Solubility Product and Common Ion Effect

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JEE Advanced 2025

LEVELJEE Advanced

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 $X \times 1 0^{- 6} mol dm^{- 3}$ . The value of $X$ is _______. Use: Solubility product constant ( $K_{s p}$ ) of barium iodate = $1.58 \times 1 0^{- 9}$

JEE Advanced 2020

LEVELJEE Advanced

An acidified solution of $0.05 M$ $Zn^{2 +}$ is saturated with $0.1 M$ $H_{2} S$ . What is the minimum molar concentration (M) of $H^{+}$ required to prevent the precipitation of $ZnS$ ? [Use $K_{sp} (ZnS) = 1.25 \times 1 0^{- 22}$ and Overall dissociation constant of $H_{2} S$ , $K_{NET} = K_{1} K_{2} = 1 \times 1 0^{- 21}$ ]

JEE Advanced 2023

LEVELJEE Advanced

On decreasing the pH from 7 to 2, the solubility of a sparingly soluble salt (MX) of a weak acid (HX) increased from $1 0^{- 4} mol L^{- 1}$ to $1 0^{- 3} mol L^{- 1}$ . The $p K_{a}$ of HX is:

JEE Advanced 2018

LEVELJEE Advanced

The solubility of a salt of weak acid(AB) at pH 3 is $Y \times 1 0^{- 3} mol L^{- 1}$ . The value of Y is_______. (Given that the value of solubility product of AB ( $K_{s p}$ ) = $2 \times 1 0^{- 10}$ and the value of ionization constant of HB( $K_{a}$ ) = $1 \times 1 0^{- 8}$ )

JEE Advanced 2022

LEVELJEE Advanced

Concentration of $H_{2} SO_{4}$ and $Na_{2} SO_{4}$ in a solution is $1 M$ and $1.8 \times 1 0^{- 2} M$ , respectively. Molar solubility of $PbSO_{4}$ in the same solution is $X \times 1 0^{- Y} M$ (expressed in scientific notation). The value of $Y$ is _________. [Given: Solubility product of $PbSO_{4}$ ( $K_{sp}$ ) = $1.6 \times 1 0^{- 8}$ . For $H_{2} SO_{4}$ , $K_{a 1}$ is very large and $K_{a 2} = 1.2 \times 1 0^{- 2}$ ]

JEE Advanced 2019

LEVELJEE Advanced

For the following reaction, the equilibrium constant $K_{c}$ at 298 K is $1.6 \times 1 0^{17}$ . $Fe^{2 +} (aq) + S^{2 -} (aq) ⇌ FeS(s)$ When equal volumes of 0.06 M $Fe^{2 +} (aq)$ and 0.2 M $S^{2 -} (aq)$ solutions are mixed, the equilibrium concentration of $Fe^{2 +} (aq)$ is found to be $Y \times 1 0^{- 17}$ M. The value of Y is ______.

To an aqueous solution containing ions such as $Al^{3 +}$ , $Zn^{2 +}$ , $Ca^{2 +}$ , $Fe^{3 +}$ , $Ni^{2 +}$ , $Ba^{2 +}$ and $Cu^{2 +}$ conc. $HCl$ , was added followed by $H_{2} S$ . The total number of cations precipitated during this reaction is/are

The solubility product of $Cr(OH)_{3}$ at $298 K$ is $6.0 \times 1 0^{- 31}$ . The concentration of hydroxide ions in a saturated solution of $Cr(OH)_{3}$ will be

(2.22 \times 1 0^{- 31})^{1/4}

(18 \times 1 0^{- 31})^{1/4}

(4.86 \times 1 0^{- 29})^{1/4}

(18 \times 1 0^{- 31})^{1/2}

The solubility of $Ca(OH)_{2}$ in water is [Given: The solubility product of $Ca(OH)_{2}$ in water = $5.5 \times 1 0^{- 6}$ ]

1.11 \times 1 0^{- 2}

1.11 \times 1 0^{- 6}

1.77 \times 1 0^{- 2}

1.77 \times 1 0^{- 6}

The solubility in water of a sparingly soluble salt $A B_{2}$ is $1.0 \times 1 0^{- 5} mol L^{- 1}$ . Its solubility product will be

4 \times 1 0^{- 15}

4 \times 1 0^{- 10}

1 \times 1 0^{- 15}

1 \times 1 0^{- 10}

Solubility of $Ca(OH)_{2}$ is $S mol L^{- 1}$ . The solubility product ( $K_{s p}$ ) under the same condition is

4 S^{3}

3 S^{4}

4 S^{2}

S^{3}

$A_{3} B_{2}$ is a sparingly soluble salt of molar mass $M$ (g mol $^{- 1}$ ) and solubility $x$ g L $^{- 1}$ . The solubility product satisfies $K_{s p} = a (\frac{x}{M})^{5}$ . The value of $a$ is ..........

The molar solubility (in $mol L^{- 1}$ ) of a sparingly soluble salt $MX_{4}$ is $S$ . The corresponding solubility product is $K_{s p}$ . $S$ is given in terms of $K_{s p}$ by the relation.

