Question

the pH of .10 M ethylamine is 11.82 a) Calculate the Kb for ethyamine using the...

the pH of .10 M ethylamine is 11.82

a) Calculate the Kb for ethyamine using the information provided

b) based on your answer in (a) calculate the pH of .15 ethylammonium chloride

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

0 0
Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Log In

Sign Up

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Calculate the pH of a 0.0416 M aqueous solution of ethylamine (C2H5NH2, Kb = 4.3×10-4) and...
Calculate the pH of a 0.0416 M aqueous solution of ethylamine (C2H5NH2, Kb = 4.3×10-4) and the equilibrium concentrations of the weak base and its conjugate acid.    pH = [C2H5NH2]equilibrium = M [C2H5NH3+ ]equilibrium =
#2 Ethylamine (CH3CH2NH2) is a base compound. a) Write base dissociation reaction ethylamine. b) If Kb...
#2 Ethylamine (CH3CH2NH2) is a base compound. a) Write base dissociation reaction ethylamine. b) If Kb of ethylamine is 7.41x10-10 , what is the pH of 0.15 M ethylamine solution?
Find the [OH−] in a 0.340 M solution of ethylamine (C2H5NH2). For ethylamine, Kb=5.6⋅10−4.
Find the [OH−] in a 0.340 M solution of ethylamine (C2H5NH2). For ethylamine, Kb=5.6⋅10−4.
Calculate the molar concentration of OH- ions in a 8.1 x 10-2 M solution of ethylamine...
Calculate the molar concentration of OH- ions in a 8.1 x 10-2 M solution of ethylamine (Kb= 6.4 x 10-4). Calculate the pH of this solution.
Calculate the expected pH of a 0.100 M solution of ammonium chloride given that Kb for...
Calculate the expected pH of a 0.100 M solution of ammonium chloride given that Kb for ammonia is 1.76x10-5
Calculate the pH of a 0.22 M CH3NH3Br solution. Kb(CH3NH2) = 4.4 ×10–4
Calculate the pH of a 0.22 M CH3NH3Br solution. Kb(CH3NH2) = 4.4 ×10–4
Calculate the pH of a 0.0786 M aqueous solution of the weak base caffeine (C8H10N4O2, Kb...
Calculate the pH of a 0.0786 M aqueous solution of the weak base caffeine (C8H10N4O2, Kb = 4.10×10-4). pH Calculate the pH of a 0.0786 M aqueous solution of the weak base caffeine (C8H10N4O2, Kb = 4.10×10-4). pH =
The pH of a 9.94×10-4 M solution of a weak base is 8.54. Calculate Kb for...
The pH of a 9.94×10-4 M solution of a weak base is 8.54. Calculate Kb for this base to three significant figures.
Calculate the pH of a 0.166 M aqueous solution of pyridine (C5H5N, Kb = 1.5×10-9) and...
Calculate the pH of a 0.166 M aqueous solution of pyridine (C5H5N, Kb = 1.5×10-9) and the equilibrium concentrations of the weak base and its conjugate acid. pH = [C5H5N]equilibrium = M [C5H5NH+]equilibrium = M
Calculate the pH of a weak base solution ([B]0 > 100 • Kb Calculate the pH...
Calculate the pH of a weak base solution ([B]0 > 100 • Kb Calculate the pH of a 0.106 M aqueous solution of triethanolamine (C6H15O3N, Kb = 5.8×10-7) and the equilibrium concentrations of the weak base and its conjugate acid.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT