A chemistry graduate student Is glven 500. mL of a 1.60M propanolc acid (HC, H CO,) solutlon. Propanolc acid Is a weak acid with K =1.3x 10 -5 What mass of KC,H CO, should the student dissolve In the HC,H,CO, solutlon to turn it Into a buffer with pH =4.537 You may assume that the volume of the solution doesn't change when the KC,H.CO, Is dissolved In It. Be sure your answer has a unit symbol, and round It to

A chemistry graduate student Is glven 500. mL of a 1.60M propanolc acid (HC, H CO,) solutlon. Propanolc acid Is a weak acid with K =1.3x 10 -5 What mass of KC,H CO, should the student dissolve In the HC,H,CO, solutlon to turn it Into a buffer with pH =4.537 You may assume that the volume of the solution doesn't change when the KC,H.CO, Is dissolved In It. Be sure your answer has a unit symbol, and round It to

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 93QRT: When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence...

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Sketch two pH curves, one for the titration of a weak acid with a strong base and one for a strong acid with a strong base. How are they similar? How are they different? Account for the similarities and the differences.
Lactic acid (CH3CHOHCO2H) is found in sour milk, in sauerkraut, and in muscles after activity. (Ka for lactic acid = 1.4 104.) (a) If 2.75 g of NaCH3CHOHCO2, sodium lactate, is added to 5.00 102 mL of 0.100 M lactic acid, what is the pH of the resulting buffer solution? (b) Is the pH of the buffered solution lower or higher than the pH of the lactic acid solution?
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
A buffer is made using 45.0 mL of 0.750 M HC3H5O2 (Ka = 1.3 105) and 55.0 mL of 0.700 M NaC3H5O2. What volume of 0.10 M NaOH must be added to change the pH of the original buffer solution by 2.5%?
Sketch a pH curve for the titration of a weak acid (HA) with a strong base (NaOH). List the major species, and explain how you would go about calculating the pH of the solution at various points, including the halfway point and the equivalence point.
Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain your answer. (i) [HA] =0.100 M = [A] (ii) [HA] = 0.300 M = [A]
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the acid.
2. If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? 100. mL 50. mL 36 mL 18 mL
a) What ratio of CH₃NH₂ to CH₃NH₃⁺ is needed to prepare a pH 10.20 buffer? (Kb for CH₃NH₂ is 4.4 × 10⁻⁴) b) What is the pH of a 1.0 L buffer made with 0.300 mol of HF (Ka = 6.8 × 10⁻⁴) and 0.200 mol of NaF to which 0.100 mol of HCl were added?
A. Sir Bong wants to prepare 2L of 5 mM benzoate buffer pH 5.00. The pKa for benzoic acid, C₆H₅COOH, is 4.20. 1. Identify the buffer components. 2. Give the equilibrium reaction involved. 3. Give the buffering action when the buffer system is added with (a) small amounts of a strong acid and (b) small amounts of a strong base. 4. What mass (in grams) of sodium benzoate (molar mass = 144 g/mol) is needed to prepare the said buffer? Report your answer up to 2 decimal places. Show your complete solution. 5. What mass (in grams) of benzoic acid (molar mass = 122 g/mol) is needed to prepare the said buffer? Report your answer up to 2 decimal places. Show your complete solution.
a. How many grams of dry NH4CI need to be added to 2.40 L of a 0.300 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.89? Kb for ammonia is 1.8×10^-5. b. What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of Na in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10^−7