MY and N Y 3 , two nearly insoluble salts, have the same K s p values of 6.2 × 10 - 13 at room temperature. Which statement would be true in regard to MY and N Y 3 ?

The molar solubility of MY in water is less than that of N Y 3 .

The molar solubilities of MY and N Y 3 in water are identical.

The salts MY and N Y 3 are more soluble in 0.5 M KY than in pure water.

The addition of the salt of KY to solution of MY and N Y 3 will have no effect on their solubilities.

MEDIUM

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$M g {(O H)}_{2}$ is precipitated when $N a O H$ is added to a solution of $M g^{2 +}$ . If the final concentration of $M g^{2 +}$ is $10^{- 10}$ M, the concentration of $O H^{-} (M)$ in the solution is

[Solubility product for $M g {(O H)}_{2} = 5.6 \times 10^{- 12}$ ]

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Important Questions on Ionic Equilibria

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

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?

EASY

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

K_{sp}

{Ag}_{2} {CO}_{3}

8 \times 10^{- 12}

, the molar solubility of

{Ag}_{2} {CO}_{3}

0 .1 M {AgNO}_{3}

is:

HARD

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

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}

1 \times 10^{- 10}

. What is the original concentration of

{Ba}^{2 +}

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

The molar solubility of

C d {(O H)}_{2}

1.84 \times 10^{- 5} M

in water. The expected solubility of

C d {(O H)}_{2}

in a buffer solution of

p H = 12

is:

HARD

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

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 ____(Nearest integer). (Given that the value of solubility product of

AB (K_{sp}) = 2 \times 10^{- 10}

, and the value of ionisation constant of

HB (Ka) = 1 \times 10^{- 8}

)

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

pH of a saturated solution of

C a {(O H)}_{2}

9

. The solubility product

(K_{s p})

C a {(O H)}_{2}

is:

HARD

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

Zirconium phosphate

[{Zr}_{3} {({PO}_{4})}_{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 ?

EASY

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

Solubility of

AgCl

is least in

HARD

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

Consider the electrochemical reaction between

A g (s)

and

C l_{2} (g)

electrodes in

1 L

0.1 M K C l

aqueous solution. Solubility product of

A g C l

1.8 x 10^{- 10}

and

F = 96500 C / m o l

. At

1 x 10^{- 6} A

current, calculate the time required to start observing the

A g C l

precipitation in the galvanic cell

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

Concentration of the

{Ag}^{+}

ions in a saturated solution of

{Ag}_{2} C_{2} O_{4}

2.2 \times 10^{- 4} mol L^{- 1}

. Solubility product of

{Ag}_{2} C_{2} O_{4}

is:

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

The

K_{s p}

for the following dissociation is

1.6 \times 10^{- 5}

{P b C l}_{2 (s)} ⇌ P b_{(a q)}^{2 +} + 2 C l_{(a q)}^{-}

Which of the following choices is correct for a mixture of

300 mL, 0 .134 M Pb {({NO}_{3})}_{2}

and

100 m L,

0.4 M N a C l ?

HARD

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

The

K_{sp}

{Ag}_{2} {CrO}_{4}, AgCl, AgBr

and

A g I

are respectively,

1.1 \times 10^{- 12}, 1.8 \times 10^{- 10}, 5.0 \times 10^{- 13}, 8.3 \times 10^{- 17}

. Which one of the following salts will precipitate last if

A g N O_{3}

solution is added to the solution containing equal moles of NaCl, NaI, NaBr and

N a_{2} C r O_{4}

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

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

Question Image

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

What is the molar solubility of

A I {(O H)}_{3}

0.2

M N a O H

solution? Given that, solubility product of

Al {(O H)}_{3} = 2.4 \times 10^{- 24}

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

The solubility product of

C r {(O H)}_{3}

298 K

6.0 \times 10^{- 31} .

The concentration of hydroxide ions in a saturated solution of

C r {(O H)}_{3}

will be

EASY

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

If the solubility product of ${AB}_{2}$ is $3.20 \times 10^{- 11} M^{3}$ , then the solubility of ${AB}_{2}$ in pure water is _______ $\times 10^{- 4} mol L^{- 1}$

[Assuming that neither kind of ion reacts with water]

EASY

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

The

K_{sp}

for bismuth sulphide

({Bi}_{2} S_{3})

1.08 \times 10^{- 73}

. The solubility of

{Bi}_{2} S_{3}

{molL}^{- 1}

298 K

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

When

1 .88 g of AgBr (s)

is added to a

10^{- 3} M

aqueous solution of

KBr,

the concentration of

Ag is 5 \times 10^{- 10} M

. If the same amount of

AgBr (s)

is added to a

10^{- 2} M

aqueous solution of

{AgNO}_{3},

the concentration of

{Br}^{-}

EASY

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

The solubility of

A g C l (s)

with solubility product

1.6 \times 10^{- 10}

0.1 M N a C l

solution would be

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibria>Solubility Equilibria of Sparingly Soluble Salts

MY and

N Y_{3}

, two nearly insoluble salts, have the same

K_{s p}

values of

6.2 \times 10^{- 13}

at room temperature. Which statement would be true in regard to MY and

N Y_{3}

MgOH2 is precipitated when NaOH is added to a solution of Mg2+ . If the final concentration of Mg2+ is 10-10 M, the concentration of OH-M in the solution is [Solubility product for MgOH2=5.6×10-12 ]

Important Questions on Ionic Equilibria

Learn and Prepare for any exam you want !

$M g {(O H)}_{2}$ is precipitated when $N a O H$ is added to a solution of $M g^{2 +}$ . If the final concentration of $M g^{2 +}$ is $10^{- 10}$ M, the concentration of $O H^{-} (M)$ in the solution is

[Solubility product for $M g {(O H)}_{2} = 5.6 \times 10^{- 12}$ ]