There are two solutions prepared. Solution P is $0.050\,\text{mol dm}^{-3}$ hydrochloric acid. Solution Q is $0.100\,\text{mol dm}^{-3}$ butanoic acid. A $2\,\text{cm}$ strip of magnesium ribbon is placed into $100\,\text{cm}^3$ of each solution. Effervescence is seen in both solutions, but it is quicker in solution P than it is in solution Q. Which statement best explains this observation?
- AMagnesium reacts with solution P to form a salt, but does not form a salt with solution Q.
- BMore particles are dissociated in solution P than are dissociated in solution Q.
- CSolution Q contains a stronger acid than solution P.
- DThe particles are closer together in solution Q than they are in solution P.