A) \[C{{H}_{3}}COOK\]
B) \[N{{a}_{2}}C{{O}_{3}}\]
C) \[N{{H}_{4}}Cl\]
D) \[NaN{{O}_{3}}\]
Correct Answer: B
Solution :
\[pH=\log \frac{1}{[{{H}^{+}}]}\] pH is inversely proportional to hydrogen ion con- centration. As the concentration of \[{{H}^{+}}\] decreases, pH increases and vice versa. Ammonium chloride\[(N{{H}_{4}}Cl)\] is a salt of weak base and strong acid. So, its aqueous solution will be acidic as \[N{{H}_{4}}Cl+{{H}_{2}}O\xrightarrow{{}}\underset{weak\,acid}{\mathop{N{{H}_{4}}OH}}\,+\underset{strone\,base}{\mathop{HCl}}\,\] So, pH of \[N{{H}_{4}}Cl\]is less than 7. Sodium nitrate\[(NaN{{O}_{3}})\] is the salt of strong acid and strong base. So, its aqueous solution is neutral as \[NaN{{O}_{3}}+{{H}_{2}}O\xrightarrow{{}}\underset{Strong\,base}{\mathop{NaOH}}\,+\underset{Strong\,acid}{\mathop{HN{{O}_{3}}}}\,\] So, pH of \[NaN{{O}_{3}}\]is 7, Potassium acetate \[(C{{H}_{3}}COOK)\] is a salt of strong base and weak acid. Its aqueous solution will be basic and pH value will be \[7\approx 8.8\] \[C{{H}_{3}}COOK+{{H}_{2}}O\xrightarrow{{}}\underset{Weak\,acid}{\mathop{C{{H}_{3}}COOH}}\,+\underset{Stong\,base}{\mathop{KOH}}\,\] Sodium carbonate \[(N{{a}_{2}}C{{O}_{3}})\]is a salt of strong base and weak acid. Its aqueous solution is also basic and its pH value will be more than 10, \[N{{a}_{2}}C{{O}_{3}}+{{H}_{2}}O\xrightarrow{{}}\underset{Strong\,acid}{\mathop{2NaOH}}\,+\underset{Weak\,base}{\mathop{{{H}_{2}}C{{O}_{3}}}}\,\]
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