I. Studying the lonization of HC2H302 in Water Equilibrium HC2HyO2(aq)+H2o(C2H,2
ID: 1019829 • Letter: I
Question
I. Studying the lonization of HC2H302 in Water Equilibrium HC2HyO2(aq)+H2o(C2H,2 (aq)+HsOt (aq) 1. Based on the initial solution color, is the H,ot concentration in the original equilibrium mixture relatively high or relatively low? Briefly explain. -The Solution was red init ak I )whl ch india ded 2. What experimental evidence do you have that the equilibrium is affected by the addition of solid NaC2H 02? What must ha NaC2H3O2? What must have happened to the HO concentra to the H3O* concentration to produce this evidence? 3. NaCtio, is not a component of the HC,H,O, equilibrium. Explain why the equlibrium is affected by the addition of solid NaC2H302 4. When the equilibrium mixture was heated, did the Hot concentration increase or decrease? Briefly explain. ecke, whun the mixture was hacted, the o Concentration duirzased 5. Based on your answer to Calculation 4,is the forward reaction exothermic or endothermic? Rewrite the equilibrium reaction to include the heat term.Explanation / Answer
(2) YES, equilibrium is affected by addition of solid NaC2H3O2. It shifts the equilibrium towards right side hence concentration of H3O+ is decreased.
(3) Because, NaC2H3O2 produces C2H3O2- ion which is one of the common ions of HC2H3O2. Hence due to common ion effect it decreases the ionisation of acetic acid.
(5) Based on the answer given for 4 calculation, the reaction is exothermic in nature. Because of that only on increasing temperature, reaction shifts in endothermic ide i.e backward in the present case, so H3O+ ion concentration is decreased.