Solubility Product

Q.

Why is water called the universal solvent?

Q.

Question 2.27

If the solubility product of CuS is $6\times {10}^{-6}$, calculate the maximum molarity of CuS in aqueous solution.

Q. pH of a saturated solution of $Ca(OH{)}_2$ is 9. The solubility product (Ksp) of $Ca(OH{)}_2$ is:

1. $0.5\times {10}^{-15}$
2. $0.25\times {10}^{-10}$
   
3. $0.125\times {10}^{-15}$
4. $0.5\times {10}^{-10}$

Q. The solubility of $AgCl$ in water at $298K$ is $1.06\times {10}^{-5}$ mole per litre. Calculate its solubility product at this temperature.

1. $1.12\times {10}^{-10}mo{l}^2{L}^{-2}$
2. $1.12\times {10}^{-10}mo{l}^{-2}{L}^2$
3. $1.12\times {10}^{10}mo{l}^{-2}{L}^2$
4. $1.12\times {10}^{10}mo{l}^2{L}^{-2}$

Q. What is the pH of a 0.5 M aqueous NaCN solution ? ${\text{pK}}_{\text{b}}\text{of}{\text{CN}}^{-}$ is 4.70.

1. 5.5
2. 7
3. 14
4. 11.5

Q. At ${25}^{\circ }C,$ the solubility product of $Mg(OH{)}_2$ is $1.0\times {10}^{-11}$. At which $pH$, will $M{g}^{2+}$ ions start precipitating in the form of $Mg(OH{)}_2$ from a solution of $0.001MM{g}^{2+}$ ions?

1. 9
2. 10
3. 11
4. 8

Q. The $K_{sp}ofA{g}_{2}Cr{O}_{4}is1.1\times {10}^{-12}at298K.$ The solubility (in $mol/L$) of $A{g}_{2}Cr{O}_4$ in a $0.1MAgN{O}_3$ solution is

1. $1.1\times {10}^{-11}$
2. $1.1\times {10}^{-10}$
3. $1.1\times {10}^{-12}$
4. $1.1\times {10}^{-9}$

Q. The solubility of a salt of weak acid (AB) at pH= 3 is $Y\times {10}^{-3}mol{L}^{-1}$. The value of Y is.
(Given that the value of solubility product of AB $\left(K_{sp}\right)=2\times {10}^{-10}$ and the value of ionization constant of $HB\left(K_a\right)=1\times {10}^{-8})$

Q.

Solubility of $\mathrm{AgCN}$ buffer solution has a $\mathrm{pH}=3$ is $\mathrm{X}$.What is the value of $\mathrm{X}$? Assume no Cyano is formed ${\mathrm{K}}_{\mathrm{sp}}=\left(\mathrm{AgCN}\right)=2.2\times {10}^{-16}$ and ${\mathrm{K}}_{\mathrm{a}}\left(\mathrm{HCN}\right)=6.2\times {10}^{-10}$

Q. pH of a saturated solution of $Ba(OH{)}_2$ is 12. The value of solubility product $\left(K_{sp}\right)ofBa(OH{)}_2$ is

1. $3.3\times {10}^{-7}$
2. $5.0\times {10}^{-7}$
3. $4.0\times {10}^{-6}$
4. $5.0\times {10}^{-6}$

Q. What is hydration enthalpy?

Q. An aqueous solution of glucose $\left(C_6{H}_{12}{O}_6\right)$ is labelled as $10\%\text{w/V}$. Calculate the volume in which $1$ mole of glucose will be dissolved.

1. $1\text{L}$
2. $3.6\text{L}$
3. $1.8\text{L}$
4. $0.9\text{L}$

Q.

What is the minimum volume of water required to dissolve 1g of calcium sulphate at 298 K? (For calcium sulphate, $K_{sp}$ is $9.1\times {10}^{-6}$).

Q. The solubility product of a sparingly soluble salt $A{X}_2$ is $3.2\times {10}^{-11}.$ The value $s^3$ $\left(inmol{L}^{-1}\right)$ is:
where s = solubility

1. $2\times {10}^{-8}$
2. $4\times {10}^{-8}$
3. $4\times {10}^{-13}$
4. $8\times {10}^{-12}$

Q. Solubility product of silver bromide is $5.0\times {10}^{-13}$. The quantity of potassium bromide (molar mass is 120 gmol${}^{-1})$ to be added to 1 litre of $0.05M$ solution of silver nitrate to start the precipitation of $AgBr$ is:

1. $1.2\times {10}^{-10}g$
2. $1.2\times {10}^{-9}g$
3. $5.0\times {10}^{-8}g$
4. $6.2\times {10}^{-5}g$

Q.

What is the molar solubility (s) of ${\mathrm{Ba}}_3{\left({\mathrm{PO}}_4\right)}_2$ in terms of ${\mathrm{K}}_{\mathrm{sp}}$?

