Consider the following salts. Which one(s) when dissolved in water will produce an acid solution?
1. ${N H}_{4} C l$
2. ${K H S O}_{4}$
3. $N a C N$
4. ${K N O}_{3}$

2 and 3

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1 and 2

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only 3

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2 and 4

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Solution

The correct option is C 1 and 2
Since $N H_{4} C l$ is salt of strong acid & weak base, it will form acidic solution.
Also, $K H S O_{4}$ will form acidic solution as it will have $[H^{+}]$ twice that of $[O H^{-}]$ due to $H_{2} S O_{4}$ .
Hence $1$ & $2$ will give acidic solution.

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Similar questions

1. N H_{4} C l 2. K H S O_{4} 3. N a C N 4. K N O_{3}

1. R b C l O_{4} 2. N a N O_{3} 3. N H_{4} C l 4. N a C l

\begin{matrix} a . N H_{4} C l & b . K_{2} S O_{4} c . N a C N & d . K N O_{3} e . A l C l_{3} & f . C u S O_{4} g . K_{2} S O_{4} . A l_{2} (S O_{4})_{3} .24 H_{2} O & h . A l C l B r I i . Z n C l_{2} & j . N a H C O_{3} \end{matrix}

Borax

N H_{4} C l

N a_{2} C O_{3}

N H_{4} N O_{3}

Which of the following salts when dissolved in water will get hydrolysed to form an acidic solution?

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