S = (\frac{K _{s p}}{128})^{1/4}

S = (\frac{K _{s p}}{256})^{1/4}

S = (\frac{K _{s p}}{256})^{1/5}

S = (\frac{K _{s p}}{128})^{1/5}

Solubility product of silver bromide is $5.0 \times 1 0^{- 13}$ . The quantity of potassium bromide (molar mass taken as $120 g mol^{- 1}$ ) to be added to $1 L$ of $0.05 M$ solution of silver nitrate to start the precipitation of $AgBr$ is

1.2 \times 1 0^{- 10} g

1.2 \times 1 0^{- 9} g

6.2 \times 1 0^{- 5} g

5.0 \times 1 0^{- 8} g

LEVELJEE Advanced

The solubility of $AgCN$ in a buffer solution of $pH = 3$ is $x$ . The value of $x$ is...... . [Assume : No cyano complex is formed; $K_{s p} (AgCN) = 2.2 \times 1 0^{- 16}$ and $K_{a} (HCN) = 6.2 \times 1 0^{- 10}$ ]

0.625 \times 1 0^{- 6}

1.6 \times 1 0^{- 6}

2.2 \times 1 0^{- 16}

1.9 \times 1 0^{- 5}

In a saturated solution of the sparingly soluble strong electrolyte $AgIO_{3}$ (molecular mass $= 283$ ) the equilibrium which sets in is $AgIO_{3} (s) ⇌ Ag^{+} (a q) + IO_{3}^{-} (a q)$ If the solubility product constant, $K_{s p}$ of $AgIO_{3}$ at a given temperature is $1.0 \times 1 0^{- 8}$ , what is the mass of $AgIO_{3}$ contained in $100 mL$ of its saturated solution?

28.3 \times 1 0^{- 2} g

2.83 \times 1 0^{- 3} g

1.0 \times 1 0^{- 7} g

1.0 \times 1 0^{- 4} g

The $K_{s p}$ for the following dissociation is $1.6 \times 1 0^{- 5}$ $P b C l_{2} (s) ⇌ P b^{2 +} (a q) + 2 C l^{-} (a q)$ Which of the following choices is correct for a mixture of 300 mL 0.134 M $P b (N O_{3})_{2}$ and 100 mL 0.4 M NaCl ?

Q < K_{s p}

Q > K_{s p}

Q = K_{s p}

Not enough data provided

LEVELJEE Advanced

An aqueous solution contains an unknown concentration of $Ba^{2 +}$ . When $50 mL$ of a $1 M$ solution of $Na_{2} SO_{4}$ is added, $BaSO_{4}$ just begins to precipitate. The final volume is $500 mL$ . The solubility product of $BaSO_{4}$ is $1 \times 1 0^{- 10}$ . What is the original concentration of $Ba^{2 +}$ ?

5 \times 1 0^{- 9} M

2 \times 1 0^{- 9} M

1.1 \times 1 0^{- 9} M

1.0 \times 1 0^{- 10} M

LEVELJEE Advanced

What is the molar solubility of $Al(OH)_{3}$ in $0.2 M NaOH$ solution? Given that, solubility product of $Al(OH)_{3} = 2.4 \times 1 0^{- 24}$

3 \times 1 0^{- 19}

12 \times 1 0^{- 21}

3 \times 1 0^{- 22}

12 \times 1 0^{- 23}

For the following Assertion and Reason, the correct option is Assertion (A) When Cu (II) and sulphide ions are mixed, they react together extremely quickly to give a solid. Reason (R) The equilibrium constant of $Cu^{2 +} (aq) + S^{2 -} (aq) ⇌ CuS (s)$ is high because the solubility product is low.

Both (A) and (R) are false.

Both (A) and (R) are true and (R) is the explanation for (A).

Both (A) and (R) are true but (R) is not the explanation for (A).

(A) is false and (R) is true.

If solubility product of $Z r_{3} (P O_{4})_{4}$ is denoted by $K_{s p}$ and its molar solubility is denoted by $S$ , then which of the following relation between $S$ and $K_{s p}$ is correct?

S = (\frac{K _{s p}}{144})^{1/6}

S = (\frac{K _{s p}}{6912})^{1/7}

S = (\frac{K _{s p}}{929})^{1/9}

S = (\frac{K _{s p}}{216})^{1/7}

The solubility product of a salt having general formula $M X_{2}$ , in water is $4 \times 1 0^{- 12}$ . The concentration of $M^{2 +}$ ions in the aqueous solution of the salt is

4.0 \times 1 0^{- 10}

1.6 \times 1 0^{- 4}

1.0 \times 1 0^{- 4}

2.0 \times 1 0^{- 6}

LEVELJEE Advanced

The stoichiometry and solubility product of a salt with the solubility curve given below is, respectively :

X_{2} Y, 2 \times 1 0^{- 9} M^{3}

X Y, 2 \times 1 0^{- 6} M^{3}

X Y_{2}, 1 \times 1 0^{- 9} M^{3}

X Y_{2}, 4 \times 1 0^{- 9} M^{3}

The molar solubility of $Zn(OH)_{2}$ in $0.1 M NaOH$ solution is $x \times 1 0^{- 18} M$ . The value of $x$ is ......... (Nearest integer) (Given; The solubility product of $Zn(OH)_{2}$ is $2 \times 1 0^{- 20}$ ).

LEVELJEE Advanced

The solubility of $CdSO_{4}$ in water is $8.0 \times 1 0^{- 4} mol L^{- 1}$ . Its solubility in $0.01 M H_{2} SO_{4}$ solution is ……… $\times 1 0^{- 6} mol L^{- 1}$ . (Round off to the nearest integer) (Assume that, solubility is much less than $0.01 M$ )