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11 Nov 2019
7. (a) (0.9 pts) The balanced equation for the acid dissociation of acetic acid is given below. Make an "ICE" table showing the initial concentrations, change in concentration and equilibrium concentrations of the three chemical species in the reaction. Initial concentration of the acetic acid is 0.0575 M, Ka, acetic acid-1.75 X 10-5 CH3COOH (aq) CH3COO-(aq) H+ (aq) â + Initial: Change: Equilibrium: (b) (0.6 pt) Use the data in the "ICE" table and the K, stated in the problem to calculate the equilibrium value of [H+
7. (a) (0.9 pts) The balanced equation for the acid dissociation of acetic acid is given below. Make an "ICE" table showing the initial concentrations, change in concentration and equilibrium concentrations of the three chemical species in the reaction. Initial concentration of the acetic acid is 0.0575 M, Ka, acetic acid-1.75 X 10-5 CH3COOH (aq) CH3COO-(aq) H+ (aq) â + Initial: Change: Equilibrium: (b) (0.6 pt) Use the data in the "ICE" table and the K, stated in the problem to calculate the equilibrium value of [H+
Bunny GreenfelderLv2
18 Feb 2019