An unknown compound, X, is thought to have a carboxyl group with a pK₂ of 2.5 and a second ionizable group with a pKa between 5.0 and 8.0. When 50.0 mL of 0.2 M NaOH is added to 75.0 mL of a 0.2 M solution of X at pH 2.5, the pH increases to 7.13. Calculate the pK₂ of the second ionizable group of X. pK₂ = 6.97 Incorrect

An unknown compound, X, is thought to have a carboxyl group with a pK₂ of 2.5 and a second ionizable group with a pKa between 5.0 and 8.0. When 50.0 mL of 0.2 M NaOH is added to 75.0 mL of a 0.2 M solution of X at pH 2.5, the pH increases to 7.13. Calculate the pK₂ of the second ionizable group of X. pK₂ = 6.97 Incorrect

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

An enzyme-catalyzed reaction was carried out in 5.0 mL of 0.15 M phosphate buffer pH 7.2. As a result of the reaction, the pH of the solution increased to pH 7.4. How many moles of OH- were produced during the reaction? H2PO4- + H2O ⇆ HPO42- + H3O+, pKa = 7.2 The answer is 8.50 × 10-5 moles But how do you solve it?
An analytical chemist is titrating 161.4 mL of a 0.8000M solution of trimethylamine ((CH,) N) with a 0.8900M solution of HIO3. The p K, of trimethylamine 3 is 4.19. Calculate the pH of the base solution after the chemist has added 161.5 mL of the HIO, solution to it. 3. 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.
Piperazine can be used as an anthelmintic (a drug that expels parasitic worms from the body). It is a dibasic compound and has 2 pKb’s as shown below: Consider the titration of 50.00 mL of 0.05000 M piperazine is titrated with 0.1250 M HCl. What is the pH after 15.00 mL of HCl have been added?
Consider the following reaction:CH3COOH(aq) + OH-(aq) -----> CH3COO- (aq) + H2O(l) How much 5.90M NaOH must be added to 460.0 mL of a buffer that is 0.0210 M acetic acid and 0.0260 M sodium acetate to raise the pH to 5.75?
10 11 12 13 14 An analytical chemist is titrating 234.9 mL of a 0.2700M solution of ethylamine (C,H,NH,) with a 0.1500M solution of HNO2. The p K, of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 484.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH =| Submit Assignment Continue
What is the pH of a buffer solution made by adding 0.15 mole of lactic acid HC3H5O3 and 0.12 mole sodium lactate to enough water to make 1.0 L of solution? What is the concentration of the hydroxide ion in the solution? KA lactic acid = 1.4 x 10 - 4
A formic acid buffer solution contains 0.20 M HCOOHHCOOH and 0.25 M HCOO− . The pKa of formic acid is 3.75. What is the pH of the buffer?
What is the pH of a buffer solution prepared by dissolving 0.10 mol of sodium acetate (NaC2H3O2) and 0.2 mol of acetic acid (HC2H3O2) in enough water to give 1.00 L solution? Ka for acetic acid = 1.8 x 10-5 .
Suppose a biochemist has 10 mL of a 1.0 M solution of a compound with two ionizable groups at a pH of 7.60. She adds 10.0 mL of 1.0 M HCI, which changes the pH to 3.40. The pK, value of one of the groups is pK,= 3.90 and it is known that pK₂ is between 7 and 10. What is the exact value of pK₂? pK₂ = 7.1 Incorrect
Histidine has ionizable groups with pKa values of 1.8, 6.0, and 9.2, as shown below (His = imidazole group). A biochemist makes up 100 mL of a 0.100 M solution of histidine at a pH of 5.40. She then adds 40 mL of 0.10 M HCl. What is the pH of the resulting solution?
45.0 mL of a buffer solution contains 0.20 M CH₂COOH and 0.25 M CH₂COONa. What is the pH of the mixture after 18.0 mL of 0.45 M HCI is added to this buffer solution? Ka of CH₂COOH = 1.8 x 105.
Calculate the pH of a buffer prepared by dissolving 0.80 moles acetic acid (CH3COOH) and 0.40 moles of sodium acetate (CH3COONa) in enough water to make 1500 mL of buffer solution. The pKa for acetic acid is 4.74