If 20 ml of 1·5 × 10^–5 M BaCl₂ solution is mixed with 40 ml of 0·9 × 10^–5MNa₂SO₄ solution, will a precipitate get formed? K_sp for BaSO₄ = 0·1 × 10^–10.

If 25.0 cm³ of 0.50 M - Ba(NO₃)₂ are mixed with 25·0 cm³ of 0·0220M-NaF, will any BaF₂ precipitate  [K_sp of Ba F₂ is 1·7 × 10^–6 at 298 K.]

Equal volumes of 0.002M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead precipitation of copper iodate? (For cupric iodate K_sp = 7·4 × 10^–8).

325.

The concentration of sulphide ion in 0·1M HCl solution saturated with hydrogen sulphide is 1·0 × 10^–19M. If 10 mL of this solution is added to 5 mL of 0·04M solution of FeSO₄, MnCl₂, ZnCl₂ and CaCl₂, in which solutions precipitation will take place? Given K_sp for FeS = 6·3 × 10^–18, MnS = 2·5 × 10^–13, ZnS =1·6 × 10^–24and CdS = 8·0 × 10^–27.

The values of K_sp of two sparingly soluble salts Ni(OH)₂ and AgCN are 2·0 × 10^–15 and 6 × 10^–17 respectively. Which salt is more soluble ? Explain

The solubility product constant of Ag₂CrO₄ and AgBr are 1·1 × 10^–12 and 5·0 × 10^–13 respectively. Calculate the ratio of the molarities of their saturated solutions.

Flow will you purify an impure sample of sodium chloride containing water soluble impurities?