**Phosphoric acid is a triprotic acid** \((K_{a1} = 6.9 \times 10^{-3}, K_{a2} = 6.2 \times 10^{-8}, \text{and } K_{a3} = 4.8 \times 10^{-13})\).**To find the pH of a buffer composed of \(H_2PO_4^-\)(aq) and \(HPO_4^{2-}\)(aq), which \(pK_a\) value should be used in the Henderson–Hasselbalch equation?**- \(pK_{a1} = 2.16\)- \(pK_{a2} = 7.21\)- \(pK_{a3} = 12.32\)**Calculate the pH of a buffer solution obtained by dissolving 18.0 g of \(KH_2PO_4\)(s) and 34.0 g of \(Na_2HPO_4\)(s) in water and then diluting to 1.00 L.**\[ \text{pH} = \] [Text Box]

Answered: Image /qna-images/answer/183c1747-0fa0-4e93-b2ec-f34ed05a2e3b.jpg

Answered: Phosphoric acid is a triprotic acid…

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

15 The K₂ of oxalic acid (H₂C₂04) is 5.37 x 10-2. What is the pH of a buffer solution that is prepared from 0.0100 M H₂C2O4 and 0.0300 M sodium oxalate (Na HC204)? Place your answer in the box. Express your answer using only a number or numbers without text. Report your result in decimal notation and to the proper number of significant figures. All numbers are measured.
Which of the following statements is true about a 1-L buffer solution prepared by mixing 1.13 mol propionic acid (C2H5COOH) and 2.03 mol sodium propionate (C2H5COONA)? Ka(C2H5COOH) = 1.34 x 10-5. The pH of the above buffer solution is less than the pka of C2H5COOH. a. b. By adding water to dilute the above buffer solution, the pH of the buffer solution will decrease. O. The pH of the above buffer solution is greater than the pKą of C2H5COOH. By readjusting the amount of propionic acid and sodium propionate, we can prepare a buffer solution ´at pH = 8.00. %3D e. By adding water to dilute the above buffer solution, the pH of the buffer solution will increase.
A buffer contains the weak acid HA and its conjugate base A−. The weak acid has a pKa of 5.25 and the buffer has a pH of 5.58. Which statement is true of the relative concentrations of the weak acid and the conjugate base in the buffer? Group of answer choices [HA] < [A−] [HA] > [A−] [HA] = [A−]
Which of the following acids (listed with Ka values) and their conjugate base should be used to form a buffer with a pH of 2.34? Group of answer choices HClO2, Ka = 1.1 × 10-2 HIO, Ka = 2.3 × 10-10 HCN, Ka = 4.9 × 10-10 C6H5OH, Ka = 1.3 × 10-10 HN3, Ka = 2.5 × 10-5
What would be the molar ratio of cyanic acid (HCNO)/sodium cyanate (NaCNO) buffer having a pH of 4.80 ? [K a(HCNO) = 2.0 × 10 –4] 11.6 mol NaCNO to 1.0 mol HCNO 12.6 mol NaCNO to 1.0 mol HCNO None of the above 13.6 mol NaCNO to 1.0 mol HCNO 10.6 mol NaCNO to 1.0 mol HCNO
For humans to maintain the pH of their blood close to 7.4, the body uses three buffer systems: carbonate, phosphate and proteins. If the pH of the blood goes below 6.8 or above 7.8, death may result. Imagine you want to make a phosphate buffer in the lab that resembles the bloods phosphate buffer. You start by mixing 1.0 M NaH2PO4 and 0.50 M Na2HPO4. H2PO4- + H2O ⇌ HPO42- + H+ pKa= 7.21 From the reaction above indicate the weak acid and the conjugate base involved in making this buffer. Calculate the pH of the phosphate buffer solution. Provide your answer with 2 decimal places. If the pH calculated in b. was the blood pH of an actual patient, would you say this patient’s blood pH is in the normal range or are they suffering from alkalosis or acidosis?
A buffer solution contains 0.316 M CH3NH3 C1 and 0.315 M CH3NH2 (methylamine). Determine the pH change when 0.069 mol HBr is added to 1.00 L of the buffer. (Assume Kb (CH3NH2) = 4.2 × 10-4.) pH after addition - pH before addition = pH change
Phosphoric acid is a triprotic acid (?a1=6.9×10−3 M, ?a2=6.2×10−8 M, and ?a3=4.8×10−13 M). To find the pH of a buffer composed of H2PO4−(aq) and HPO2−4(aq), which pKa value would you use in the Henderson–Hasselbalch equation? 1. p?a1=2.16 2. p?a2=7.21 3. p?a3=12.32 Calculate the pH of a buffer solution obtained by dissolving 21.021.0 g KH2PO4(s) and 39.0 g Na2HPO4(s) in water and then diluting to 1.00 L. pH=?
A buffer with pH = 8.96 must be created. 8.90 g of the acid component of the best buffer system will be used, and the volume of the solution will be 1 L. Choose which is the best buffer system, then compute the mass of the salt or base component of the chosen system. Choices: HClO (Ka = 2.9 x 10-8 , 52.46 g/mol)& KClO (90.55 g/mol) NH3 (Ka = 5.65 x 10-10 , 17.031g/mol) &NH4Cl (53.491 gmol) CH3COOH (Ka = 1.77 x 10-5 , 60.052 g/mol) & CH3COOK (98.15 g/mol) HClO2 (Ka = 1.1 x 10-2 , 68.46 g/mol)) & KClO2 (106.55 g/mol)
Acetic acid has a Ka of 1.8 x 10¬º. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: A. [acetic acid] ten times greater than [acetate], B. [acetate] ten times greater than [acetic acid], and C. [acetate] = [acetic acid]. Match each buffer to the expected pH. Drag the appropriate items to their respective bins. • View Available Hint(s) Reset Help [acetate] ten times greater than [acetic acid] [acetate] = [acetic acid] [acetic acid] ten times greater than [acetate] pH = 3.74 pH = 4.74 pH = 5.74
What is the [H3O+] and the pH of a benzoic acid-benzoate buffer that consists of 0.13 M C6H5COOH and 0.30 M C6H5COONa? (Ka of benzoic acid = 6.3 × 10−5) Be sure to report your answer to the correct number of significant figures. [H3O+] = ___× 10___MpH =____
a) Calculate the pH of a solution containing 0.30 M HF and 0.30 M NaF.The Ka for HF is 7.2×10-4. pH = b) Carbonate buffers are important in regulating the pH of blood at 7.40. If the carbonic acid concentration in a sample of blood is 0.0014 M, determine the bicarbonate ion concentration required to buffer the pH of blood at pH = 7.40. Ka = 4.3×10-7 Сoncentration = M c) You have 75.0 mL of 0.10 M HA. After adding 30.0 mL of 0.10 M NaOH , the pH is 5.50. What is the Ka value of HA ? = d) Consider the titration of 80.0 mL of 0.100 M Ba(OH)2 by 0.400 M HCl. Calculate the pH of the resulting solution after the following volumes of HCl have been added. 40.0 mL pH = 50.0 mL pH =

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