5.Which substance would be the best buffer at pH 7.6 if it had to be able to buffer against either acid or base? A. one with a pKa of 5.6 B. one with a pKa of 7.6 C. one with a pKa of 9.6 D. The pKa of a substance doesn't tell you whether it would be a good buffer at this pH. 6. For the following reaction, which of the following is true? A B AG = +15.9 A. The conversion of A to B is spontaneous B. The conversion of A to B is exergonic C. Both A and B D. Neither A nor B

5.Which substance would be the best buffer at pH 7.6 if it had to be able to buffer against either acid or base? A. one with a pKa of 5.6 B. one with a pKa of 7.6 C. one with a pKa of 9.6 D. The pKa of a substance doesn't tell you whether it would be a good buffer at this pH. 6. For the following reaction, which of the following is true? A B AG = +15.9 A. The conversion of A to B is spontaneous B. The conversion of A to B is exergonic C. Both A and B D. Neither A nor B

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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Ag+(aq)+e-→Ag(s) 0.800 Al3+(aq)+3e-→Al(s) -1.676 Au+(aq)+e-→Au(s) 1.692 Au3+(aq)+3e-→Au(s) 1.498 Ba2+(aq)+2e-→Ba(s) -2.912 Be2+(aq)+2e-→Be(s) -1.847 Br2(l)+2e-→2Br-(aq) 1.066 Ca2+(aq)+2e-→Ca(s) -2.868 Cd2+(aq)+2e-→Cd(s) -0.403 Ce4+(aq)+e-→Ce3+(aq) 1.72 Cl2(g)+2e-→2Cl-(aq) 1.358 Co2+(aq)+2e-→Co(s) -0.28 Co3+(aq)+e-→Co2+(aq) 1.92 Cr2+(aq)+2e-→Cr(s) -0.913 Cr3+(aq)+e-→Cr2+(aq) -0.407 Cr3+(aq)+3e-→Cr(s) -0.744 CrO42-(aq)+4H2O(l)+3e-→Cr(OH)3(s)+5OH-(aq) -0.13 Cr2O72-(aq)+14H+(aq)+6e-→2Cr3+(aq)+7H2O(l) 1.36 Cu+(aq)+e-→Cu(s) 0.521 Cu2+(aq)+e-→Cu+(aq) 0.153 Cu2+(aq)+2e-→Cu(s) 0.342 F2(g)+2e-→2F-(aq) 2.866 Fe2+(aq)+2e-→Fe(s) -0.447 Fe3+(aq)+e-→Fe2+(aq) 0.771 Fe3+(aq)+3e-→Fe(s) -0.037 2H+(aq)+2e-→H2(g) 0.000 2H2O(l)+2e-→H2(g)+2OH-(aq) -0.828 H2O2(aq)+2H+(aq)+2e-→2H2O(l) 1.776 Hg2+(aq)+2e-→Hg(l) 0.851 2Hg2+(aq)+2e-→Hg22+(aq) 0.92 Hg22+(aq)+2e-→2Hg(l) 0.797 I2(s)+2e-→2I-(aq) 0.536…
What is the ratio of [A] / [HA] for a buffer solution of HA with a pH of 7 if the pK₂ = 5 for HA? O A. 0.01 O B. 10 O C. 0.1 D. 100
What is the pH of a buffer made with NH3 ( 0.200M) and NH4Cl (0.300M).Ka NH4+ = 5.68 x 10 -10 ( pH = pKa + log Base/Acid) Select one: a. 9.25 b. 9.07 c. 4.58 d. 4.75 e. 7.00
What is the pH after .03 mol of OH is added to 1.0 L of a buffer containing .05 mol of NH4* and .07 mol of NH3 ? - Pb2+ 1. .034 M .079 M Br I- O 8.55 Ο 10.86 8.95 O 9.40 O 9.95
Consider the list of acids and their pKa values attached What mass ratio of sodium salt to acid is needed to prepare this buffer?
4. An acetic acid-acetate buffer contains 0.200 M CH3CO2H and 0.200 M NaCH3CO2. If 0.050 M NAOH is added to the buffer solution, what is the final pH of the solution? (CH3CO2H's Ka = 1.8 x 10-5) %3D (pH = pKa + log{[Base]/[Acid]}) %3D
Name Formula Ka Kb Nitrous acid HNO2 1.4 x 10–11 Hypochlorous acid HClO 3.0 x 10–8 Phenol C6H5OH 9.52 x 10–5 Benzoic Acid C6H5COOH 6.28 x 10–5 Which of the following compounds could be used to create a buffer with a pH of 3.80? Nitrous acid Hypochlorous acid Phenol Benzoic acid 4 only 2 only 1 only 1 and 4 2 and 3
you have found the pKa to be 10.3. “Acid-free” paper should have a pH between 8.7 and 10.2. What is the pH of the buffer in your paper pulp if you add 0.581 mM calcium carbonate to pulp that started with 0.452 mM acid (pH=3.37)?
A buffer is formed by dissolving 0.105 moles of HCIO, hypochorous acid; and 0.115 moles of NaCIO, sodium hypochlorite; in 200 ml of water. Ka 3.0 X 10-8. a) Find the pH of the buffer. b) How does the pH compare with the pka? c) How much does the pH change when 2.00 ml of 0.50 M NaOH is added to the buffer? d) What would be the pH change if 2.00 ml of 0.50 M NaOH was added to 200 ml of pure H2O? e) How does this pH change compare to the addition of the same amount of 0.50 M NaOH to the buffer solution (as in c)?
Given 100.0 mL of a buffer that is 0.50 M in HOCI and 0.60 M in NaOC1, what is the pH after 20.0 mL of 1.0 M NaOH has been added? (K ₂ for HOCI=3.5 × 10-8) a a. 7.55 O b.7.46 O c. 7.70 O d. 7.88 e. 7.63
Kk.94.
Which of the following acids would you use to make a buffer with a pH of 3.00? a. Nitrous acid (Ka = 7.2*10-4) b. Monobasic sodium citrate (Ka2 = 1.7*10-5) c. Ascorbic acid (Ka = 8.0*10-5) d. Hypochlorous acid (Ka = 3.0*10-8)