A 100 ml of 0.100 M phosphate buffer solution with a pH of 8.10 is to be prepared by adding 1.00 M HCl(aq) to 20.0 mL of 0.500 M Na;PO4(ag) in a 100-mL volumetric flask, and diluting the solution with water to the 100-mL mark. How much of 1.00 M HCl(eg) is required to prepare the buffer solution? The pKa's for the three ionization steps of H3PO4 are: pKa1 = 2.16, pKa2 = 7.21, pKa3 = 12.32 O 1.14 mL O 11.1 mL O 6.23 mL O 7.84 mL

A 100 ml of 0.100 M phosphate buffer solution with a pH of 8.10 is to be prepared by adding 1.00 M HCl(aq) to 20.0 mL of 0.500 M Na;PO4(ag) in a 100-mL volumetric flask, and diluting the solution with water to the 100-mL mark. How much of 1.00 M HCl(eg) is required to prepare the buffer solution? The pKa's for the three ionization steps of H3PO4 are: pKa1 = 2.16, pKa2 = 7.21, pKa3 = 12.32 O 1.14 mL O 11.1 mL O 6.23 mL O 7.84 mL

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

In the titration of 70.0 mL of a 0.300 M HF with 0.300 M KOH, calculate the pH: (a) after 35.0 nL of the standard KOH solution has been added; and (b) after 80 mL of the standard KOH solution has been added. Ka for HF = 1.74 x10^5
In each of the following questions, assume that there is no volume change when HCl is added to water in part (a) or the phosphate buffer in part (c). (a) Calculate the pH when 0.091 moles of HCl are added to 1.000 liter of water. (b) What is the difference between the pH of pure water (pH 7.00) and the pH of the solution after HCl was added? (c) Calculate the pH when 0.091 moles of HCl are added to 1.000 liters of a buffer containing 0.352M KH2PO4 and 0.321 M K2HPO4. (d) The pH before the HCl was added is equal to 7.168. What is the difference between the pH before adding the HCl and after adding the HCl?
Calculate the pH of the following buffer solutions: (a) a solution made by dissolving 2.668 g KH2PO4 and 2.095 g K2HPO4 in water to give 200. mL of solution. Stepwise acid dissociation constants for phosphoric acid may be found in your textbook. (b) a solution made by mixing 35.00 mL 0.33 M NH2OH with 15.00 mL 0.27 M NH3OHCl. The base dissociation constant Kb is 6.60 x 10-9 for NH2OH. Assume that the final volume is the sum of the volunes of the two solutions that are mixed.
You are titrating 20.0mL sample of 0.131 M Ba(OH)2 with 0.350 M HCL. (a) What volume in mL of HCL solution is needed to reach the equivalence point? (b) What is the pH after 20.0ml of HCL have been added. (c) Sketch a titration curve for the above process. Label the axes and the points calculated in (a) and (b) above.
An analytical chemist is titrating 151.8 mL of a 0.1600M solution of piperidine (C,HNH) with a 0.5500M solution of HIO. The p K, of piperidine is 2.89. Calculate the pH of the base solution after the chemist has added 47.8 mL of the HIO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HIO, solution added. Round your answer to 2 decimal places. pH=
Calculate the change in pH when 9.00 mL of 0.100 M HCl(aq) is added to 100.0 mL of a buffer solution that is 0.100 M in NH, (aq) and 0.100 M in NH, Cl(aq). Consult the table of ionization constants as needed. ApH = 9.17 Calculate the change in pH when 9.00 mL of 0.100 M NaOH is added to the original buffer solution. ApH 9.32 0
When a 23.3 mL sample of a 0.379 M aqueous hypochlorous acid solution is titrated with a 0.407 M aqueous sodium hydroxide solution,(1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 32.5 mL of sodium hydroxide have been added?
A buffer, consisting of H₂PO4 and HPO42, helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. What is the pH of a soft drink in which the buffer ingredients are 6.50 g of NaH2PO4 and 8.00 g of Na2HPO4 per 355 mL of solution? The Ka of H₂PO4 is 6.20 x 10-8.
If 100.0 mL of 0.250 M HBr is titrated with 0.150 M KOH answer the following questions. What is the pH of the solution before the titration begins? How many milliliters of NaOH must be added to reach the equivalence point? HBr (aq) + KOH (aq)  KBr (aq) + H2O (l) What is the pH of the solution at the equivalence point? What is the pH of the solution when 30.0 mL of KOH has been added? What is the pH of the solution when 180.0 mL of KOH has been added?
A buffer solution is made that is 0.409 M H2S and 0.409 M in NaHS. If Ka1 for H2S is 1.00x10^-7, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.087 mol NaOH is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter.)
100.0 mL of a 0.200 M H3PO4(aq) solution is titrated with 325.0 mL of a 0.100 M NaOH(aq) solution. What is the pH of the titrated solution?
Can you help me answer the PH=