Question

Determine the pH (to two decimal places) of the following solutions. If the 5% approximation is...

Determine the pH (to two decimal places) of the following solutions. If the 5% approximation is valid, use the assumption to compute pH.

8.72×10-3 M sodium hydrogen sulfate

pKa hydrogen sulfate ion is 1.92

8.73×10-3 M trifluoroacetic acid

pKa trifluoroacetic acid is 0.20

8.20×10-3 M ethylamine

pKa ethylammonium ion is 10.87

2.51×10-1 M sodium nitrite

pKa nitrous acid is 3.37

Homework Answers

Answer #1

sodium hydrogen sulfate:

PH = 1/2Pka-1/2 log[C]

PH = 1/2x 1.92- 1/2log[8.72x10-3]

PH = 0.96 - 1/2[log8.72-3]

PH = 0.96- 1/2 [0.9405-3]

PH = 0.96+1.029

PH =1.98

Trifluoroacetic acid:

pKa trifluoroacetic acid is 0.20

concentration 8.73×10-3 M

PH = 1/2Pka-1/2 log[C]

PH = 1/2x 0.20- 1/2log[8.73x10-3]

PH = 0.1 - 1/2[log8.73-3]

PH = 0.1- 1/2 [0.9410-3]

PH = 0.1+1.029

PH = 1.129

Ethylamine:

pKa ethylammonium ion is 10.87

concentration 8.20×10-3 M

PH = 1/2Pka-1/2 log[C]

PH = 1/2x 10.87- 1/2log[8.20x10-3]

PH = 0.1 - 1/2[log8.20-3]

PH = 0.1- 1/2 [0.9138-3]

PH = 0.1+1.043

PH = 1.143

sodium nitrite:

pKa nitrous acid is 3.37

concentration 2.51×10-1 M

PH = 1/2Pka-1/2 log[C]

PH = 1/2x 3.37- 1/2log[2.51x10-1]

PH = 1.685 - 1/2[log2.51 -1]

PH =1.685- 1/2 [0.3996-1]

PH = 1.685+0.3002

PH = 1.985

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the pH (to two decimal places) of a 4.31×10-3 M solution of oxalic acid. A...
Calculate the pH (to two decimal places) of a 4.31×10-3 M solution of oxalic acid. A table of pKa values can be found here. If the 5% approximation is valid, use the assumption to compute pH.
Can the five percent approximation be applied in determining the pH of the following solutions? A...
Can the five percent approximation be applied in determining the pH of the following solutions? A table of pKa values can be found here. Yes No  5.94×10-1 M dimethylammonium ion Yes No  5.52×10-1 M chloroacetic acid Yes No  6.64×10-4 M ammonium ion Yes No  3.99×10-4 M benzoic acid
Determine the pH (to two decimal places) of a solution prepared by adding 59.7 mL of...
Determine the pH (to two decimal places) of a solution prepared by adding 59.7 mL of 0.356 M butanoic acid (C3H7COOH) to 0.923 g of sodium butanoate (NaC3H7COO). Assume the volume of the solution does not change and that the 5% approximation is valid. Ka butanoic acid is 4.82
Find the pH of the following solutions given: pH = pKa + log (base/acid) 1) The...
Find the pH of the following solutions given: pH = pKa + log (base/acid) 1) The titration of 450.00 mL of 0.5 M nitric acid with 0.3 M sodium hydroxide after 250.0 mL of sodium hydroxide has been added... 2)Given the Kb for aniline = 4.3 x 10-3 at 25 degree Celsius, what is the pH of a .40 Molar solution of anilinium nitratate?
Calculate the pH of the following hydrochloric acid (HCl) solutions. Assume that HCl is completely dissociated...
Calculate the pH of the following hydrochloric acid (HCl) solutions. Assume that HCl is completely dissociated into hydrogen ion (H+) and chloride ion (Cl-) in water. (a) 10-2 M, 10-3 M, 10-4 M, 10-5 M, 10-6 M, 10-7 M, 10-8 M, 10-9 M (b) Draw a plot of pH as a function of HCl concentrations based on the solutions of (a)
Determine if the following salt solutions (0.123 M) are basic, acidic or neutral. Determine the pH...
Determine if the following salt solutions (0.123 M) are basic, acidic or neutral. Determine the pH of the solution, if possible. (Ammonium: Ka = 5.8 x 10-10, Sulfate: Kb = 8.3 x 10-13) a. Sodium nitrate b. Sodium sulfate c. Ammonium nitrate d. Ammonium sulfate
1. Find the pH of the following solutions: a) 9.5×10−2 M propionic acid (C2H5COOH). b) 0.103...
1. Find the pH of the following solutions: a) 9.5×10−2 M propionic acid (C2H5COOH). b) 0.103 M hydrogen chromate ion (HCrO−4). c) 0.125 M pyridine (C5H5N).
Determine the pH of each of the following solutions. (a) 0.821 M hydrogen peroxide (weak acid...
Determine the pH of each of the following solutions. (a) 0.821 M hydrogen peroxide (weak acid with Ka = 2.4e-12). (b) 0.306 M boric acid (weak acid with Ka = 5.8e-10). (c) 0.309 M pyridine (weak base with Kb = 1.7e-09).
Determine the pH of each of the following two-component solutions. 0.135 M in NH4Cl and 0.150...
Determine the pH of each of the following two-component solutions. 0.135 M in NH4Cl and 0.150 M in HNO3 8.92×10−2 M in sodium benzoate and 0.220 M in potassium bromide
Calculate the pH of each of the following solutions containing two solutes in the concentrations indicated....
Calculate the pH of each of the following solutions containing two solutes in the concentrations indicated.             (a)        0.50 M HOAc (acetic acid), 0.5 M NaOAc (sodium acetate); Ka = 1.8 x 10-5             (e)        0.400 M NaHSO4 , 0.400 M Na2SO4 ; Ka = 1.2 x 10-2
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT