Chemical Equilibrium Test

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Chemical Equilibrium Test - 35

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Weekly Quiz Competition

Question 1
4 / -1

Solubility product of silver bromide is 5.0 ×10^-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

A
1.2 × 10^-10 g

B
1.2 × 10^-9 g

C
6.2 × 10^-5 g

D
5.0 × 10^-8 g
Question 2
4 / -1

At 25^oC, the solubility product of Mg (OH)₂ is 1.0 × 10^-11. At which pH, will Mg²⁺ ions start precipitating in the form of Mg (OH)₂ from a solution of 0. 001M Mg²⁺ ions ?

A
9

B
10

C
11

D
8
Question 3
4 / -1

The solubility of AgCl in 0. 2M NaCl solution is
(K_SP of AgCl = 1.20 × 10^-10)

A
6.0 × 10^-10 M

B
0.2 M

C
1.2 × 10^-10 M

D
0.2 × 10^-10 M
Question 4
4 / -1

Solid Ba (NO₃)₂ is gradually dissolved in a 1.0 × 10^-4 M Na₂CO₃ solution. At what concentration of Ba²⁺ will a precipitate begin to form?
(K_SP for BaCO₃ = 5.1 × 10^-9)

A
4.1 × 10^-5 M

B
5.1 × 10^-5 M

C
8.1 × 10^-8 M

D
8.1 × 10^-7 M

Solution
Question 5
4 / -1

In qualitative analysis, in III group NH₄ Cl is added before NH₄OH because

A
to increase the concentration of NH₄⁺ ions

B
to increase the concentration of Cl^- ions

C
to reduce the concentration of OH^- ions

D
to increase the concentration of OH^- ions
Question 6
4 / -1

If K_P of Ag ₂S is 10^-17, then the solubility of Ag₂S in 0.1 M solution of Na₂S will be

A
10^-8

B
5 × 10^-9

C
10^-15

D
10^-16
Question 7
4 / -1

Solubility product constant [K_sp ] of salts of types MX, MX₂ and M₃X at temperature T are 4.0 × 10^-8, 3.2 × 10^-14 and 2.7 × 10 respectively. Solubilities (mol, dm^-3) of the salts at temperature T are in the order

A
MX > MX₂ > M₃X

B
M₃X > MX₂ > MX

C
MX₂ > M₃X > MX

D
MX > M₃X > MX₂

Solution
Question 8
4 / -1

Solubility product of a salt AB is 1 x 10^-8 M² in a solution in which the concentration of A⁺ ions is 10^-3 M. The salt will precipitate when the concentration of B^- ions is kept

A
Between 10^-8 to 10^-7 M

B
between 10^-7 M to 10^-8 M

C
> 10^-5 M

D
< 10^-8 M
Question 9
4 / -1

In a saturated solution of the sparingly soluble strong electrolyte AgIO₃ (molecular mass = 283) the equilibrium which sets in is
AgIO₃ (s) ⇌ Ag⁺ (aq) IO₃^- (aq)
If, the solubility product constant K_sp of AgIO₃ at a given temperature is 1.0 × 10^-8, then what is the mass of AgIO₃ contained in 100 mL of its saturated solution ?

A
2.83 × 10^-2 g

B
2.83 × 10^-3 g

C
1.0 × 10^-7 g

D
1.0 × 10^-4 g
Question 10
4 / -1

The solubility in water of a sparingly soluble salt AB₂ is 1.0 × 10^-5 mol L^-1. Its solubility product number will be

A
4 × 10^-15

B
4 × 10^-10

C
1 × 10^-15

D
1 × 10^-10

Solution

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Chemical Equilibrium Test - 35

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Question 1

1.2 × 10-10 g

1.2 × 10-9 g

6.2 × 10-5 g

5.0 × 10-8 g

Question 2

9

10

11

8

Question 3

6.0 × 10-10 M

0.2 M

1.2 × 10-10 M

0.2 × 10-10 M

Question 4

4.1 × 10-5 M

5.1 × 10-5 M

8.1 × 10-8 M

8.1 × 10-7 M

Solution

Question 5

to increase the concentration of NH4+ ions

to increase the concentration of Cl- ions

to reduce the concentration of OH- ions

to increase the concentration of OH- ions

Question 6

10-8

5 × 10-9

10-15

10-16

Question 7

MX > MX2 > M3X

M3X > MX2 > MX

MX2 > M3X > MX

MX > M3X > MX2

Solution

Question 8

Between 10-8 to 10-7 M

between 10-7 M to 10-8 M

> 10-5 M

< 10-8 M

Question 9

2.83 × 10-2 g

2.83 × 10-3 g

1.0 × 10-7 g

1.0 × 10-4 g

Question 10

4 × 10-15

4 × 10-10

1 × 10-15

1 × 10-10

Solution

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1.2 × 10^-10 g

1.2 × 10^-9 g

6.2 × 10^-5 g

5.0 × 10^-8 g

6.0 × 10^-10 M

1.2 × 10^-10 M

0.2 × 10^-10 M

4.1 × 10^-5 M

5.1 × 10^-5 M

8.1 × 10^-8 M

8.1 × 10^-7 M

to increase the concentration of NH₄⁺ ions

to increase the concentration of Cl^- ions

to reduce the concentration of OH^- ions

to increase the concentration of OH^- ions

10^-8

5 × 10^-9

10^-15

10^-16

MX > MX₂ > M₃X

M₃X > MX₂ > MX

MX₂ > M₃X > MX

MX > M₃X > MX₂

Between 10^-8 to 10^-7 M

between 10^-7 M to 10^-8 M

> 10^-5 M

< 10^-8 M

2.83 × 10^-2 g

2.83 × 10^-3 g

1.0 × 10^-7 g

1.0 × 10^-4 g

4 × 10^-15

4 × 10^-10

1 × 10^-15

1 × 10^-10