The ionic product of water, Kw = 2.93 × 10−15 mol dm−6 at 10 °C. Calculate the pH of a 0.0131 mol dm−3 solution of calcium hydroxide at 10 °C Give your answer to two decimal places.
[OH-] = 0.0262 mol dm-3[H+] = (Kw/[OH-]) = 2.93 x 10−15 / 0.0262 (= 1.118 x 10−13) pH = (− log (1.118 x 10−13) = 12.9514 = 12.95
WB
Related Chemistry A Level answers
All answers ▸What is Ionisation Energy and the three factors that affect it? 2)State and explain the general trend in first ionisation energies for the Period 3 elements.
Would you expect a calcium ion to be bigger, smaller or the same size as a calcium atom? Give TWO reasons to explain your answer.
Define the standard enthalpy of formation
Predict whether the lattice energy of magnesium oxide, MgO, is more or less exothermic than the lattice energy of magnesium sulfide, MgS. Justify your answer in terms of the sizes and the charges of the ions involved.