Your goal is to make a buffer with a pH of 4.95 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of acetic acid added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.

Your goal is to make a buffer with a pH of 4.95 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of acetic acid added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A technician is adding 50 ml of 1M NaOH to 2000 ml of a 150 mM solution of the carbonic acid buffer that had an initial pH 8.9. They know that at the initial pH the concentration of weak acid was 0.143 M and the concentration of conjugate base was 0.007 M. What pH will the resulting final solution have? Show all details of your working out for each individual mathematical manipulation that you do apply (skipping steps will receive a deduction). The calculation must be presented such that it can be recapitulated by the marker. In each step of your working out use the chemical formulas of the compounds that constitute the weak acid and conjugate base. Provide the final pH to 1 decimal place, make sure to round the result accordingly. State the final answer in a complete sentence.
A buffer contains the weak acid HA and its conjugate base A−. The weak acid has a pKa of 5.25 and the buffer has a pH of 5.58. Which statement is true of the relative concentrations of the weak acid and the conjugate base in the buffer? Group of answer choices [HA] < [A−] [HA] > [A−] [HA] = [A−]
Which of the following acids (listed with Ka values) and their conjugate base should be used to form a buffer with a pH of 2.34? Group of answer choices HClO2, Ka = 1.1 × 10-2 HIO, Ka = 2.3 × 10-10 HCN, Ka = 4.9 × 10-10 C6H5OH, Ka = 1.3 × 10-10 HN3, Ka = 2.5 × 10-5
A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Determine the value of Ka for the weak acid. Show ICE table and show set up of Ka expression.
Calculating the pH at equivalence of a titration A chemist titrates 50.0 mL of a 0.5851 M ethylamine (C2H5NH2) solution with 0.8192M HBr solution at 25 °C. Calculate the pH at equivalence. The pK of ethylamine is 3.19. b Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of HBr solution added. pH = ] ☑
ou need to produce a buffer solution that has a pH of 5.03. You already have a solution that contains 10. mmol (millimoles) of acetic acid. How many millimoles of acetate (the conjugate base of acetic acid) will you need to add to this solution? The pKa of acetic acid is 4.74. Express your answer in millimoles.
What is the proper unit of molar ratio of weak acid and its conjugate base in a buffer solution? Is it mol to mol or part to part? Or is it unitless? I need to express the answer 1.45/1 = [A]/[HA] to the right unit. See image for more details. the buffer is acetic acid/sodium acetate buffer.
Please explain your reasoning, thank you! 75.0 mL of 1.35 M base, B, is titrated with 1.25 M hydrochloric acid, HCl. Kb(B) = 2.25×10-6. Determine the pH after 50.0 mL of HCl have been added. Be sure to express the correct reaction(s) and show all of your work. You may assume the initial concentration of conjugate acid is zero.
How many grams of sodium acetate (CH3CO2Na, Mw =82.0 g/mole) should be present in 1.0 L of 0.65 mole acetic acid (CH3CO2H) solution to achieve a buffer of pH = 4.47? K = 1.78 × 10 for benzoic acid. Please keep your answer to one decimal place.
How would you create a buffer solution at a pH of your choosing (between pH 4-6) by adding solid sodium acetate to 50mL of 0.1M acetic acid? Use the Henderson-Hasselbalch equation to calculate the mass of sodium acetate that you will need to produce this acetate buffer (K, = 1.75 x 10-5). Make a note of your chosen pH and the mass of sodium acetate that you will need in part 4 in the "procedure and data" section before turning in your pre-lab assignment.
You are asked to make a buffer of pH 3.4 and given the above acids. Of these acids, which would create a buffer with the best capacity against acids? Which would have the best buffering capacity against bases? Which could not be used at all for this project? Best against acids Best against bases Acid #1 has a pka of 3.15 Acid #2 has a pKa of 3.65 Acid #3 has a pKa of 4.23 Acid #4 has a pka of 4.79 Cannot be used Acid #2 Acid #1 Acid #4
Determine the quantity of sodium acetate (CH3COONa) needed to create buffer solution at a particular pH. Do this by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the mass of starting material required. Complete Parts 1-3 before submitting your answer. NEXT > Sodium acetate (CH3COONa) is added to an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.000. Let x represent the concentration of CH3COO in the water after the addition of CH3COONa. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) CH3COOH(aq) + 0.200 1.0 x 10-² -1.0 x 10-5 -1.8 x 10-5 x+1.0 × 105x-1.0 × 10-5x+1.8 × 10-5x-1.8 × 10- [0] 0 [x - 5.00] [500.0] x 1.8 x 10-5 1 [x+1.0 x 10] Question 4 of 23 Ka = [0.200] H₂O(l) [x-1.0 x 10] 2 Determine the quantity of sodium acetate (CH3COONa) needed to create buffer…