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12 Dec 2019

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

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Bunny Greenfelder
Bunny GreenfelderLv2
13 Dec 2019

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Related questions

7.)) A buffer may be prepared by mixing a weak acid with itssalt. Which of the acids below is the best for the preparation of abuffer with a pH of 4.50?

a) carbonic acid, H2CO3; Ka = 4.8 x 10-7

b) formic acid, HCO2H; Ka = 1.9 x 10-4

c) dihydrogen phosphate ion, H2PO4 ?, Ka = 6.2 x 10-8

d) ammonium ion, NH4+; Ka = 5.6 x 10-10

PLEASE EXPLAIN HOW YOU GOT YOUR ANSWER

Please give answers for parts a, b, c, and d

1. Youhave a 250 mL sample of 1.62 M acetic acid (Ka= 1.8x10^-5).Calculate the pH of the best buffer. Determine the concentrationsof components needed to make a solution that could resist (<0.5pH change) the addition of 0.15 mol of a strong acid orbase.

2.Carbonic acid is a diprotic acid, H2CO3, with Ka1=4.2x10^-7 and Ka2= 4.8x10^-11 at 25 degrees. The ion product forwater is Kw= 1.0x10^-14 at 25 degrees. What is the OH-concentration of a solution tha tis 0.28 M inNa2CO3?

3. A titration of 200 mL of 1.00 MH2A was done with 1.16 M NaOH. For the diprotic acid H2A, Ka1=2.50x10^-5, Ka2= 3.10x10^-9. Calculate the pH after 600 mL of 1.16M NaOH have been added.

4. 15.0 mL of 0.50 M NaOH is addedto a 100 mL sample of 0.430 M NH3 (Kb for NH3= 1.8x10^-5). What isthe equilibrium concentration of NH4+ ions?.....and NH4?.....andpH?

Step bystep to get full answer....I want to make sure I am working theseproblems correctly...best, most clear and concise answer gets fullpoints... feel free to dumb it down:-)

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