Solubility product

At 300 K, the molar conductivities of the aqueous solutions of three salts at two different concentrations are given below:

Salt	Concentration (M)	Molar conductivity (S cm$^2$ mol$^{-1}$)
$\ce{NaNO3}$	0.01	111
	0.04	101
$\ce{NaCl}$	0.01	117
	0.04	107
$\ce{AgNO3}$	0.01	125
	0.04	116

The conductivity of a saturated aqueous solution of AgCl is $1.40\times10^{-6}$ S cm$^{-1}$ at 300 K. If the solubility of AgCl in water at 300 K is X mol L$^{-1}$, then $\log_{10}(X^{-1})$ is

(Assume that AgCl dissolved in water ionizes completely and that the molar conductivity of saturated AgCl solution is equal to its limiting molar conductivity.)

The solubility product constants of $\ce{Ag2CrO4}$ and AgBr are $32x$ and $4y$ respectively at 298 K. The value of $\left(\dfrac{\text{molarity of }\ce{Ag2CrO4}}{\text{molarity of AgBr}}\right)$ can be expressed as :

$\ce{M3A2}$ is a sparingly soluble salt of molar mass $y$ g mol$^{-1}$ and solubility $x$ g L$^{-1}$. The ratio of the molar concentration of the anion ($\ce{A^{3-}}$) to the solubility product of the salt is

Consider the following data.

Electrolyte	$\Lambda^\circ_m$ (S cm² mol$^{-1}$)
$\ce{BaCl2}$	$x_1$
$\ce{H2SO4}$	$x_2$
HCl	$x_3$

$\ce{BaSO4}$ is sparingly soluble in water. If the conductivity of the saturated $\ce{BaSO4}$ solution is $x$ S cm$^{-1}$ then the solubility product of $\ce{BaSO4}$ can be given as

(Here $\Lambda_m=\Lambda^\circ_m$)

The solubility of barium iodate in an aqueous solution prepared by mixing 200 mL of 0.010 M barium nitrate with 100 mL of 0.10 M sodium iodate is $\boldsymbol{X}\times10^{-6}\ \mathrm{mol\,dm^{-3}}$. The value of $\boldsymbol{X}$ is _____.

Use: Solubility product constant ($K_{sp}$) of barium iodate $= 1.58\times10^{-9}$

On decreasing the $p\mathrm{H}$ from 7 to 2, the solubility of a sparingly soluble salt (MX) of a weak acid (HX) increased from $10^{-4}\,\mathrm{mol\,L^{-1}}$ to $10^{-3}\,\mathrm{mol\,L^{-1}}$. The $pK_\mathrm{a}$ of HX is

Concentration of $\ce{H2SO4}$ and $\ce{Na2SO4}$ in a solution is 1 M and $1.8 \times 10^{-2}$ M, respectively. Molar solubility of $\ce{PbSO4}$ in the same solution is $X \times 10^{-Y}$ M (expressed in scientific notation). The value of $Y$ is ________.

[Given: Solubility product of $\ce{PbSO4}$ $(K_{sp}) = 1.6 \times 10^{-8}$. For $\ce{H2SO4}$, $K_{a1}$ is very large and $K_{a2} = 1.2 \times 10^{-2}$]

The $K_{sp}$ for bismuth sulphide ($\mathrm{Bi_2S_3}$) is $1.08\times10^{-73}$. The solubility of $\mathrm{Bi_2S_3}$ in mol L$^{-1}$ at 298 K is

The solubility product of a sparingly soluble salt $\mathrm{A_2X_3}$ is $1.1\times10^{-23}$. If specific conductance of the solution is $3\times10^{-5}$ S m$^{-1}$, the limiting molar conductivity of the solution is $x\times10^{-3}$ S m$^2$ mol$^{-1}$. The value of $x$ is ______.

The solubility of AgCl will be maximum in which of the following ?

At 310 K, the solubility of $\mathrm{CaF_2}$ in water is $2.34\times10^{-3}$ g/100 mL. The solubility product of $\mathrm{CaF_2}$ is ______ $\times10^{-8}$ (mol/L)$^3$. (Give molar mass : $\mathrm{CaF_2}$ = 78 g mol$^{-1}$)

If the solubility product of PbS is $8\times10^{-28}$, then the solubility of PbS in pure water at 298 K is $x\times10^{-16}$ mol L$^{-1}$. The value of $x$ is _______. (Nearest Integer)

[Given : $\sqrt2$ = 1.41]

The value of $|\mathbf y|$ is ____.

An acidified solution of 0.05 M $\ce{Zn^{2+}}$ is saturated with 0.1 M $\ce{H2S}$. What is the minimum molar concentration (M) of $\ce{H+}$ required to prevent the precipitation of ZnS?

Use $K_{sp}(\ce{ZnS}) = 1.25\times10^{-22}$ and overall dissociation constant of $\ce{H2S}$, $K_{\text{NET}} = K_1K_2 = 1\times10^{-21}$.

For the following reaction, the equilibrium constant $K_c$ at 298 K is $1.6\times10^{17}$.

$$\ce{Fe^{2+}(aq) + S^{2-}(aq) <=> FeS(s)}$$

When equal volumes of 0.06 M $\ce{Fe^{2+}}(aq)$ and 0.2 M $\ce{S^{2-}}(aq)$ solutions are mixed, the equilibrium concentration of $\ce{Fe^{2+}}(aq)$ is found to be $Y\times10^{-17}$ M. The value of $Y$ is ______

The solubility of a salt of weak acid (AB) at pH 3 is $\mathbf Y\times10^{-3}$ mol L⁻¹. The value of Y is ______.

(Given that the value of solubility product of AB ($K_{sp}$) = $2\times10^{-10}$ and the value of ionization constant of HB ($K_a$) = $1\times10^{-8}$)

Dilution processes of different aqueous solutions, with water, are given in LIST-I. The effects of dilution of the solutions on $[\mathrm{H^+}]$ are given in LIST-II.

(Note: Degree of dissociation ($\alpha$) of weak acid and weak base is $\ll 1$; degree of hydrolysis of salt $\ll 1$; $[\mathrm{H^+}]$ represents the concentration of $\mathrm{H^+}$ ions)

Match each process given in LIST-I with one or more effect(s) in LIST-II. The correct option is

Zirconium phosphate $\ce{[Zr3(PO4)4]}$ dissociates into three zirconium cations of charge +4 and four phosphate anions of charge −3. If molar solubility of zirconium phosphate is denoted by S and its solubility product by $K_{sp}$ then which of the following relationship between S and $K_{sp}$ is correct ?

The $K_{sp}$ of $\ce{Ag2CrO4}$ is $1.1\times10^{-12}$ at 298 K. The solubility (in mol/L) of $\ce{Ag2CrO4}$ in a 0.1 M $\ce{AgNO3}$ solution is

The solubility product ($K_{sp}$; mol³ dm⁻⁹) of $\ce{MX2}$ at 298 K based on the information available for the given concentration cell is (take $2.303\times R\times298/F=0.059$ V)