Example 5Find the pH of 0.10 M H₂His²+, 0.10 M H₂His+, 0.10 M HHis, 0.10 MHis, where His stands for the amino acid histidine (pKa=1.60,pKa2=5.97, pKa=9.28)0.10 M H3His²+: Treat it as a monoprotic acidal

Answered: Example 5 Find the pH of 0.10 M…

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

We dissolve 0.612 mol of a weak acid, HA, and 12.0 g of NaOH in enough water to produce 1.00 L of solution. The final pH of this solution is 4.62. What is the dissociation constant, Ka, of HA? The temperature is 25.0°C. Your Answer: Answer
Calculate the ratio [CH3COOH]/[NaCH3COO] that gives a solution with pH = 5.00? Hint: Rearrange the Hendersen-Hasselbach equation to solve pH = pka + log [base]/[acid] The Ka of CH3COOH is 1.8x10-5
A 1.083 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES¯K†, MW = 220.29 g/mol) is dissolved in 82.92 mL of water.To the solution, 11.64 mL of HCl is added, resulting in a pH of 6.58. Calculate the concentration of the HCl solution. The pKą of ACES is 6.85. [HCI] = M
Sulfurous acid, H2SO3, is diprotic: pka1= 1.81, pka2= 6.91. Calculate the concentrations of all acid species: [ H2SO3 ], [ HSO3¯ ], [ SO3²- ], the pH and the pOH in a 1.9 mol L-1 solution of Sulfurous acid. [H₂SO3 ] = __ mol L-1, [HSO3¯ ] = __ mol L-1, [ SO3²- ] = __ pH = mol L-1, pOH =
Arrange the following acids in order of decreasing acid strength, 1 being the weakest and 4 being the strongest. 1 2 3 4 H₂S (pKa = 7.02) HCO3- (pka = 10.33) HF (pKa = 3.17) HPO4²- (pKa = 12.38) Which of these solutions will have the lowest pH? O 0.1 M acetic acid (pka = 4.76) 0.1 M HCN (pKa = 9.21) O 1 x 10-6 M HCl O 0.1 M NH3 (pKb = 4.76)
Find the pH of a 0.381 M aqueous solution of hypobromous acid (HOBr), for which Ka = 2.1 * 10-⁹. 9.45 5.11 8.89 4.55
What is the pH of 0.31 M diethylammonium chloride, (C2H5)2NH2Cl. The Kb of diethylamine, (C2H5)2NH, is 6.9 x 10-4.
Q1
Common aspirin is acetylsalicylic acid, which has the structure shown below and a pKa of 3.5. Calculate the pH of a solution in which one normal adult dose of aspirin ( 5.7×102mg ) is dissolved in 0.33 L of water. Express your answer to one decimal place.Common aspirin is acetylsalicylic acid, which has the structure shown below and a pKa of 3.5. Calculate the pH of a solution in which one normal adult dose of aspirin ( 5.7×102mg ) is dissolved in 0.33 L of water. Express your answer to one decimal place.
Malic acid is a weak diprotic organic acid with Ka1 = 4.0 × 10-4 and Ka2 = 9.0 × 10-5.a Letting the symbol H2A represent malic acid, write the chemical equations that represent Ka1 and Ka2 . Write the chemical equation that represents Ka1 × Ka2. b Qualitatively describe the relative concentrations of H2A, HA-, A2-, and H3 O+ in a solution that is about one molar in malic acid.c Calculate the pH of a 0.0175 M malic acid solution and the equilibriumconcentration of [H2 A].d What is the A2- concentrationin in solutions b and c?
Table: Name: Serine pka: 2.187 (CO2H) / 9.209 (NH3) Ka: 6.50*10^-3 (CO2H) / 6.18*10^-10 (NH3) a) What is the pH, along with the concentration of each form of serine, in a 0.020 0 M solution of serine hydrochloride? b) What is the pH, along with the concentration of each form of serine, in a 0.020 0 M solution of the sodium salt of serine? c) What is the pH, along with the concentration of each form of serine, in a 0.020 0 M solution of serine? d) Calculate the isoionic and isoelectric pH for 0.020 0 M serine.
3. Draw the two structures in most abundance of the amino acid, cysteine, at a pH of 8.0. What are their respective concentrations in a 50 mM solution? If you had 1.0 L of this solution, how much 3.0 M NaOH would be required to take the pH to 10.4? What two species are now in most abundance (draw the structures)?

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS

Example 5 Find the pH of 0.10 M H₂His²+, 0.10 M H₂His+, 0.10 M HHis, 0.10 M His, where His stands for the amino acid histidine (pKa=1.60, pKa2=5.97, pKa=9.28) 0.10 M H3His²+: Treat it as a monoprotic acid al