A student titrates 20.0 cm³ of a metal hydroxide, M(OH)2, of concentration 0.060mol/dm³ with a strong acid of concentration 0.050mol/dm³. It requires 24.0cm³ of acid to neutralise the metal hydroxide.

1. (a)(i)Calculate the number of moles of acid in 24.0cm³ of the acid. moles[1]
2. (a)(ii)Calculate the number of moles of OH¯ ions in 20.0cm³ of the metal hydroxide. moles[1]
3. (a)(iii)Deduce whether the acid used is more likely to be hydrochloric acid or sulfuric acid. Explain your answer.[1]
4. (b)A student added excess calcium carbonate to 50 cm³ of 0.10mol/dm³ hydrochloric acid.
5. (b)(i)Construct an equation for the reaction of calcium carbonate with hydrochloric acid.[1]
6. (b)(ii)The volume of gas produced in the first 2 minutes is 24 cm³. Calculate the average rate of reaction over the first 2 minutes, in cm³/s. reaction rate = .cm³/s[1]
7. (b)(iii)The student repeats the experiment using 50 cm³ of 0.10mol/dm³ ethanoic acid. Use the kinetic particle theory to explain why the rate of reaction is slower with ethanoic acid than with hydrochloric acid.[3]