Question

Will rate for sure

In Experiment 4, you will investigate the following reaction: CH3COOH (aq) + NaOH (aq) → CH3COONa (aq) + H2O (l) You will add controlled amounts of sodium hydroxide to an acetic acid solution. Throughout the course of the reaction, the chemical species present in the reaction mixture will change, along with their concentration. To understand a titration experiment, it is important to know what species are present in the reaction mixture at a given time, as well as how much of each is present. These questions will help you review stoichiometry of reactions. Assume that your initial aqueous solution contains only 0.100 mol of acetic acid and has a volume of 100 mL. To this acetic acid solution you will add a 1.0 mol/L NaOH solution. Let's see what happens after adding different amounts of NaOH. Suppose you have added a total of 22.0 mL of NaOH solution since the beginning of the titration. How many mol of acetate ions are present in the reaction mixture at this point?

Answer 1

CH₃COOH(aq) + NaOH(aq) ------> CH₃COO^-(aq) + Na⁺(aq) + H₂O(l)

Total moles of acetic acid present = molarity*volume of acetic acid solution in litres = 0.1

moles of NaOH added = molarity*volume of NaOH solution in litres = 1*0.022 = 0.022

Thus, moles of acetate ions in the solution = moles of NaOH added = 0.022

Total volume of the solution = 122 ml = 0.122 litres

Thus, molar concentration of acetate ions = moles/volume of the solution in litres = 0.022/0.122 = 0.18 M