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(B, C) $1$. The salt of a strong acid and a weak base undergoes cationic hydrolysis, resulting in an acidic solution with $pH < 7$. This is a correct

Vedclass · Accepted Answer

$pH$ of an aqueous solution of $10^{-8} \ M \ HCl$ is $8$.

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(B, C) $1$. The salt of a strong acid and a weak base undergoes cationic hydrolysis, resulting in an acidic solution with $pH $2$. For a salt of a weak acid and a weak base, the $pH$ is determined by the relation $pH = 7 + \frac{1}{2}(pK_{a} - pK_{b})$. If $K_{b}  pK_{a}$, which implies $pH $3$. For a very dilute solution of $HCl$ $(10^{-8} \ M)$, the contribution of $H^{+}$ ions from water cannot be neglected. The total $[H^{+}] = 10^{-8} + 10^{-7} \approx 1.1 	imes 10^{-7} \ M$. Thus, $pH = -\log(1.1 	imes 10^{-7}) \approx 6.96$, which is less than $7$. The statement that $pH$ is $8$ is incorrect.$4$. The conjugate acid of $NH_{2}^{-}$ is formed by adding a proton $(H^{+})$, resulting in $NH_{3}$. This is a correct statement.Therefore, statements $B$ and $C$ are incorrect.

Which of the following statements are incorrect?

Similar Questions

Statement $A$: Addition of $NH_4OH$ in the presence of excess $NH_4Cl$ to an aqueous solution of $BaCl_2$ results in the precipitation of $Ba(OH)_2$.
Reason $B$: $Ba(OH)_2$ is insoluble in water.

The increasing order of $pH$ of $0.1 \ M$ solution of the following compounds is:

Calculate the $pH$ of the resultant mixtures:
$(a)$ $10 \, mL$ of $0.2 \, M \, Ca(OH)_{2} + 25 \, mL$ of $0.1 \, M \, HCl$
$(b)$ $10 \, mL$ of $0.01 \, M \, H_{2}SO_{4} + 10 \, mL$ of $0.01 \, M \, Ca(OH)_{2}$
$(c)$ $10 \, mL$ of $0.1 \, M \, H_{2}SO_{4} + 10 \, mL$ of $0.1 \, M \, KOH$

Identify the correct statements from the following.
$(A)$ The ionic product of water at $100^{\circ} C$ is $< 10^{-14}$.
$(B)$ $pH$ of a solution decreases with increasing temperature.
$(C)$ $NaH_2PO_4$ on hydrolysis gives a basic solution.
$(D)$ $NH_3$ can act both as Bronsted acid and base.

Which one of the following statements is not true?

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