\( CaSO_{4(s)}\leftrightarrow Ca^{2+}_{(aq)} + SO_{4}^{2-}(aq)\)

K_{sp} = \( [Ca^{2+}][SO_{4}^{2-}]\)

Assuming the solubility of calcium sulphate is x. So,

K_{sp} = x^{2}

\( \;9.1\times 10^{-6} = x^{2}\)

\( 9.1×10−6=x^2 \)

\( ∴ \;x = 3.02\times 10^{-3} mol/L\)

\( ∴x=3.02×10−3mol/L\)

Now, molecular mass os calcium sulphate is 136g/mol. Solubility in calcium sulphate in g/mol is

\( = 3.02\times 10^{-3} \times 136\)

\( =3.02×10−3×136\)

\( = 0.41 g/L\)

i.e. 1 litre H_{2}O will be required to dissolve 0.41g of calcium sulphate.Thus, minimum volume of H_{2}O required to dissolve 1 gram of CaSO_{4} at 298K is

=\( \dfrac{1}{0.41} L = 2.44 L\)

Answered by Abhisek | 1 year agoThe concentration of sulphide ion in 0.1M HCl solution saturated with hydrogen sulphide is 1.0 × 10^{–19} M. If 10 mL of this is added to 5 mL of 0.04M solution of the following: FeSO_{4}, MnCl_{2}, ZnCl_{2} and CdCl_{2} . in which of these solutions precipitation will take place?

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, Ksp = 6.3 × 10^{–18}).

The ionization constant of benzoic acid is 6.46 × 10^{–5} and Ksp for silver benzoate is 2.5 × 10^{–13}. How many times is silver benzoate more soluble in a buffer of pH 3.19 compared to its solubility in pure water?

Equal volumes of 0.002 M solutions of sodium iodate and cupric chlorate are mixed together. Will it lead to precipitation of copper iodate? (For cupric iodate K_{sp} = 7.4 × 10^{–8} ).

The solubility product constant of Ag_{2}CrO_{4} and AgBr are 1.1 × 10^{–12} and 5.0 × 10^{–13}, respectively. Calculate the ratio of the molarities of their saturated solutions.