What is the minimum pH necessary to cause a precipitate of Pb OH 2 K sp - 1-2- 10 -5 to form in a 0-12 M PbC l 2 solution-

The correct option is B 10.0 The dissociation of the above salt can be written as: #160; Pb(OH)_2 → Pb^+2 + 2OH^ Therefore, the equation of K_ ...

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Standard X

Chemistry

What is the m...

Question

What is the minimum pH necessary to cause a precipitate of $P b {(O H)}_{2} (K_{s p} = 1.2 \times 10^{- 5})$ to form in a $0.12 M P b C l_{2}$ solution?

12.4

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Solution

The correct option is B $10.0$
The dissociation of the above salt can be written as:
$P b (O H)_{2} \to P b^{+ 2} + 2 O H^{-}$
Therefore, the equation of $K_{s p} =$ $[P b^{+ 2}] [O H^{-}]^{2}$
In present case, it is are given that $K_{s p} = 1.2 \times 10^{- 5}$ and $[P b + 2] = 0.12 M .$
NOw we can calculate $[O H^{-}] = \sqrt{\frac{1.2 x 10^{- 5}}{.012}} = 10^{- 4}$
Therefore, $p O H = - l o g (10^{- 4}) = l o g (10^{4}) = 4$
$⟹ p H = 14 - p O H$
$⟹ p H = 14 - 4 = 10$

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Similar questions

Q. What is the minimum pH of a solution

0.10 M

{M g}^{2 +}

from which

M g {(O H)}_{2}

will not precipitate?

K_{s p} M g {(O H)}_{2} = 1.2 \times 10^{- 11} M^{3}

Q. At

25^{o} C,

will a precipitate of

M g (O H)_{2}

form, in a

10^{- 4} M

solution of

M g (N O_{3})_{2}

if pH of the solution is adjusted to

9.0

K_{s p} [M g (O H)_{2}]) = 10^{- 11} M^{3}

. At what minimum value of pH will precipitation start?

Q. At

25^{\circ} C

, will a precipitate of

M g (O H)_{2}

form when a

0.0001 M

solution of

M g (N O_{3})_{2}

is adjusted to a

p H

9.0

? At what minimum value of

p H

will precipitation start?
[Given that:

K_{s p} (M g (O H)_{2}) = 10^{- 11} M^{3}

]

Q. At

25^{o} C,

will a

1 \times 10^{- 4} M

solution of

M g (N O_{3})_{2}

form a precipitate of

M g (O H)_{2}

if pH of the solution is adjusted to 9.0.

K_{s p} (M g (O H))_{2} = 8.9 \times 10^{- 12} M^{3} .

At which minimum pH will the precipitation start?

\sqrt{8.9} = 2.98

l o g 2.98 = 0.474

Q. The

K_{s p}

for

M g (O H)_{2}

in water is

1.2 \times 10^{- 11}

. In an acidic solution, if the

M g^{2 +}

concentration is

1.2 \times 10^{- 5} m o l / L

, what is the pH at which

M g (O H)_{2}

just begins to precipitate?

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What is the minimum pH necessary to cause a precipitate of Pb(OH)2(Ksp = 1.2×10−5) to form in a 0.12 M PbCl2 solution?

What is the minimum pH necessary to cause a precipitate of $P b {(O H)}_{2} (K_{s p} = 1.2 \times 10^{- 5})$ to form in a $0.12 M P b C l_{2}$ solution?