A student researcher added 50 mL of 0.01 M sodium hydroxide to 100 mL of 0.05 phosphate buffer atpH 7.2. Determine the pH of the resulting solution.a. Determine the concentrations of H2PO, and HPO,2- in the final solution

Buffer are solution which resist change in PH when acid or base are added The pH the buffer…

Answered: A student researcher added 50 mL of…

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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a. What is the pH of a buffer solution that is 0.12 M NH3 and 0.12 M NH4+? К, for NH3 is 1.8 x 10-5. pH b. What is the pH if 37 mL of 0.24 M hydrochloric acid is added to 555 mL of this buffer? pH
A buffer solution is composed of 1.324 g of KH,PO4 and 4.362 g of Naz HPO4. (K, for dihydrogen phosphate ion is 6.2 × 10-8.) a. What is the pH of the buffer solution? pH = b. What mass of KH;PO4 must be added to decrease the buffer solution pH by 0.10 unit from the value calculated in part a? Mass =
HCL Solution-- 20 mL HCl with 25.46 mL of 0.1240 M NaOH
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Consider the titration of a 40.0 mL of 0.211 M weak acid HA (Ka = 2.7 x 10⁻⁸) with 0.100 M LiOH. c. How many mL of the LiOH would be required to reach the halfway point of the titration? d. What is the pH of the solution at the equivalence point? e. What would be the pH of the solution after that addition of 100.0 mL of LiOH?
A 25.00 mL sample of 0.280 M LiOH is titrated with 0.750 M HCl at 25 °C. a. Calculate the initial pH before any titrant is added b. Calculate the pH of the solution after 5.00 mL of the titrant is added.
1.0.20 mol of KOH is added to 1.00 L of a solution that contains 0.50 M HC3H5O2 (Ka = 1.3 x 10) and 1.00M NaC3H5O2. a. Write the balanced net ionic equation for the reaction that occurs. b. Determine the pH of the solution after the reaction. Assume the addition of KOH did not change the volume.
6. A buffer solution contains 0.120 moles of propionic acid, HC3H502, and 0.100 moles of sodium propionate, NaC3H5O2, in 1.00 L of solution. Ka = 1.32 x 10-5 a. What is the pH of this buffer? b. What is the pH of this buffer after the addition of 0.010 mol of NaOH? c. Beginning with the initial buffer from part a, what is the pH of the buffer after the addition of 0.010 mol of HBr?
A sample weighing 1.25 g of the diprotic acid potassium acid phthalate (KHP) is dissolved in 50.0 ml of water. Consider the titration of this solution with 0.100 M NaOH. The two Ka's for KHP are 1.12 x 10¯3 and 3.90 x 10 a. Calculate the pH of this solution before adding any NaOH. b. How many ml of NaOH must be added to reach the equivalence point? What is the pH at the equivalence point? c. Calculate the pH of the solution after 100. ml of NaOH have been added.
5. A common buffer solution can be prepared by using ammonia and ammonium salts. The base equilibrium constant is 1.815×10-5. A student is preparing a pH buffer solution with 2.561 M NH3 solution and (NH4)2SO4 solid. Please answer the following questions. A. B. What is the best pH buffer range of the buffer solution that can be prepared by NH3 solution and (NH4)2SO4 solid? Please put down "1" if the answer is pH = 4.741 ± 1, please put down "2" if the answer is pH = 4.741 ± 10, please put down "3" if the answer is pH = 9.26 ± 1, please put down "4" if the answer is pH = 9.26 ± 10. Your answer follows. Assume that the addition of the solid will NOT change the volume, how many grams of is needed to prepare a pH = 8.66 buffer solution? The volume of the buffer solution is 250.0 mL. grams
a. Determine the pH change when 0.100 mol KOH is added to 1.00 L of a buffer solution that is 0.452 M in HClO and 0.357 M in ClO-.pH after addition − pH before addition = pH change= ? b. A buffer solution contains 0.387 M CH3NH3Br and 0.409 M CH3NH2 (methylamine). Determine the pH change when 0.084 mol HI is added to 1.00 L of the buffer.pH after addition − pH before addition = pH change = ? c. Determine the pH change when 0.057 mol HI is added to 1.00 L of a buffer solution that is 0.414 M in HF and 0.229 M in F-.pH after addition − pH before addition = pH change =?
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A student researcher added 50 mL of 0.01 M sodium hydroxide to 100 mL of 0.05 phosphate buffer at pH 7.2. Determine the pH of the resulting solution. a. Determine the concentrations of H2PO4 and HPO2 in the final solution