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 ▸Alcohols can be converted into alkenes by removing water. The alcohol 3-methylpent-2-ol forms a mixture of organic products when dehydrated. Describe the conditions of this reaction. Name all the organic products.
Unsaturated fats change bromine water from orange to colourless. How?
The shape around the oxygen atom in butan-2-ol is non linear. Predict the shape and angle of the C-O-H bond giving explanations
Explain, with reference to the electronic transitions involved, how characteristic flame colours of metal ions are formed and why the flame colours are different.