Choose the solution with lowest pH value:

C a C O_{3}

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C H_{3} C O O N a

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C a (O H)_{2}

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C a C l_{2}

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Solution

The correct option is D $C a C l_{2}$
$C H_{3} C O O N a$ is a salt of weak acid with strong base. Its solution will be basic with highest pH.
$C a C O_{3}$ and $C a (O H)_{2}$ are salts of weak acid with weak base. They will have intermediate pH.
$C a C l_{2}$ is a salt of strong acid with weak base. Hence, its solution will be acidic with lowest pH.

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Similar questions

Which of the following salt solutions ( $0.1 M$ each) will have the lowest pH values?

C a (O H)_{2}

p H

5 \times 10^{- 2} M

C a (N O_{3})_{2}

K_{s p} (C a (O H)_{2}) = 5 \times 10^{- 6} M^{3}]

C a (O H)_{2}

p H

5 \times 10^{- 2} M

C a (N O_{3})_{2}

K_{s p} (C a (O H)_{2}) = 5 \times 10^{- 6} M^{3}]

$2 C a (O H)_{2} + 2 C l_{2} \to A - - + B - - + 2 H_{2} O$

A & B are

C a (O H)_{2}

(K_{s p})

C a (O H)_{2}

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