The 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 0.04 M solution of the following: FeSO₄, MnCl₂, ZnCl2 and CdCl₂. in which of these solutions precipitation will take place?

Question

For the reaction \( \mathrm{N_2} + 3\mathrm{H_2} \rightleftharpoons 2\mathrm{NH_3} \), the equilibrium constant \(K_c\) is 0.5 at a certain temperature. If initially, 1 mole of \(\mathrm{N_2}\) and 3 moles of \(\mathrm{H_2}\) are placed in a 1 L container, what is the equilibrium concentration of \(\mathrm{NH_3}\)?

Answer 1

S^{2-} = 10^{-19}}{15} = 6.67 * 10^{-20} M

M^{2+} = {5 * 0.04}{15} = 0.0133 M

Ksp and Q Check

Compound	Ksp	Q = [M²⁺][S²⁻]	Ppt?
FeS	\( 4.9 \times 10^{-19} \)	\( 8.9 \times 10^{-22} \)	No
MnS	\( 2.5 \times 10^{-10} \)	\( 8.9 \times 10^{-22} \)	No
ZnS	\( 2 \times 10^{-25} \)	\( 8.9 \times 10^{-22} \)	Yes
CdS	\( 8 \times 10^{-27} \)	\( 8.9 \times 10^{-22} \)	Yes

Precipitation in ZnCl₂ and CdCl₂.

The 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 0.04 M solution of the following: FeSO₄, MnCl₂, ZnCl2 and CdCl₂. in which of these solutions precipitation will take place?

Solution and Explanation

Ksp and Q Check

Top Questions on Law Of Chemical Equilibrium And Equilibrium Constant

The 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 0.04 M solution of the following: FeSO4, MnCl2, ZnCl2 and CdCl2. in which of these solutions precipitation will take place?

Solution and Explanation

Ksp and Q Check

Top Questions on Law Of Chemical Equilibrium And Equilibrium Constant

The 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 0.04 M solution of the following: FeSO₄, MnCl₂, ZnCl2 and CdCl₂. in which of these solutions precipitation will take place?