1. Acetate buffers are used in biochemical studies of enzymes and other chemical components of cells to prevent pH changes that might change the biochemical activity of these compounds. (Ka 1.8 x 105) a) Calculate the pH of an acetate buffer that is a mixture with 0.20M acetic acid and 0.20M sodium acetate b) Calculate the pH after 2.0 mL of 0.10M NaOH is added to 100.0mL of this buffer, giving a solution with a volume 101.0m L.

1. Acetate buffers are used in biochemical studies of enzymes and other chemical components of cells to prevent pH changes that might change the biochemical activity of these compounds. (Ka 1.8 x 105) a) Calculate the pH of an acetate buffer that is a mixture with 0.20M acetic acid and 0.20M sodium acetate b) Calculate the pH after 2.0 mL of 0.10M NaOH is added to 100.0mL of this buffer, giving a solution with a volume 101.0m L.

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...

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8. You will perform some calculations to see the difference between a pH buffer solution and a weak acid solution of the same pH when a small amount of strong base is added. Chlorous acid, HClO2, is a moderately strong acid with a Ka 1.110×10-². Please answer the following questions. A. = B. What is the molarity of the HClO2 solution whose pH is 2.38? M Please provider your answer below. 3.76E-5 Check answer A 仁 To prepare a buffer solution of the same pH, what is the molarity of the NaClO₂ if the molarity of the HClO2 is 0.6013 M? M Please provider your answer below. 0.₂ Check answer → $ $
You have 1.5 liter of solution that is composed of 8.88 grams of NH3 and 11.33 grams of ammonium chloride mixed well. Kb for ammonia =1.8 x 10^-5 (A) is this a buffer solution? Why or why not? (B)if it is a buffer solution, what is the pH of this buffer solution? (C)how many mL of 1.50 M HCl can be added to this solution before the buffer is exhausted (d) how many mL of 1.5 M NaOH can be added to this solution before the buffer is exhausted?
7. The pH titration curve of a weak acid, HA, is shown me below. As the titration progresses, HA is converted into its conjugate base, A-. 12 10 8 (a) What is the volume of NaOH at the equivalence point? 2 25 30 35 15 20 volume of NaOH added (mL) 5 10 (b) At what volume (or volumes) is all of the acid present in the protonated (HA) form? (c) At what volume (or volumes) is all of the acid present in the conjugate base (A') form? (d) At what point along the titration will half the original amount of HA have been converted to A-?
1. How do you prepare a 100mL of 0.1 M phosphate buffer?To make 100 mL of 0.1 M phosphate buffer: Calculate the amount of sodium phosphate needed. moles of sodium phosphate = (0.1 mol/L) x (0.1 L) = 0.01 moles mass of sodium phosphate = moles x molar mass = 0.01 moles x 142 g/mol = 1.42 g Dissolve 1.42 g of sodium phosphate in distilled water in a 100 mL volumetric flask. Adjust the pH of the solution to the desired value (usually around 7.4) using a strong acid or strong base. Bring the solution to the final volume (100 mL) with distilled water. 2. From the anterior buffer, how do you make 100mL of 0.05 M? To make 100 mL of 0.05 M phosphate buffer from the 0.1 M stock solution: Calculate the amount of the 0.1 M phosphate buffer needed. moles of phosphate buffer = (0.05 mol/L) x (0.1 L) = 0.005 moles Calculate the volume of the 0.1 M phosphate buffer needed. moles = concentration x volume (in liters) volume = moles / concentration = 0.005 moles / 0.1 mol/L = 0.05 L or 50 mL Measure…
7. A solution was made by mixing 50.0 mL of 0.750 M HCN with 25.0 mL of water. What is the pH of this solution? The pka of HCN = 9.31. 8. One of the compounds featured on the TV series "Breaking Bad" was hydrofluoric acid (HF), pKa = 3.14. a) A solution of HF has a pH = 1.77. What was the initial [HF] for this solution in mol L-1? b) What is the equilibrium concentration of F in this solution in mol L-1? c) What is the percent ionization of HF in this solution?
4. What is the pH of a buffer made from 0.42 M H3BO3 and 0.22 M H2BO3-, if the Ka for H3BO3 is 7.3 x 10-10 ? (use 2 decimal places for pH)
A student prepared 100.0 mL of a buffer in the lab that contains 0.300 M of a weak acid, HA, and 0.200 M of its conjugate base, NaA. The student then added 1.0x10 moles of NaOH to the buffer. a) Write down your student name and number b) Write down how the student calculated the final moles of A and HA after adding the NaOH: moles A finl =2.0x102 mole - 1.0x10-3mole moles HA na = 3.0x102mole +1.0x10-3mole c) There is an error in their formula. Identify the error d) Calculate the correct final moles of A and HA
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Sketch the following titrations. Clearly mark the equivalent point, appropriate x-axis titles on each graph: a) the titration of a strong acid (flask) with a strong base (buret) b) the titration of a week acid with a strong base c) the titration of a weak base with a strong acid
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