Chemistry

posted by .

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.

  • Chemistry -

    I'm not sure of what your symbols mean. HF by itself is not a buffer; however, HF in combination with its salt (NaF) is a buffer and your designation of high concn and low concn may be intended to show that. If NaOH is added, it reacts with the H3O^+, and removing H3O^+ shifts the equilibrium to the right to create more H3O^+ to replace that which was removed. The pH will not change much.

Respond to this Question

First Name
School Subject
Your Answer

Similar Questions

  1. science - chemistry (Le Chatelier's)

    How does the concentration of the reactants affect the amount of product obtained?
  2. Chemistry

    I just did a lab on Acids and Bases and I am having trouble with the lab questions I was given to complete. Concentration of NaOH: 0.09999 M Volume of NaOH: 3.25 mL # moles of NaOH: 0.325 moles Initial Concentration of Weak Acid: ?
  3. Chemistry

    A solution with pH = 4 has 1. relatively high concentration of OH- 2. relatively low concentration of H3O+ 3. relatively high concentration of H3O+ 4. zero concentration of OH-
  4. Chemistry

    A solution with pH = 4 has 1. relatively high concentration of OH- 2. relatively low concentration of H3O+ 3. relatively high concentration of H3O+ 4. zero concentration of OH- Some of the answers people are giving me are confusing. …
  5. Chemistry(Please respond, thank you)

    The ionization constant of HA is 4.0e-4. Using the ice table what is the equilibrium concentration of HA in terms of its initial concentration and x?
  6. Chemistry

    Select the statements that correctly describe buffers.?
  7. Chemistry

    You have 800 mL of a 0.050M phosphate buffer, pH 6.5. You need to increase the pH of this buffer to 7.5 by using 6.00M NaOH. Determine the volume of NaOH needed. What will be the final concentration of the buffer?
  8. chemistry

    Titration was used to determine the molarity of acetic acid in vinegar. A primary standard solution of KHP was used to standardize the NaOH. 1. When performing this experiment, impure KHP was used to standardize the NaOH solution. …
  9. Science

    Which of the following correctly identifies active transport?
  10. Science!

    Which of the following correctly identifies active transport?

More Similar Questions