........HCHO2 --> H^+ + CHO2^-
I........0.2......0......0
C.......-0.006..0.006...0.006
E......0.2-0.006..0.006..0.006
Ka = (H^+)(CHO2^-)(HCHO2)
Ka = (0.006)(0.006)/(0.2-0.006)
Ka = ?
pH = -log(H^+) = -log(0.006) = ?
HCHO2 --> H^+ + CHO2^-
Le Chatelier's Principle tells us that when we do something to a system in equilibrium that the reaction will shift so as to undo what we've done to it. Therefore, if we add CHO2^- the reaction must get rid of what we've added. It can do that by shifting to the left. In doing so (H^+) will decrease and (HCHO2) will increase.
If a solution of formic acid contains 0.2 M HCHO2, 0.006 M CHO2-, and 0.006 M H+,
What is the Ka of the acid?
What is the ph of the solution at the concentrations given?
What would happen to the equilibrium position if more CHO2- were added to the solution?
1 answer
2 answers