8. A solution is prepared by dissolving 0.020 moles of solid NaBr into 1.0 L of 0.020 M HBr. What statement is true for this solution? A. The solution is an acidic buffer with a high buffer capacity. B. The solution is a basic buffer with a high buffer capacity. C. The solution is an acidic buffer with a low buffer capacity. D. The solution is a basic buffer with a low buffer capacity. E. The solution is not a buffer.

8. A solution is prepared by dissolving 0.020 moles of solid NaBr into 1.0 L of 0.020 M HBr. What statement is true for this solution? A. The solution is an acidic buffer with a high buffer capacity. B. The solution is a basic buffer with a high buffer capacity. C. The solution is an acidic buffer with a low buffer capacity. D. The solution is a basic buffer with a low buffer capacity. E. The solution is not a buffer.

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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Similar questions

Among the given choices below, what is the best basis for choosing the right indicator for a given acid-base titration process? a. The identity of the base in the titration process b. The molarity of the acid or the base c. The pH at the equivalence point of the titration process d. The identity of the acid in the titration process
When titrating a strong acid with a strong base, the equivalence point is reached when: Select one: a. The pH indicator changes color. b. The amount of base added is exactly enough to react away all of the acid. c. The pH is determined solely by the amount of acid originally present. d. The pH is determined solely by excess base after all the acid has been neutralized.
John needs to create a buffered solution at a pH of 3.5 for his biomedical laboratory. a. Using the chart below, determine the appropriate acid for this application. Acid pk, Phosphoric 2.12 Pyruvic 2.49 Lactic 3.86 Benzoic 4.19 b. Research and state the conjugate base of the the acid. c. Describe how John would determine the amounts of acid and base needed to create the buffered solution.
Consider an ammonium buffer (NH4+). Which species would react if an external acid, H3O+ were added? a. NH3 b. NH4+ c. H3O+
2. What is the role of buffer in: a. pH b. buffering capacity c. pka and Henderson and Hasselbach equation
16. Which of the following will form a buffer? a. A mixture of HCIO (aq) and HCIO, (aq) b. A mixture of HCN (aq) and KCN (aq) c. A mixture of NaC,H,O, (aq) and KC,H,O, (aq) d. 10 (aq) with slowly added NaOH e, HNO, (aq) with slowly added HCI
11. What effect will addition of excess of HCI have on the pH of a solution of NH3? a. increase the pH b. decrease the pH C. no effect d. cannot tell from information given > Answer and brief explanation: 12. A buffer solution may be a mixture of a. a weak acid and its salt b. a weak base and its salt C. an excess of a weak acid with a strong base d. all of the above > Answer and brief explanation: 13. The ammonium ion would be classified as a Bronsted a. acid b. base > Answer and brief explanation:
C. increases by one A. decreases by one B. decreases by one tenth In a solution, when the concentrations of a weak acid and its conjugate base are equal, A. the system is not at equilibrium. D. increases ten fold B. the buffering capacity is significantly decreased. C. the -log of the [H*] and the -log of the K, are equal. D. all of the above are true. p. Consider a solution which is 0.10M in CH3COOH and 0.20 M in NaCH;COO. Which of the following statements is TRUE?
the sodium acetate - acetic acid buffer keep the pH: a. =4.8 b. = 8.9 C. = 1.8 O d. = 7.7
Look up the formula of the following compounds often found in buffers:a. acetic acidb. sodium acetatec. phosphoric acidd. monopotassium phosphate (also known as potassium dihydrogen phosphate)e. dipotassium phosphate
In weak acid-weak base titration, the equivalence point is a. above pH 7 b. at pH 7 c. bellow pH 7 d. all of above
Which of the following systems will form (a) buffer solution(s)? A.NaHSOA/H25OA B. Na2HAsOA / NaH2AsO4 C. NaH2AsOA / Na2AsO4 D.All three given form buffer solutions.