Question

A student measures the molar solubility of nickel(II) cyanide in a water solution to be 2.00×10-8 M. what is the ksp

Answer 1

The molar solubility of nickel(II) cyanide is
1.91
×
10
−
8
M
.
The nickel (II) cyanide dissociates in water as shown below.

N
i
(
C
N
)
2
(
s
)
↔
N
i
2
+
(
a
q
)
+
2
C
N
−
(
a
q
)
s
2
s
N
i
(
C
N
)
2
(
s
)
↔
N
i
2
+
(
a
q
)
+
2
C
N
−
(
a
q
)
s
2
s


Where,
s
s
is the solubility of nickel (II) cyanide.

The value of solubility product of nickel(II) cyanide is calculated by the formula given below.

K
s
p
=
[
N
i
2
+
]
[
C
N
−
]
2
K
s
p
=
[
N
i
2
+
]
[
C
N
−
]
2

Substitute the values in the above formula.

K
s
p
=
(
1.91
×
10
−
8
M
)
(
2
×
1.91
×
10
−
8
M
)
2
=
27.871
×
10
−
24
K
s
p
=
(
1.91
×
10
−
8
M
)
(
2
×
1.91
×
10
−
8
M
)
2
=27.871×
10
−
24


Therefore, the calculated value of solubility product of nickel(II) cyanide is
27.871
×
10
−
24
.
27.871
×
10
−
24
.

Answer 2

27.871×10−24

Step-by-step explanation:

The molar solubility of nickel(II) cyanide is 1.91×10−8M.

The nickel (II) cyanide dissociates in water as shown below

Ni(CN)2(s)↔Ni2+(aq)+2CN−(aq)s2s

Where, s is the solubility of nickel (II) cyanide.

The value of solubility product of nickel(II) cyanide is calculated by the formula given below.

Ksp=[Ni2+][CN−]2

Substitute the values in the above formula. Ksp=(1.91×10−8M)(2×1.91×0−8M)2=27.871×10−24