Given that the solubility product of Ag2CrO4 is 1.9x 10-12, will a precipitate be formed when 10 ml of 0.05M AgNO3 and 30 ml of 0.03 M Na2CrO4 are mixed ?PLEASE SHOW THE WORKING

Answers 1

Explanation:

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Class 11

>>Chemistry

>>Equilibrium

>>Solubility Equilibria

>>The solubility product of Ag2CrO4 is 1.9

Question

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The solubility product of Ag

2

CrO

4

is 1.9X10

−12

.The volume of water in mL that can dissolve 4mg of Ag

2

CrO

4

is about:

Hard

Solution

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Correct option is A)

Ag

2

CrO

4

⇌2Ag

+

+CrO

4

2−

Let S mol/L be the solubility of Ag

2

CrO

4

[Ag

2

CrO

4

]=[CrO

4

2−

]=S

[Ag

+

]=2S

K

sp

=[Ag

+

]

2

[CrO

4

2−

]

1.9×10

−12

=(2S)

2

×S=4S

3

S=7.8×10

−5

M

The molar mass of Ag

2

CrO

4

=331.7 g/mol

Convert solubility of Ag

2

CrO

4

from mol/L to g/L.

S=7.8×10

−5

mol/L×331.7 g/mol

S=0.0259 g/L

Convert solubility of Ag

2

CrO

4

from g/L to mg/mL.

S=0.0259 g/L×

1 g

1000 mg

×

1000 mL

1 L

S=0.0259 mg/mL

To dissolve 4 mg of Ag

2

CrO

4

, volume of water required will be 4 mg×

0.0259 mg

1 mL

=154 mL≃150 mL.

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