Assuming the maximum concentration of each solution is y mol/L
On mixing the solutions the volume of the concentration of each solution is reduced to half. After mixing the maximum concentration of each solution is
\( \dfrac{y}{2}\) mol/L.
Thus, [FeSO4]
= [Na2S] = \( \dfrac{y}{2}\)M
So, [Fe2+]
= [FeSO4] = \( \dfrac{y}{2}\) M
\( FeS(s) \leftrightarrow Fe^{2+}_{(aq)} + S^{2-}_{(aq)}\)
Ksp = \( [Fe^{2+}][S^{2-}] \)
\( =6.3×10^{−18}\)
\( = (\dfrac{y}{2})(\dfrac{y}{2})\dfrac{y^{2}}{4} \)
\( = 6.3\times 10^{-18}\)
Thus, y = \( 5.02\times 10^{-9}\)
Thus, if the concentration of FeSO4 and Na2SO4 are equal to or less than that of
\( 5.02\times 10^{-9}M\), then there won’t be precipitation of FeS.
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: FeSO4, MnCl2, ZnCl2 and CdCl2 . in which of these solutions precipitation will take place?
What is the minimum volume of water required to dissolve 1g of calcium sulphate at 298 K? (For calcium sulphate, Ksp is 9.1 × 10–6).
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 Ksp = 7.4 × 10–8 ).
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.