10−14 mol2 dm−6), the pH of pure water is 7.007.007.00.
The pH of a 2.0×10−3 mol dm−32.0 \times 10^{-3}\text{ mol dm}^{-3}2.0×10−3 mol dm−3 solution of barium hydroxide, Ba(OH)2\text{Ba(OH)}_2Ba(OH)2, at 298 K298\text{ K}298 K is 11.6011.6011.60.
The pH of a 1.0×10−3 mol dm−31.0 \times 10^{-3}\text{ mol dm}^{-3}1.0×10−3 mol dm−3 solution of sulfuric acid, H2SO4\text{H}_2\text{SO}_4H2SO4, is 3.003.003.00 assuming complete dissociation.
Diluting a solution of hydrochloric acid with a pH of 5.005.005.00 by a factor of 100010001000 with pure water at 298 K298\text{ K}298 K results in a solution with a pH of 8.008.008.00.
77 exam-style questions on AQA A Level Chemistry Acids and bases (A-level only), covering Brønsted–Lowry acid–base equilibria in aqueous solution (A-level only), Definition and determination of pH (A-level only), The ionic product of water, $K_w$ (A-level only), Weak acids and bases $K_a$ for weak acids (A-level only), pH curves, titrations and indicators (A-level only), and Buffer action (A-level only). Each one has a worked solution and a mark scheme showing where the marks go.