Which of the following aqueous solutions will | vedclass

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(B) To determine the $pH$ of the salt solutions,we analyze the nature of the salt:$1$. $NaCl$ is a salt of a strong acid $(HCl)$ and a strong base $(N

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$Na_2CO_3$

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(B) To determine the $pH$ of the salt solutions,we analyze the nature of the salt:$1$. $NaCl$ is a salt of a strong acid $(HCl)$ and a strong base $(NaOH)$,so it is neutral $(pH \approx 7)$.$2$. $Na_2CO_3$ is a salt of a weak acid $(H_2CO_3)$ and a strong base $(NaOH)$,making it basic $(pH > 7)$.$3$. $NH_4Cl$ is a salt of a strong acid $(HCl)$ and a weak base $(NH_4OH)$,making it acidic $(pH $4$. $NaHCO_3$ is an amphoteric salt,but it is less basic than $Na_2CO_3$ because $Na_2CO_3$ undergoes hydrolysis to produce more $OH^-$ ions.Comparing these,$Na_2CO_3$ produces the highest concentration of $OH^-$ ions in solution,resulting in the highest $pH$.

Which of the following aqueous solutions will have the highest $pH$?

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