At 25°C,the PH of water is 7.00.The standard enthalpy change of reaction of the autoionization of water 2H2O(l) converts into H3O+(aq) and OH-(aq) is  ∆H°RXN is 56.78 KJ/mol.calculate hydroxide ion concentration of pure water at 60°C?

(a) Using the expression Ka=[H+][A−]/[HA], explain how to determine which solution has the lower pH, 0.10MHF(aq) or 0.10MHC2H3O2(aq). Do not perform any numerical calculations. (b) Which solution has a higher percent ionization of the acid, a 0.10M solution of HC2H3O2(aq) or a 0.010M solution of HC2H3O2(aq) ? Justify your answer including the calculation of percent ionization for each solution.

A weak base has a base hydrolysis constant, Ko, of 3.1 × 106. What is the pH of a 0.11 M solution of the weak base? pH =

7 (a) Describe what happens when each of the following molecules is separately dissolved in water and illustrate with an equation in each case: (i) ethanoic acid (CH₂COOH) (ii) ammonia (NH3) (b) Identify the conjugate acids and bases in the substances mentioned in question 7(a) above. (c) Explain the difference between: (i) a strong acid and weak acid and (ii) a strong base and a weak base