9. What can be Statement can be TRUE about acidic buffer? a. It is made ofa mixture odf strong acid and salt of its conjugate acid b. Concentration of hydrogen ions in acidic buffer is greater than concentration of OH ions which is present in the solution c. Dilution of buffer by adding large amount of water doesnt change the pH of buffer solution d. Acidic buffer usually works effectively at pH range of above 7 10. A buffer solution is made of mixture of aqueous methanoic acid HCOOH With aqueous sodium methanoate acid NAHCOO The equilibrium reaction takes place in buffer solution is: HCOOH → HCOO- + H* Small amount of NAOH is then added to that buffer solution. What reaction take places at the buffer solution to resist change of pH caused by addition of base? а. НСООН +н- b. HCOO-+H с. НСООН +Он- d. HCOOH +ОН- HCOOH: НСООН > HCOO+H20 НСООН?

9. What can be Statement can be TRUE about acidic buffer? a. It is made ofa mixture odf strong acid and salt of its conjugate acid b. Concentration of hydrogen ions in acidic buffer is greater than concentration of OH ions which is present in the solution c. Dilution of buffer by adding large amount of water doesnt change the pH of buffer solution d. Acidic buffer usually works effectively at pH range of above 7 10. A buffer solution is made of mixture of aqueous methanoic acid HCOOH With aqueous sodium methanoate acid NAHCOO The equilibrium reaction takes place in buffer solution is: HCOOH → HCOO- + H* Small amount of NAOH is then added to that buffer solution. What reaction take places at the buffer solution to resist change of pH caused by addition of base? а. НСООН +н- b. HCOO-+H с. НСООН +Он- d. HCOOH +ОН- HCOOH: НСООН > HCOO+H20 НСООН?

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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Which of the following constitute a buffer? A. NH3 and KNO3 B. HCN & NaCN C. HF & NaCl D. NaOH & NaCl Group of answer choices C A & C B A, B and C
What is the pH of a buffer made by combining 45 ml of 0.15M nitrous acid and 20 ml of 0.175 M sodium nitrite a. 3.43 b. 3.64 c. 3.28 d. 3.06
At which point of the titration curve is there maximum buffering capacity for a weak acid?A. at the start of the titration B. at 25 % neutralization C. at 50 % neutralization D. at 100 % neutralization
During a titration, it is found that 59.5 mL of a solution of NaOH is needed to neutralize a solution that contains 1.69 g HCL. What is the concentration of the NaOH solution? a.) 0.3535m b.) 0. 6869m c.) 0. 7790m d.) 0. 6051m e.) 1.055m
The point where the indicator actually changes color is called the. . of the titration. 1. start point 2. middle point 3. end point 4. zero point а. 1 O b. 2 с. 3 O d. 4
Which of the following best describes Buffers? A. Buffers are weak acid and conjugate base pairs that resist changes in the pH of a solution. B. Buffers promote pH changes of a solution by contributing hydronium ions to the solution. C. Buffers are solutions containing a strong acid and a weak base resulting in neutralization. D. Buffers are of minimal importance to pH regulation in body fluids.
Which of the following pairs cannot be used to make a buffer? a. HF and NaF b. HC2H3O2 and NaOH c. HBr and KBr d. NH3 and NH4Cl
Which of the following would be considered a buffer solution? Select one: a. 0.1 M HCIO4/0.1 M NaclO4 b. 0.1 M H2S04/0.1 M NaHSO4 c. 0.1 M HNO3/0.1 M NaNO3 d. 0.1 M NaHCO3/0.1 M Na2CO3
Which of the following is true In an acid-base titration A. Water is never formed B. You are trying to make a precipitate C. Moles acid = moles base at the point of neutralization D. The pH will always be = to 7.0 at the neutralization point
You have two buffered solutions. Buffered solution 1 consists of 5.0 M HOAc and 5.0 M NaOAc; buffered solution 2 is made of 0.050 M HOAc and 0.050 M NaOAc. How do the pHs of the buffered solutions compare? Select one: a. The pH of buffered solution 1 is greater than that of buffered solution 2. b. The pH of buffered solution 2 is greater than that of buffered solution 1. c. The pH of buffered solution 1 is equal to that of buffered solution 2. d. Cannot be determined without the Ka values. e. None of these (A-D).
Ans all of them
For a buffer containing HF (aq) and NaF (aq), what ratio of ([F ]/ [HF]) is needed to give a buffer of pH 2.35? 0.16 O 1.00 0.45 0.80 O 6.31