Equilibrium

In a qualitative analysis, Bi3+ is detected by appearance of precipitate of BiO(OH)(s). Calculate pH when the following equilibrium exists at 298 K : BiO(OH)(s) BiO+(aq) + OH-(aq), K = 4 × 10-10 (Given : log 2 = 0.3010)

1. 4.699
2. 5.286
3. 8.714
4. 9.301

The correct order of solubility of the given salts in water at 298 K is array|l|l| Salt & Ksp at 298 K \ AgBr & 5.0 10-13 \ Zn(OH)2 & 1.0 10-15 \ Hg2Cl2 & 1.3 10-18 \ array

1. Zn(OH)2 > AgBr > Hg2Cl2
2. Hg2Cl2 > Zn(OH)2 > AgBr
3. AgBr > Zn(OH)2 > Hg2Cl2
4. Hg2Cl2 > AgBr > Zn(OH)2

The ratio of solubility of AgCl in 0.1 M KCl solution to the solubility of AgCl in water is: (Given : Solubility product of AgCl = 10-10)

1. 10-4
2. 10-6
3. 10-9
4. 10-5

Find out the solubility of Ni(OH)2 in 0.1 M NaOH. Given that the ionic product of Ni(OH)2 is 2 10-15.

1. 2 10-8 M
2. 1 10-13 M
3. 1 108 M
4. 2 10-13 M

pH of a saturated solution of Ca(OH)2 is 9. The solubility product ( Ksp) of Ca(OH)2 is :

1. 0.125 10-15
2. 0.5 10-10
3. 0.5 10-15
4. 0.25 10-10

The solubility of BaSO4 in water is 2.42 10-3 g L-1 at 298 K. The value of its solubility product (Ksp) will be (Given molar mass of BaSO4 = 233 g mol-1)

1. 1.08 10-10 mol2 L-2
2. 1.08 10-12 mol2 L-2
3. 1.08 10-14 mol2 L-2
4. 1.08 10-8 mol2 L-2

Concentration of the Ag+ ions in a saturated solution of Ag2C2O4 is 2.2 10-4 mol L-1. Solubility product of Ag2C2O4 is

1. 2.66 10-12
2. 4.5 10-11
3. 5.3 10-12
4. 2.42 10-8

MY and NY3, two nearly insoluble salts, have the same Ksp values of 6.2 10-13 at room temperature. Which statement would be true in regard to MY and NY3?

1. The salts MY and NY3 are more soluble in 0.5 M KY than in pure water.
2. The addition of the salt of KY to solution of MY and NY3 will have no effect on their solubilities.
3. The molar solubilities of MY and NY3 in water are identical.
4. The molar solubility of MY in water is less than that of NY3.

The solubility of AgCl(s) with solubility product 1.6 10-10 in 0.1 M NaCl solution would be

1. 1.25 10-5 M
2. 1.6 10-9 M
3. 1.6 10-11 M
4. zero

The Ksp of Ag2CrO4, AgCl, AgBr and AgI are respectively, 1.1 10-12, 1.8 10-10, 5.0 10-13, 8.3 10-17. Which one of the following salts will precipitate last if AgNO3 solution is added to the solution containing equal moles of NaCl, NaBr, NaI and Na2CrO4?

1. AgBr
2. Ag2CrO4
3. AgI
4. AgCl

Identify the correct order of solubility in aqueous medium.

1. Na2S > CuS > ZnS
2. Na2S > ZnS > CuS
3. CuS > ZnS > Na2S
4. ZnS > Na2S > CuS

The values of Ksp of CaCO3 and CaC2O4 are 4.7 10-9 and 1.3 10-9 respectively at 25 . If the mixture of these two is washed with water, what is the concentration of Ca2+ ions in water ?

1. 5.831 10-5 M
2. 6.856 10-5 M
3. 3.606 10-5 M
4. 7.746 10-5 M

pH of a saturated solution of Ba(OH)2 is 12. The value of solubility product (Ksp) of Ba(OH)2 is

1. 3.3 10-7
2. 5.0 10-7
3. 4.0 10-6
4. 5.0 10-6

In qualitative analysis, the metals of group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains Ag+ and Pb2+ at a concentration of 0.10 M. Aqueous HCl is added to this solution until the Cl- concentration is 0.10 M. What will the concentrations of Ag+ and Pb2+ be at equilibrium ? ( Ksp for AgCl = 1.8 10-10, Ksp for PbCl2 = 1.7 10-5)

1. [Ag+] = 1.8 10-7 M, [ Pb2+] = 1.7 10-6 M
2. [Ag+] = 1.8 10-11 M, [ Pb2+] = 8.5 10-5 M
3. [Ag+] = 1.8 10-9 M, [ Pb2+] = 1.7 10-3 M
4. [Ag+] = 1.8 10-11 M, [ Pb2+] = 1.7 10-4 M

If pH of a saturated solution of Ba(OH)2 is 12, the value of its Ksp is

1. 4.00 10-6 M3
2. 4.00 10-7 M3
3. 5.00 10-6 M3
4. 5.00 10-7 M3

If the concentration of OH- ions in the reaction Fe(OH)3(s) Fe3+(aq) + 3OH-(aq) is decreased by 1/4 times, then equilibrium concentration of Fe3+ will increase by

1. 64 times
2. 4 times
3. 8 times
4. 16 times

H2S gas when passed through a solution of cations containing HCl precipitates the cations of second group of qualitative analysis but not those belonging to the fourth group. It is because

1. presence of HCl decreases the sulphide ion concentration
2. solubility product of group II sulphides is more than that of group IV sulphides
3. presence of HCl increases the sulphide ion concentration
4. sulphides of group IV cations are unstable in HCl.

The solubility product of a sparingly soluble salt AX2 is 3.2 10-11. Its solubility (in moles/L) is

1. 5.6 10-6
2. 3.1 10-4
3. 2 10-4
4. 4 10-4

The solubility product of AgI at 25 C is 1.0 10-16 mol2 L-2. The solubility of AgI in 10-4 N solution of KI at 25 C is approximately (in mol L-1)

1. 1.0 10-16
2. 1.0 10-12
3. 1.0 10-10
4. 1.0 10-8

Solubility of MX2 type electrolytes is 0.5 10-4 mole/lit., then find out Ksp of electrolytes.

1. 5 10-12
2. 25 10-10
3. 1 10-13
4. 5 10-13

Solubility of M2S salt is 3.5 10-6 then find out solubility product.

1. 1.7 10-6
2. 1.7 10-16
3. 1.7 10-18
4. 1.7 10-12