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19 Nov 2019
The pKa of acetic acid is 4.7. What is the buffering range of this acid and its conjugate base? Explain your answer. Calculate the volume of 6 M acetic acid needed to prepare 100 mL of a 0.10 M acetic acid (CH_3COOH) solution. Calculate the mass of sodium acetate (CH_3COONa) required to prepare 50 mL of a 0.10 M sodium acetate solution. Calculate the volume of 1 M sodium hydroxide (NaOH) needed to prepare 10 mL of a 0.10 M sodium hydroxide solution. Calculate the volume of 1 M hydrochloric acid (HCl) needed to prepare 10 mL of a 0.10 M hydrochloric acid solution. Determine the volumes of 0.10 M CH_3COOH and 0.10 M CH_3COONa required to prepare 10 mL of the following pH buffers. a. pH 3.7 b. pH 4.7 c. pH 5.7 If asked to prepare a buffer solution at pH 4.6.which of the following acids and their conjugate base would be the best choice? Explain your answer Write a balanced equation for the dissociation equilibrium of acetic acid. In activity 2, there was 2 ml of buffer per Calculate the final pH of the undiluted buffer after 0.25 ml of 0.1 m NaOH are added. The K_a of CH_3COOH =1.8 times 10 ^-5.Use the CH_3COOH + NaOH reaction equation, an ICE table, and a balanced dissociation equilibrium equation to help determine your pH.
The pKa of acetic acid is 4.7. What is the buffering range of this acid and its conjugate base? Explain your answer. Calculate the volume of 6 M acetic acid needed to prepare 100 mL of a 0.10 M acetic acid (CH_3COOH) solution. Calculate the mass of sodium acetate (CH_3COONa) required to prepare 50 mL of a 0.10 M sodium acetate solution. Calculate the volume of 1 M sodium hydroxide (NaOH) needed to prepare 10 mL of a 0.10 M sodium hydroxide solution. Calculate the volume of 1 M hydrochloric acid (HCl) needed to prepare 10 mL of a 0.10 M hydrochloric acid solution. Determine the volumes of 0.10 M CH_3COOH and 0.10 M CH_3COONa required to prepare 10 mL of the following pH buffers. a. pH 3.7 b. pH 4.7 c. pH 5.7 If asked to prepare a buffer solution at pH 4.6.which of the following acids and their conjugate base would be the best choice? Explain your answer Write a balanced equation for the dissociation equilibrium of acetic acid. In activity 2, there was 2 ml of buffer per Calculate the final pH of the undiluted buffer after 0.25 ml of 0.1 m NaOH are added. The K_a of CH_3COOH =1.8 times 10 ^-5.Use the CH_3COOH + NaOH reaction equation, an ICE table, and a balanced dissociation equilibrium equation to help determine your pH.
Hubert KochLv2
4 Apr 2019