On adding 0.1, M solution each of [Ag^+], [Ba^{2+}], [Ca^{2+}] in a Na₂SO₄ solution, species fir

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6-2.Equilibrium-II (Ionic Equilibrium)

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On adding $0.1\, M$ solution each of $[Ag^+], [Ba^{2+}], [Ca^{2+}]$ in a $Na_2SO_4$ solution, species first precipitated is $[K_{sp}\, BaSO_4 = 10^{-11}, K_{sp}\, CaSO_4 = 10^{-6}, K_{sp}\,Ag_2SO_4 = 10^{-5}]$

$Ag_2SO_4$

$BaSO_4$

$CaSO_4$

All of these

(AIIMS-2008)

Solution

The species having minimum value of $K_{sp}$ will get precipitated first of all because ionic product will exceed the solubility product of such a species. The $K_{sp}$ value is minimum for $BaSO_4(10^{-11})$, so, $BaSO_4$ will get precipitated first of all.

Standard 11

Chemistry

Solubility of $B(OH)_2$ in water at $25\,^oC$ is $10^{-7}\ M$ . The value nearest to $K_{sp}$ is

normal

The solubility product of a salt having general formula $M{X_2},$ in water is : $4 \times {10^{ – 12}}$. The concentration of ${M^{2 + }}$ ions in the aqueous solution of the salt is

medium

(AIEEE-2005)

The solubility of $Ba_3(AsO_4)_2$ (molar mass $= 690$) is $6.9 \times 10^{-2} \,g/100\, mL$. What is the value of its $K_{sp}$?

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Solubility of $AgCl$ in $0.2\,M\, NaCl$ is $x$ and that in $0.1\, M\, AgNO_3$ is $y$ then which of the following is correct ?

medium

At $298$ $K$ temp. the ${K_{sp}}$ of $Ca{F_2}$ is $1.7 \times {10^{ – 10}}$. One person daily drinks $2.5$ $L$ saturated water by $Ca{F_2}$ . Then how much gram $Ca{F_2}$ present in his body? (Molecular mass of $Ca{F_2}$ is $ 78$ $g$ $mol^{-1}$ )

medium

On adding $0.1\, M$ solution each of $[Ag^+], [Ba^{2+}], [Ca^{2+}]$ in a $Na_2SO_4$ solution, species first precipitated is $[K_{sp}\, BaSO_4 = 10^{-11}, K_{sp}\, CaSO_4 = 10^{-6}, K_{sp}\,Ag_2SO_4 = 10^{-5}]$

Solution

Similar Questions

Solubility of $B(OH)_2$ in water at $25\,^oC$ is $10^{-7}\ M$ . The value nearest to $K_{sp}$ is

The solubility product of a salt having general formula $M{X_2},$ in water is : $4 \times {10^{ – 12}}$. The concentration of ${M^{2 + }}$ ions in the aqueous solution of the salt is

The solubility of $Ba_3(AsO_4)_2$ (molar mass $= 690$) is $6.9 \times 10^{-2} \,g/100\, mL$. What is the value of its $K_{sp}$?

Solubility of $AgCl$ in $0.2\,M\, NaCl$ is $x$ and that in $0.1\, M\, AgNO_3$ is $y$ then which of the following is correct ?

At $298$ $K$ temp. the ${K_{sp}}$ of $Ca{F_2}$ is $1.7 \times {10^{ – 10}}$. One person daily drinks $2.5$ $L$ saturated water by $Ca{F_2}$ . Then how much gram $Ca{F_2}$ present in his body? (Molecular mass of $Ca{F_2}$ is $ 78$ $g$ $mol^{-1}$ )

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