13.) You mix 44.0 mL of 0.070 M NaOH with 22.0ml of 0.14M benzoic acid (Ka=6.3x10^-5)....
13.) You mix 44.0 mL of 0.070 M NaOH with 22.0ml of 0.14M benzoic acid (Ka=6.3x10^-5). What molecules and ions exist in this solution? List them in order of decreasing concentration. To do this answer the following questions.
How many moles of C6H5CO2H were added to the mixture?
How many moles of NaOH was added to the mixture?
What is the prodominant solute present in solution after mixing the benzoic acid and NaOH solution?
A.) NaOH
B.) NaHCO2
C.) HCO2H
What is the concentration of benzoic acid in the solution following reaction with NaOH but before coming to equlibrilum?
Concentration= M
Homework Answers
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13.) You mix 44.0 mL of 0.070 M NaOH with 22.0ml of 0.14M
benzoic acid (Ka=6.3x10^-5)....
Calculate the pH of a 0.015 M solution of benzoic acid (C6H5CO2H) given that Ka =...
Calculate the pH of a 0.015 M solution of benzoic acid (C6H5CO2H) given that Ka = 6.3x10 for the acid. C6H5CO2H (aq) + H2O(l) C6H5CO2 (aq) + H20 (aq) 3P)CH PH =
A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH...
A 25.0 mL sample of 0.150 M benzoic acid is titrated with a 0.150 M NaOH solution. What is the pH after the addition of 13.0 mL of NaOH? The Ka of benzoic acid is 6.3x10-5.
1.) 20.00 mL of 0.11 M benzoic acid (C6H5COOH, Ka = 6.3x10-5) is titrated with 0.25...
1.) 20.00 mL of 0.11 M benzoic acid (C6H5COOH, Ka = 6.3x10-5) is titrated with 0.25 M NaOH. What volume of base is required to reach the equivalence point in the titration? 2.) Calculate pH at each of the following points in the titration. a) 4.00 mL b) 8.80 mL
25.00 mL of 0.150M benzoic acid HC7H5O2 was titrated with 0.200 M NaOH. Calculate the pH...
25.00 mL of 0.150M benzoic acid HC7H5O2 was titrated with 0.200 M NaOH. Calculate the pH at the following points. Ka for benzoic acid is 6.3x10-5 a. Before adding any NaOH b. Halfway to equivalence c. After adding 12.2 mL of the NaOH d. At the equivalence point Please answer all the parts!
A pH 4.88 buffer which was prepared by dissolving 0.10 mol of benzoic acid (Ka=6.3x10-5) and...
A pH 4.88 buffer which was prepared by dissolving 0.10 mol of benzoic acid (Ka=6.3x10-5) and 0.50 mol of sodium benzoate in sufficient pure water to form a 1.00 L solution. A 2.00 mL of 2.00 M HI solution was added to a 70.0 mL aliquot of this solution. a) What was the pH of the new 72.0 mL solution. b) If 0.01 mol A13+ is added to this new solution, will Al3+ ion be separated as Al(OH)3(s) (Ksp =...
A mixture contains 0.250 M benzoic acid, a monoprotic acid (Ka = 6.28 × 10‒5), and...
A mixture contains 0.250 M benzoic acid, a monoprotic acid (Ka = 6.28 × 10‒5), and 0.400 M sodium benzoate. How many mL of a HCl solution whose pH is 0.523 should be added to 500 mL of this buffer to change its pH from what it is to pH = 4.20?
Given the following information: hypochlorous acid HCIO CoH3COOH Ka = 3.5x10-8 Kg = 6.3x10-5 benzoic acid...
Given the following information: hypochlorous acid HCIO CoH3COOH Ka = 3.5x10-8 Kg = 6.3x10-5 benzoic acid (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.246 M aqueous hypochlorous acid and sodium benzoate are mixed. It is not necessary to include states such as (aq) or (s). (2) At equilibrium the will be favored. (3) The pH of the resulting solution will be _ seven. Submit Answer
A mixture contains benzoic acid, a monoprotic acid (Ka = 6.28 x 10-5, 0.250 M), and...
A mixture contains benzoic acid, a monoprotic acid (Ka = 6.28 x 10-5, 0.250 M), and sodium benzoate (0.400 M). 500 mL of this buffer were treated with 250 mL of a NaOH solution whose pH was 12.875. What should the pH be after addition of the base?
parts d and e please Assume that you dissolve 0.235 g of the weak acid benzoic...
parts d and e please
Assume that you dissolve 0.235 g of the weak acid benzoic acid, C.H.COOH, in enough water to make 1.00×10 mL of solution and then titrate the solution with 0.108 M NaOH. Benzoic acid is a monoprotic acid. Ka = 6.3x10-5 1. What is the pH of the original benzoic acid solution before the titration is started? pH= 2.96 A. How many moles of acid do you have? _1.9x108__moles B. What is the initial molarity of...
Titrate 40.0 mL of 0.0350 M benzoic acid (C6H5COOH, Ka = 6.3 × 10–5) with 0.0700...
Titrate 40.0 mL of 0.0350 M benzoic acid (C6H5COOH, Ka = 6.3 × 10–5) with 0.0700 M NaOH Calculate the pH in the solution at equivalent point. a) 5.716 b) 8.284 c) 8.372 d) 5.628 e) 7.546
Calculate the pH of a 0.015 M solution of benzoic acid (C6H5CO2H) given that Ka = 6.3x10 for the acid. C6H5CO2H (aq) + H2O(l) C6H5CO2 (aq) + H20 (aq) 3P)CH PH =
A pH 4.88 buffer which was prepared by dissolving 0.10 mol of benzoic acid (Ka=6.3x10-5) and 0.50 mol of sodium benzoate in sufficient pure water to form a 1.00 L solution. A 2.00 mL of 2.00 M HI solution was added to a 70.0 mL aliquot of this solution. a) What was the pH of the new 72.0 mL solution. b) If 0.01 mol A13+ is added to this new solution, will Al3+ ion be separated as Al(OH)3(s) (Ksp =...
Given the following information: hypochlorous acid HCIO CoH3COOH Ka = 3.5x10-8 Kg = 6.3x10-5 benzoic acid (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.246 M aqueous hypochlorous acid and sodium benzoate are mixed. It is not necessary to include states such as (aq) or (s). (2) At equilibrium the will be favored. (3) The pH of the resulting solution will be _ seven. Submit Answer
parts d and e please
Assume that you dissolve 0.235 g of the weak acid benzoic acid, C.H.COOH, in enough water to make 1.00×10 mL of solution and then titrate the solution with 0.108 M NaOH. Benzoic acid is a monoprotic acid. Ka = 6.3x10-5 1. What is the pH of the original benzoic acid solution before the titration is started? pH= 2.96 A. How many moles of acid do you have? _1.9x108__moles B. What is the initial molarity of...
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