91Ó°ÊÓ

To begin, we must write the acetic acid ionisation equation:

\({\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{COOH(aq)}} \to {\bf{C}}{{\bf{H}}_{\bf{3}}}{\bf{CO}}{{\bf{O}}^{\bf{ - }}}{\bf{(aq) + }}{{\bf{H}}^{\bf{ + }}}{\bf{(aq)}}\)

a)The crucial component of adding \({\rm{HCl}}\) is the addition of \({{\bf{H}}^ + }\)ions. As a result, \({{\bf{H}}^ + }\)ion concentrations will rise. Increasing the concentration of the products, on the other hand, will push the equilibrium towards the reactants, according to the Le Chatelier principle. As a result, \({\rm{C}}{{\rm{H}}_3}{\rm{COOH}}\) concentrations will rise while \({\rm{C}}{{\rm{H}}_3}{\rm{CO}}{{\rm{O}}^ - }\) and \({\rm{C}}{{\rm{H}}_3}{\rm{CO}}_2^ - \)concentrations will fall. The concentration of \({\rm{C}}{{\rm{H}}_3}{\rm{COOH}}\) will increase, the concentration of \({\rm{C}}{{\rm{H}}_3}{\rm{CO}}{{\rm{O}}^ - }\)will decrease, and the concentration of \({{\bf{H}}^ + }\)will remain unchanged.

b) The addition of acetate ions, whose concentration will rise, is the most significant element of adding \({\rm{KC}}{{\rm{H}}_3}{\rm{C}}{{\rm{O}}_2}\). Increasing the concentration of the products, on the other hand, will shift the equilibrium closer to the reactants, according to the Le Chatelier principle. As a result, \({\rm{C}}{{\rm{H}}_3}{\rm{COOH}}\) concentrations will grow while \({\rm{C}}{{\rm{H}}_3}{\rm{CO}}{{\rm{O}}^ - }\)and\({{\bf{H}}^ + }\) concentrations will decrease. In sum, \({\rm{C}}{{\rm{H}}_3}{\rm{COOH}}\) concentrations will rise, \({{\bf{H}}^ + }\) concentrations will fall, and \({\rm{C}}{{\rm{H}}_3}{\rm{CO}}{{\rm{O}}^ - }\) ions concentrations will remain stable.

c) We are not affecting the concentration of any of the species involved in the reaction by adding \({\rm{NaC}}{{\rm{l}}_,}\). As a result, the concentration of none of the species in the reaction will appreciably change.

d) When we add \({\rm{KOH}}\), it's the addition of ions that's crucial. The \(O{H^ - }\)ions will combine with the \({{\bf{H}}^ + }\)ions to create water, lowering the \({{\bf{H}}^ + }\)ions concentration. However, according to the Le Chatelier principle, lowering product concentrations causes the equilibrium to gravitate toward the products. This means that \({\rm{C}}{{\rm{H}}_3}{\rm{COOH}}\)concentrations will decrease significantly while \({{\bf{H}}^ + }\) and \({\rm{C}}{{\rm{H}}_3}{\rm{CO}}{{\rm{O}}^ - }\)concentrations will increase. The concentration of \({\rm{C}}{{\rm{H}}_3}{\rm{COOH}}\) will decrease, the concentration of \({\rm{C}}{{\rm{H}}_3}{\rm{CO}}{{\rm{O}}^ - }\) will increase, and the concentration of \({{\bf{H}}^ + }\)ions will remain unchanged.

e) We will, of course, increase the concentration of \({\rm{C}}{{\rm{H}}_3}{\rm{C}}{{\rm{O}}_2}{\rm{H}}\) if we add \({\rm{C}}{{\rm{H}}_3}{\rm{C}}{{\rm{O}}_2}{\rm{H}}\). Increasing the concentration of reactants, on the other hand, will push the equilibrium towards the products, according to the Le Chatelier principle. As a result, the concentration of \({{\bf{H}}^ + }\)and \({\rm{C}}{{\rm{H}}_3}{\rm{C}}{{\rm{O}}_2}{\rm{H}}\) will decrease, whereas will increase.