A reaction occurs at a pH of approximately 5. Which of the following buffer systems would be best used to make a solution with this pH?
Select one:
a. [CH3COOH] :[CH3COO-]
b. [H2PO4-]: [HPO42-]
c. [H2CO3] :[HCO3-]
d. none of these.
Acetic acid sodium acetate buffer pH range is 3.7-5.6 and same for phosphate buffer varries from pH 5.8 to 8. The bicarbonate buffer is the one which mentains basic pH of our blood (pH of this buffer adove 7) .As pH 5 is suitable for the mentioned reaction so the correct answer will be
a) [CH3COOH];[CH3COO-]
A reaction occurs at a pH of approximately 5. Which of the following buffer systems would...
Consider a solution consisting of the following two buffer systems: H2CO3 HCO3– + H+ pKa = 6.4 H2PO4– HPO42– + H+ pKa = 7.2 At pH 6.4, which one of the following is true of the relative amounts of acid and conjugate base present? ***Please explain why the right answer is right and why the other ones are wrong. a. [H2CO3] > [HCO3- ] and [H2PO4- ] > [HPO42- ] b. [HCO3- ] > [H2CO3] and [HPO42- ] > [H2PO4-...
Which of the following buffer pairs would do the best at resisting pH change at a pH of 5? Select one: a. H2PO4− and HPO4−2 b. CH3COOH and CH3COO− c. NH4+ and NH3 d. There is not enough information to tell.
Which of the following combinations would be best to buffer an aqueous solution at a pH of 9.02 Use the References to access important values if needed for this question HNO2 and NO27, Kg = 4.5E-4 H3PO4 and H2PO4, Ka1 = 7.5E-3 H2P04 and HPO42-, K42 = 6.2E-8 CH2COH and CH3COO", KA = 1.8E-5 NHA and NH3, K= 5.7E-10 Submit Answer I question attempt remaining Autosaved at 10.16A
Buffer action 4 A buffer solution consisting of 0.05 mol/L acetic acid (CH3COOH) and 0.05 mol/L acetate (CH3COO-) has been used to buffer a 1 L solution at pH 4.7. A small amount of sodium hydroxide solution containing 0.0001 mol NaOH was added. Which of the following reactions best represents the buffer action? + Select one: O a. NaOH(aq) Na+(aq) + OH(aq) O b. CH3COOH(aq) + H2O(1) CH3COO(aq) H30*(aq) O c. CH3COO(aq) + H2O(0) CH3COOH(aq) OH(aq) O d. CH3COOH(aq) +...
In lab if you must make a buffer of pH=8.5, which of the following buffer systems would be best? How much of each species would you need in order to make 100ml of this buffer? 0.1M CH3COOH 0.1M NH3 0.1M KH2P04 0.1M NaCH3C00 0.1M NH4Cl 0.1M K2HPO4 *Please show all steps thank you!
In lab if you must make a buffer of pH=3.5, which of the following buffer systems would be best? How much of each species would you need in order to make 100ml of this buffer? 0.1M CH3COOH 0.1M NH3 0.1M KH2P04 0.1M NaCH3COO 0.1M NH4Cl 0.1M K2HPO4 *Please show all steps thank you!
If a buffer were needed with a pH of 7.0, what would be the best combination of weak acid and conjugate base to formulate the buffer? (please explain why you chose your answer) A) H3PO4 and H2PO4- B) H2PO4- and HPO42- C) HPO42- and PO43- D) acetic acid and acetate E) lactic acid and lactate
Which of the following acids would be best for preparing a buffer solution with an approximately neutral pH? H2CO3 - Ka = 4.3 x 10-7 H2S - Ka = 9.1 x 10-8 H3C6H5O7 - Ka = 7.1 x 10-4 HNO2 - Ka = 4.6 x 10-4
Which of the following buffers will have the best buffer capacity? a. A solution containing 0.157 M H2PO4- and 0.189 M HPO42- b. A solution containing 0.043 M H2PO4- and 0.025 M HPO42- c. A solution containing 0.101 M H2PO4- and 0.101 M HPO42 d. They all have the same buffer capacity
what concentrations of CH3COO- and CH3COOH of those below would give a buffer with a pH of 4.11 (pKa= CH3COOH=4.84) Br What concentrations of [CH3COO 1 and [CH1COOH1 of those below would give a buffer with a pH of 4.11? (pKa CH3COOH = 4.84). 10 a) (CH3COO]-0.15 M, [CH3COOH] = 0.10 M b) [CH3COO]-0.10 M, [CH3COOH] = 0.53 M c) [CH3COO]-0.46 M, [CH3COOH]= 0.10 M d) [CH3COO]- 0.23 M, [CH3COOH] = 0.10 M 14