Question

A) Consider the acid-base nature of the salt [(C₂H₅)₃NH]CH₃COO, when it is dissolved in water.

(1) What are the acid-base properties of the cation, (C₂H₅)₃NH⁺?   _________acidic basic neutral

(2) What are the acid-base properties of the anion, CH₃COO^-?   _________acidic basic neutral

(3) Would an aqueous solution of [(C₂H₅)₃NH]CH₃COO be acidic, basic or neutral?

B )Consider the acid-base nature of barium hypochlorite, Ba(ClO)₂, when it is dissolved in water.

(1) What are the acid-base properties of the cation?   _________acidic basic neutral

(2) What are the acid-base properties of the anion?   _________acidic basic neutral

(3) Would an aqueous solution of barium hypochlorite be acidic, basic or neutral?

Answer 1

The cations which able to donate protons (H+) or accept lone pair of electrons are acidic in nature.

The antions which able to donate lone pairs of electrons or accept protons (H+)   are basic in nature.

(C2H5)3NH+ is Acidic in nature because it donates H+ ions

(C2H5)3NH+ + H2O $\rightarrow$ (C2H5)3N + H3O+  (concentration of H+ ions increased. so, acidic)

CH3COO- is basic in nature because it accepts H+ ions

CH3COO- + H2O $\rightarrow$ CH3COOH  + -OH (concentration of H+ ions decreased it means it accepts the H+ ions . so, basic)

[(C2H5)3NH]CH3COO is almost neutral because it is salt of weak base-weak acid. It can dissociate very low amount when dissolved in water.

Ba(ClO)2 salt

Ba2+   Acidic in nature because it accepts lone pair

Ba2+ + 2H2O $\rightarrow$ Ba(OH)2 + 2H+  (concentration of H+ ions increased. so, acidic)

ClO-  is basic in nature because it accepts H+ ions

ClO- + H2O $\rightarrow$ HClO  + -OH (concentration of H+ ions decreased it means it accepts the H+ ions . so, basic)

Ba(ClO)2 is salt of a weak acid-strong base when dissolved in water it gives basic solution. Solution is basic in nature beacuse the concentration of OH– increases.

Ba2+ + 2H2O $\rightarrow$ Ba(OH)2