Question

predict whether aqueous solutions of the following compounds are acidic, basic, or neutral.

compound solution is...?

nh₄cl acidic basic neutral

nano₃ acidic basic neutral

nach₃co₂ acidic basic neutral

Explanation:

• For \(NH_4Cl\): \(NH_4Cl\) dissociates into \(NH_4^+\) and \(Cl^-\). \(NH_4^+\) is the conjugate acid of a weak base (\(NH_3\)) and will hydrolyze in water: \(NH_4^+ + H_2O

ightleftharpoons NH_3\cdot H_2O + H^+\), producing \(H^+\) ions. \(Cl^-\) is the conjugate base of a strong acid (\(HCl\)) and does not hydrolyze. So the solution is acidic.

• For \(NaNO_3\): \(NaNO_3\) dissociates into \(Na^+\) and \(NO_3^-\). \(Na^+\) is the cation of a strong base (\(NaOH\)) and \(NO_3^-\) is the conjugate base of a strong acid (\(HNO_3\)). Neither ion hydrolyzes in water. So the solution is neutral.
• For \(NaCH_3CO_2\) (\(NaC_2H_3O_2\)): It dissociates into \(Na^+\) and \(CH_3COO^-\). \(Na^+\) is the cation of a strong base (\(NaOH\)) and does not hydrolyze. \(CH_3COO^-\) is the conjugate base of a weak acid (\(CH_3COOH\)) and will hydrolyze: \(CH_3COO^-+H_2O

ightleftharpoons CH_3COOH + OH^-\), producing \(OH^-\) ions. So the solution is basic.

Answer:

• \(NH_4Cl\): acidic
• \(NaNO_3\): neutral
• \(NaCH_3CO_2\): basic