Question

1. Determine the volume, in mL, of 2.00 M HC₂H₃O₂ stock solution that would need to be diluted to 50 mL in order to produce a solution that is 0.30 M in HC₂H₃O₂.

Ox - [HAC); O not included in the rICE table because it is a (s) or (I) O [HAc); -x O [HAC); Ох

2. Write the equilibrium constant expression, K_a, for the ionization of acetic acid, HC₂H₃O_2.

3.In the rICE table for the dissociation of acetic acid, what is the expression for acetic acid taken directly from the equilibrium line of your ICE table? Do not use the x is small assumption. [HAc]_i is the initial concentration of acetic acid

Answer 1

Mixi = M₂ V2 Hi and vi are concentration and volume of stock solution. rebectively, while Me and Ve are final concentration and volume respectively M = 2.00M M2 = 0.30M Vi= ? 1/2 = 50ml M₂ V2 = MINI Vi= M2 V2 = 0.30 M X 50 mL = 7.5 mL M, 8.00 M Hence, 7.5 ml of 2.00m stock solution of H₂ H302 is. needed to be diluted to SomL, 0.30M HC 2 H 3020 Toptions of I question are given in 3 question and Options of 3 quation are in question ) CH₂O2 (aq) + Ht lag! HC2H302 (99) - HC, Hд (О НАС C2 H302 - = AC 7 HAC laq) + egevilibrium constant ex pression Ka = [H+][AC-11 [HAC] Ac laql + Ht Cagl Ka = lonization constant of HC2H302 3. ICE Table: concentration (MI HAclaq) + H+ (aq) + Ac-lag) CHAcli c +x x concentration of +x x HAC x E [HACIi-x At equilibrium LED HAce= I HAile = [HACJi - x) Hence, option I is correct