The aqueous solution of which of the followin | vedclass

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(B) $NaCl$ is a salt of a strong acid $(HCl)$ and a strong base $(NaOH)$,so its solution is neutral $(pH \approx 7)$.$NH_4Cl$ is a salt of a weak base

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$Na_2CO_3$

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(B) $NaCl$ is a salt of a strong acid $(HCl)$ and a strong base $(NaOH)$,so its solution is neutral $(pH \approx 7)$.$NH_4Cl$ is a salt of a weak base $(NH_4OH)$ and a strong acid $(HCl)$,so its solution is acidic $(pH $NaHCO_3$ is an acidic salt,making its solution weakly basic.$Na_2CO_3$ is a salt of a strong base $(NaOH)$ and a weak acid $(H_2CO_3)$,which undergoes anionic hydrolysis to produce $OH^-$ ions,making the solution strongly basic $(pH > 7)$.Therefore,$Na_2CO_3$ has the highest $pH$.

The aqueous solution of which of the following will have the highest $pH$?

Similar Questions

$NH_4CN$ is a salt of a weak acid $HCN$ $(K_a = 6.2 \times 10^{-10})$ and a weak base $NH_4OH$ $(K_b = 1.8 \times 10^{-5})$. $A$ $1 \ M$ solution of $NH_4CN$ will be:

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