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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.

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Related questions

Please explain to me thank you.

Which one of the following aqueous solutions, when mixed with an equal volume of 0.10 mol L-1 aqueous NH3, will produce a buffer solution?

A) 0.10 mol L-1 CH3COOH

B) 0.050 mol L-1 NaOH

C) 0.20 mol L-1 NH4Cl

D) 0.20 mol L-1 HCl

E) 0.10 mol L-1 HCl

NUMBER 2

Which of the following has the highest buffer capacity?

A) 0.10 M H2PO4- / 0.10 M HPO42-

B) 0.50 M H2PO4- / 0.10 M HPO42-

C) They all have the same buffer capacity.

D) 0.10 M H2PO4- / 0.50 M HPO42-

E) 0.50 M H2PO4- / 0.50 M HPO42-

NUMBER 3

Which of the following acids should be used to prepare a buffer with a pH of 4.5?

A) HBrO, Ka = 2.3 ✕ 10-9

B) CH3COOH, Ka = 1.8 ✕ 10-5

C) C5H5O5COOH-2, Ka = 4.0 ✕ 10-6

D) C6H4(COOH)2, Ka = 2.9 ✕ 10-4

E) HOC6H4OCOOH, Ka = 1.0 ✕ 10-3

A buffer solution with a pH of 6.00 is needed in an experiment. Which of the following buffer systems would work best?

a. H2PO4/ HPO42‒ KA of H2PO4 is 6.2×10‒8

b. NH3 / NH4+ KB of NH3 is 1.8×10‒5

c. N2H4 / N2H5+ KB of N2H4 is 9.6×10‒7

d. H2CO3 / HCO3‒ KA of H2CO3 is 4.3×10‒7

e. HNO2 / NO2‒ KA of is HNO2 is 7.1×10‒4

please explain

Which of the following combinations would be the best to buffer an aqueous solution at a pH of 5.0?H3PO4 and H2PO4- (Ka=7.5e-3)HNO2 and NO2 (Ka=(4.5e-4)CH3CO2H and CH3COO (Ka= 1.8e-5)H2PO4 and HPO4 (Ka=6.2e-8)please explain why! thanks

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