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).

324. What is the maximum concentration of equimolar solutions of ferrous sulphate and sodium sulphide so that when mixed in equal volumes, there is no precipitation of iron sulphide? (For iron sulphide, K_sp = 6·3 × 10^–18).

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?