Le Chatelier's principle simply explains how equilibria change as you change the conditions of a reaction. If you have a reaction that is at equilibrium lets say (A + 2B <--> C + D) by removing C or D we can drive the reaction forward and products more products. I can provide a more in-depth description if needed.
Answer:
Solution that is 0.100 M CH3COOH (acetic acid)
and 0.100 M NaCH3COO (sodium acetate)
Find pH of buffer solution:
CH3COOH(aq) + H2O ↔ CH3COO-
(aq) + H3O+(aq)
[CH3COOH] [CH3COO-
] [H3O+]
initial 0.100 0.100 ≈0
-x x x
equil 0.100 – x 0.100 + x xFind pH of buffer solution:
CH3COOH(aq) + H2O ↔ CH3COO-
(aq) + H3O+(aq)
Ka = [CH3COO-
][H3O+
]
[CH 3COOH] = (.100 + x)x
(.100 - x) = 1.8 x 10-5
x = 1.80 x 10-5 M
pH = 4.7
Explanation:
It is 3 moles. Don't doubt urself
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