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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2. What is the role of buffer in: a. pH b. buffering capacity c. pka and Henderson and Hasselbach equation
define the buffer capacity. a) buffer capacity is the amount of acid that can be added until all of the acid is used up b) buffer capacity is the amount of base that can be added until all of the base is used up c) buffer capacity is the amount of acid that can be added until all of the base is used up d) buffer capacity is the amount of acid ir base that can be added to a buffer without destroying its effectiveness e) buffer capacity is the amount of base that can be added until all of the acid is used up
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
Which of the following insoluble salts are more soluble in a 0.10 hydrochloric acid solution than in a pure water solution? Chose all that apply a. Nickel (II) sulfide b. barium fluoride c. lead chloride d. lead bromide e. calcium fluoride f. silver sulfite
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:
Question is attached.
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?
Which one of the following statement is correct? a. Lewis acids include molecules or atoms that have octet deficiency. b. In a given reaction, the position of equilibrium favors the formation of strong acid and strong base. c. Dilution increases the pH of the buffer solution. d. For a weak acid titrated with a strong base the steep portion of titration curve at equivalence point occurs over a long pH range (from about pH 4 to pH 10) e. In Bronsted terms , the strength of acid is determined by its tendency to accept proton whereas the strength of base is dependent upon its tendency to donate proton.
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
You are asked to prepare 304 µL of a 1/38 dilution solution from your collected sample.How much your collected sample and buffer solution will you require? a. 7 µL of sample and 297 µL of buffer b. 4 µL of sample and 300 µL of buffer c. 8 µL of sample and 296 µL of buffer d. 1 µL of sample and 37 µL of buffer