Question

Each of the insoluble salts below are put into 0.10 M hydrobromic acid solution. Do you expect their solubility to be more, less, or about the same as in a pure water solution? Clear All More soluble than in pure lead bromide water Similar solubility as in calcium carbonate pure water Less soluble than in pure nickel(II) hydroxide water

Answer 1

Part- A.  

Solubility of lead bromide decreases in 0.10 M hydrobromic acid solution. This is due to the common ion effect which causes the equilibrium to be shifted towards backward direction. Therefore solubility of the insoluble lead bromide decreases ( Le Chatelier's Principle).

In case of calcium carbonate and nickel (II) hydroxide opposite result obtained, i.e the solubility of the insoluble salt s increases in 0.10 M hydrobromic acid. This can be explained on the basis of un- common ion effect. Un- common ion increses the ionic strength of the solution and also increases the interionic attraction. Therefore more reactant dissolved in the solution and hence solubility increases.

Part-B

In case of nickel (II) sulfates and barium fluoride, solubility increases in 0.10 M hydrochloric acid than pure water due to uncommon ion effect.

But in case of lead chloride, solubility decreases in 0.10 M hydrochloric acid than pure water due to commom ion effect.