Question

1. Briefly explain why the pH of 1.0 x 10^-2M HCl is different from that of 1.0 x 10^-2M HC2H3O2. pH = -log[H+] HCl is strong acid. HC2H3O2 is weak acid. They have different pH due to different[H+] 2. (a) Calculate the percent error in your experimentally determined Ka's for the HC2H3O2 solutions in Part III, using Equation 20. percent error, % = ((calculated Ka - literature Ka) / literature Ka) (100%) (Eq. 20) (b) Are the magnitudes of your percent errors random, or do you see a pattern? Briefly explain. 3. Briefly explain why the pH change that resulted when you added 6M NaOH to the buffer solution was of a different magnitude than the pH change that resulted when you added aqueous NaOH to distilled water. 4. (a) Write the chemical equation for the reaction that occurred when you added 6M NaOH to the buffer solution. (b) Write the chemical equation for the reaction that occurred when you added 6M HCl to the buffer solution.

          1. Briefly explain why the pH of 1.0 x 10^-2M HCl is different from that of 1.0 x 10^-2M HC2H3O2. pH = -log[H+] HCl is strong acid. HC2H3O2 is weak acid. They have different pH due to different[H+] 2. (a) Calculate the percent error in your experimentally determined Ka's for the HC2H3O2 solutions in Part III, using Equation 20. percent error, % = ((calculated Ka - literature Ka) / literature Ka) (100%) (Eq. 20) (b) Are the magnitudes of your percent errors random, or do you see a pattern? Briefly explain. 3. Briefly explain why the pH change that resulted when you added 6M NaOH to the buffer solution was of a different magnitude than the pH change that resulted when you added aqueous NaOH to distilled water. 4. (a) Write the chemical equation for the reaction that occurred when you added 6M NaOH to the buffer solution. (b) Write the chemical equation for the reaction that occurred when you added 6M HCl to the buffer solution.

1. Briefly explain why the pH of 1.0 x 10^-2M HCl is different from that of 1.0 x 10^-2M HC2H3O2. pH = -log[H+] HCl is strong acid. HC2H3O2 is weak acid. They have different pH due to different[H+] 2. (a) Calculate the percent error in your experimentally determined Ka's for the HC2H3O2 solutions in Part III, using Equation 20. percent error, % = ((calculated Ka - literature Ka) / literature Ka) (100%) (Eq. 20) (b) Are the magnitudes of your percent errors random, or do you see a pattern? Briefly explain. 3. Briefly explain why the pH change that resulted when you added 6M NaOH to the buffer solution was of a different magnitude than the pH change that resulted when you added aqueous NaOH to distilled water. 4. (a) Write the chemical equation for the reaction that occurred when you added 6M NaOH to the buffer solution. (b) Write the chemical equation for the reaction that occurred when you added 6M HCl to the buffer solution.

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