if x moles of NaCN have to be added to 5 L of water to dissolve 0.5 mole Fe(OH)3 in the form of Fe(CN)6 then calculate the value of x/13.25 ( given: ksp of Fe(OH)3 is 2.7×10^-39 . Kf =10^30
Answers
Answer:
if x moles of NaCN have to be added to 5 L of water to dissolve 0.5 mole Fe(OH)3 in the form of Fe(CN)6 then calculate the value of x/13.25 ( given: ksp of Fe(OH)3 is 2.7×10^-39 . Kf =10^30
Explanation:
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What is the solubility ( in mol/L ) of Fe(OH)
3
in a solution of pH=8.0 ? [K
sp
forFe(OH)
3
=1.0×10
−36
] Calculate the solubility of A
2
X
3
in pure water, assuming that neither kind of ion reacts with water.For A
2
X
3
[K
sp
=1.1×10
−23
]
Medium
Solution
verified
Verified by Toppr
pH=8
∴pOH=14−8=6
∴−log[OH
−
]=6
∴[OH
−
]=10
−6
M
Fe(OH)
3
⇋
Fe
3+
+3OH
−
At t=0- s 0 0
At t= equilibrium- (s−x) s (3s+10
−6
)
∴K
sp
=s×(3s+10
−6
)
3
⟹10
−36
=s×(3s)
3
⟹10
−36
=27s
4
⟹s
4
−0.037×10
−36
∴s=4.386×10
−10
mol/L
Therefore, solubility of Fe(OH)
3
is 4.386×10
−10
mol/L
A
2
X
3
⇋2A
x+
+3X
y−
At t=0- s 0 0
At t= equilibrium- (s−x) (2s) (3s)
K
sp
=(2s)
2
(3s)
3
=(4×27)s
5
⟹1.1×10
−23
=108s
5
⟹s=(
108
1.1×10
−23
)
1/5
⟹s=1×10
−5
mol/L
Therefore solubility of A
2
X
3
is 10
−5
mol/L