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11 Dec 2019

Determine the volumes of each solution you would use to prepare a 1.0L of a pH 5.00 buffer. Choose solutions from the following list. For the answer, list the solution and the volume of that solution.

0.10 M HCOOH Ka = 1.8 x 10^-4

0.10 M HCOONa

0.10 M CH₃COOH Ka = 1.8 x 10^-5

0.10 M CH₃COONa

0.10 M HCN Ka = 4.9 x 10^-10

0.10 M NaCN

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13 Dec 2019

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Related questions

Which of the following combinations would make a buffer with pH closest to 9.0?
Given:

HClO2 â Ka = 1.1 Ã 10-2
NH3 â Kb = 1.8 Ã 10-5
HNO2 â Ka = 7.2 Ã 10-4
C5H5N â Kb = 1.5 Ã 10-9

Choices:

Equal volumes of 0.10 M HClO2 and 0.10 M NaClO2

Equal volumes of 0.10 M HCl and 0.10 M NaCl

Equal volumes of 0.10 M C5H5NHCl and 0.10 M C5H5N

Equal volumes of 0.10 M HNO2 and 0.10 M NaNO2

Equal volumes of 0.10 M NH4Cl and 0.10 M NH3

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 HPO₄^2-

B) 0.50 M H₂PO₄^- / 0.10 M HPO₄^2-

C) They all have the same buffer capacity.

D) 0.10 M H₂PO₄^- / 0.50 M HPO₄^2-

E) 0.50 M H₂PO₄^- / 0.50 M HPO₄^2-

^{NUMBER 3}

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

A) HBrO, K_a = 2.3 â 10^-9

B) CH₃COOH, K_a = 1.8 â 10^-5

C) C₅H₅O₅COOH^-2, K_a = 4.0 â 10^-6

D) C₆H₄(COOH)₂, K_a = 2.9 â 10^-4

E) HOC₆H₄OCOOH, K_a = 1.0 â 10^-3

What is the hydronium ion concentration in a solution prepared by mixing 50.00 mL of 0.10 M HCN with 50.00 mL of 0.030 M NaCN? Assume that the volumes of the solutions are additive and that Ka = 4.9 x 10^ -10 for HCN.

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