The pH of an acetate buffer was determined to be 4.76. Then, a few drops of...

Question

Question

The pH of an acetate buffer was determined to be 4.76. Then, a few drops of 1.0 M NaOH was added to it. Which of the following is true?

A. The buffer solution contains equal amounts of CH₃COOH and CH₃COO^–.

B. The buffer solution contains slightly more CH₃COOH than CH₃COO^–.

C. The buffer solution contains slightly more CH₃COO^– than CH₃COOH.

Answer 1

Answer #1

Answer 2

Similar Homework Help Questions

1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic...

1) Calculate the pH of the 1L buffer composed of 500 mL of 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of HCl is added (Ka HC2H3O2 = 1.75 x 10-5). Report your answer to the hundredths place. 2) Calculate the pH of the 1L buffer composed of 500 mL 0.60 M acetic acid plus 500 mL of 0.60 M sodium acetate, after 0.010 mol of NaOH is added (Ka HC2H3O2 = 1.75...
Which of the following statements is TRUE? At pH = 9, [CH3COOH] would be a lot...

Which of the following statements is TRUE? At pH = 9, [CH3COOH] would be a lot lower than [CH3COO-] At pH = 2, [CH3COO-] would be dominant, compared to [CH3COOH] The ratio of concentration of acetate to acetic acid in a solution would go up as pH goes down. At pH = 4.76, [CH3COO-] = 2 * [CH3COOH]
Buffer action 4 A buffer solution consisting of 0.05 mol/L acetic acid (CH3COOH) and 0.05 mol/L...

Buffer action 4 A buffer solution consisting of 0.05 mol/L acetic acid (CH3COOH) and 0.05 mol/L acetate (CH3COO-) has been used to buffer a 1 L solution at pH 4.7. A small amount of sodium hydroxide solution containing 0.0001 mol NaOH was added. Which of the following reactions best represents the buffer action? + Select one: O a. NaOH(aq) Na+(aq) + OH(aq) O b. CH3COOH(aq) + H2O(1) CH3COO(aq) H30*(aq) O c. CH3COO(aq) + H2O(0) CH3COOH(aq) OH(aq) O d. CH3COOH(aq) +...

9. 15.00 mL of 0.100 M NaOH are added to 50.00 mL of a buffer solution...

9. 15.00 mL of 0.100 M NaOH are added to 50.00 mL of a buffer solution containing 1.0 mmol CH3COOH and 1.0 mmol CH3C00-. What is the new solution pH? (a) 11.89 (b) 2.11 (c) 7.87 (d) Can't tell / need more info. 10. The equilibrium constant for the below reaction is 4.2 x 10 Which of the following statements is FALSE? CuBr (s) = Cu+ (aq) + Br- (aq) (a) CuBr has poor solubility in water. (b) If 15.0...
15.00 mL of 0.100 M NaOH are added to 50.00 mL of a buffer solution containing...

15.00 mL of 0.100 M NaOH are added to 50.00 mL of a buffer solution containing 1.0 mmol CH3COOH and 1.0 mmol CH3COO-. What is the new solution pH? (show work) a) 11.89 b) 2.11 c) 7.87 d) can't tell/need more info.
A buffer at pH of 4.35 contains CH3COOH at a concentration of 0.60 M and CH3COONa...

A buffer at pH of 4.35 contains CH3COOH at a concentration of 0.60 M and CH3COONa at a concentration of 0.30 M. What will be the pH when 75.8 mL of 0.980 M NaOH is added to 450.4 mL of the buffer? The pKa of CH3COOH is 4.76 dlace of

1.A 1.00 liter solution contains 0.28 M acetic acid and 0.36 M sodium acetate. If 0.180...

1.A 1.00 liter solution contains 0.28 M acetic acid and 0.36 M sodium acetate. If 0.180 moles of potassium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of potassium hydroxide.) A. The number of moles of CH3COOH will remain the same. B. The number of moles of CH3COO- will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will increase....
Prepare 100mL of a 0.2M acetate buffer solution of pH =4.76 (using 17.6N acetic acid and...

Prepare 100mL of a 0.2M acetate buffer solution of pH =4.76 (using 17.6N acetic acid and sodium acetate). a. Calculate the volume of acetic acid and weight of sodium acetate necessary to prepare the buffer solution. pKa of acetic acid is 4.76
A buffer is prepared by adding 18.0 g of sodium acetate (CH3COONa) to 490 mL of...

A buffer is prepared by adding 18.0 g of sodium acetate (CH3COONa) to 490 mL of a 0.140 M acetic acid (CH3COOH) solution. 1) Determine the pH of the buffer. 2) Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. (Express your answer as a chemical equation. Identify all of the phases in your answer.) 3) Write the complete ionic equation for the reaction that occurs when...

1) A buffer solution contains 0.356 M C6H5NH3Cl and 0.303 M C6H5NH2 (aniline). Determine the pH...

1) A buffer solution contains 0.356 M C6H5NH3Cl and 0.303 M C6H5NH2 (aniline). Determine the pH change when 0.066 mol NaOH is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change=? 2) Determine the pH change when 0.068 mol HCl is added to 1.00 L of a buffer solution that is 0.462 M in CH3COOH and 0.227 M in CH3COO-. pH after addition − pH before addition = pH change =?