Q. At $310K$, the solubility of $Ca{F}_2$ in water is $2.34\times {10}^{-3}g/100mL$. The solubility product of $Ca{F}_2$ is $\times {10}^{-8}{\left(mol/L\right)}^3$
(Given molar mass: $Ca{F}_2=78gmo{l}^{-1}$)

Q. Solubility of AgCl in water 0.01M $CaC{l}_2$, 0.01M NaCl and 0.05M $AgN{O}_3$ are $S_1,S_2,S_3$ and $S_4$ respectively then $(K_{sp}AgCl={10}^{-10}{M}^2)$

1. > > >
2. > > >
3. > = >
4. > > <

Q.

$K_{sp}Mg(OH{)}_2$ is $4.0\times {10}^{-12}$. The number of moles of $M{g}^{2+}$ ions in one litre of its saturated solution in 0.1 M NaOH is :

1. $8.0\times {10}^{-6}$

2. $1.0\times {10}^{-4}$

3. $4.0\times {10}^{-10}$

4. $2.0\times {10}^{-6}$

Q.

What role does lattice energy play in the stability of ionic compounds?

Q. $M(OH{)}_x$ has $K_{sp}=4\times {10}^{-12}$ and solubility $={10}^{-4}M$ . Then the value of $x$ is:

1. 1
2. 2
3. 3
4. 4

Q.

The dissociation constant of a weak acid is $1.0\times {10}^{-5}$. The equilibrium

constant for the reaction with strong base is

1. 1.0 x 10^-5

2. 1.0 x 10^-9

3. 1.0 x 10⁹

4. 1.0 x 10¹⁴

Q. The molar solubility of $Cd(OH{)}_2$ is $1.84\times {10}^{-5}M$ in water. The expected solubility of $Cd(OH{)}_2$ in a buffer solution of $pH=12$ is:

1. $1.84\times {10}^{-9}M$
2. $2.49\times {10}^{-}M$
3. $6.23\times {10}^{-11}M$
4. $2.49\times {10}^{-10}M$

Q. The solubility of $lead\left(II\right)iodide$ is $0.064g/100mL$ at ${25}^{o}C.$ What is its solubility product?

1. $2.08\times {10}^{-8}mo{l}^{-3}{L}^3$
2. $0.17\times {10}^{-8}mo{l}^{-3}{L}^3$
3. $3.5\times {10}^{-8}mo{l}^3{L}^{-3}$
4. $1.07\times {10}^{-8}mo{l}^3{L}^{-3}$

Q.

The ratio of water of crystallization present in Mohr’s salt to that of Potash alum is$\dots \dots ..x{10}^{-1}$

Q. Ionic conductance of H+ and So4_ are x and y cms^- . Find the equivalent conductance of HSO4 1] 2x+ y/2 2] x+y/2 3] x/2+y 3]x/2 +y/2

Q. Solubility product constant ($K_{sp}$) of salts of types MX, $M{X}_2$ and $M_{3}X$ at temperature 'T' are $4.0\times {10}^{-8},3.2\times {10}^{-14}$ and $2.7\times {10}^{-15},$ respectively. Solubilities (mol $d{m}^{-3}$) fo the salts at temperature 'T' are in the order

1. $MX>M{X}_2>M_{3}X$
2. $M_{3}X>M{X}_2>MX$
3. $M{X}_2>M_{3}X>MX$
4. $MX>M_{3}X>M{X}_2$

Q. When equal volumes of the following solutions are mixed, precipitation of $AgCl$ ($K_{sp}=1.8\times {10}^{-10}$) will occur only with:

1. ${10}^{-4}MA{g}^{+}$ and ${10}^{-4}MC{l}^{-}$
2. ${10}^{-5}MA{g}^{+}$ and ${10}^{-5}MC{l}^{-}$
3. ${10}^{-6}MA{g}^{+}$ and ${10}^{-6}MC{l}^{-}$
4. ${10}^{-10}MA{g}^{+}$ and ${10}^{-10}MC{l}^{-}$

Q. The solubility product of $A_2{X}_3$ is $1.08\times {10}^{-23}$, its solubility will be:

1. $1\times {10}^{-3}$
2. $1\times {10}^{-6}$
3. $1\times {10}^{-5}$
4. $1\times {10}^{-4}$

Q. The standard electrode potential values, $E^o$, for $A{l}^{3+}/Al$ and $T{l}^{3+}/Tl$ are $-1.66\text{V}$ and $+1.26\text{V}$ respectively. Select the correct statement.

1. Aluminium has a high tendency to form $A{l}^{3+}$ as compared to thallium
2. $T{l}^{3+}$ is a powerful reducing agent
3. Thallium is more electropositive than aluminium
4. Thallium has a high tendency to form $T{l}^{3+}\left(aq\right)$ as compared to Aluminium