Question

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 =
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 0.166 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.
Calculate the pH of a 0.375 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4)...
Calculate the pH of a 0.375 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH =    [HNO2 ]equilibrium =    M [NO2- ]equilibrium =    M
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 pH of a 0.334 M aqueous solution of phenol (a weak acid) (C6H5OH, Ka...
Calculate the pH of a 0.334 M aqueous solution of phenol (a weak acid) (C6H5OH, Ka = 1.0×10-10) and the equilibrium concentrations of the weak acid and its conjugate base. pH =    [C6H5OH ]equilibrium =    M [C6H5O- ]equilibrium =    M
Calculate the pH of a 0.501 M aqueous solution of chlorous acid (HClO2, Ka = 1.1×10-2)...
Calculate the pH of a 0.501 M aqueous solution of chlorous acid (HClO2, Ka = 1.1×10-2) and the equilibrium concentrations of the weak acid and its conjugate base. pH = [HClO2]equilibrium = M [ClO2- ]equilibrium = M
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 =
A) What is the degree of ionization of ethylamine, C2H5NH2, in an 0.90 M aqueous solution?...
A) What is the degree of ionization of ethylamine, C2H5NH2, in an 0.90 M aqueous solution? B) What is the percent ionization of ethylamine, C2H5NH2, in an 0.90 M aqueous solution?
A 25mL sample of 0.10M C2H5NH2 (ethylamine) is titrated with 0.150M HCl. What is the pH...
A 25mL sample of 0.10M C2H5NH2 (ethylamine) is titrated with 0.150M HCl. What is the pH of the solution after 9mL of acid have been added to the amine? [Kb(C2H5NH2) = 6.5 X 10^-4]
Consider a solution of 0.36 M C2H5NH2 (Kb = 5.6×10-4). Decide if each of the following...
Consider a solution of 0.36 M C2H5NH2 (Kb = 5.6×10-4). Decide if each of the following is a major or minor species in the solution, and calculate the pH. OH− H2O C2H5NH3+ C2H5NH2 H+ AND pH?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT