Thursday
February 26, 2015

Homework Help: Chemistry

Posted by sh on Thursday, June 3, 2010 at 1:49pm.

Consider the following buffer equilibrium:
HF (high concentration) + H2O <--> H3O+ (low concentration) + F- ( high concentration)
Using Le Chatelier's Principle, explain what happens to the pH of the buffer solution when a small amount of NaOH is added.

Wouldn't OH- react with HF to form water? But they're both on the reactants side.

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

Chemistry - A solution with pH = 4 has 1. relatively high concentration of OH- 2...
Chemistry - A solution with pH = 4 has 1. relatively high concentration of OH- 2...
Chemistry(Please respond, thank you) - The ionization constant of HA is 4.0e-4. ...
Chemistry - Select the statements that correctly describe buffers.? 1) The pH of...
Science 1 question - 5. Which of the following would be true during the ...
Science - Which of the following would be true during the inhalation phase of ...
CHEM - A concentrated weak acid is best described as which of the following? (a...
Chemistry - Ok so you have 50mL of sucrose and 977mL of buffer solution - after ...
chemistry - Using the concentration of CH3COOH (0.8326M) and the equilibrium ...
Chemistry - A buffer solution contains HC2H3O2 at a concentration of 0.225 M ...

Members