Question

1. What concentration of ammonia is required to have a solution with a pH of 11.35?...

1. What concentration of ammonia is required to have a solution with a pH of 11.35? Kb = 1.8x10-5

2. A 1.81 x 10−3 M solution of quinine, a drug used in treating malaria, has a pH of 9.82. What is the value of Kb? Express your answer in scientific notation, 2 significant figures.

3. A diprotic acid, H2A has the following Kas: Ka1 = 3.13 x 10-7 and Ka2 = 8.93 x 10-11. What is the Kb of HA-?

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
1. What is the pH of a 1.05M solution of carbonic acid? Ka1 = 4.3 x...
1. What is the pH of a 1.05M solution of carbonic acid? Ka1 = 4.3 x 10-7 Ka2 = 5.6 x 10-11 2. A diprotic acid, H2A has the following Kas: Ka1 = 3.94 x 10-7 and Ka2 = 8.78 x 10-11. What is the Kb of HA-? 3.A diprotic acid, H2A has the following Kas: Ka1 = 3.94 x 10-7 and Ka2 = 8.78 x 10-11. What is the Kb of HA-?
-What concentration of ammonia is required to have a solution with a pH of 11.36? Kb...
-What concentration of ammonia is required to have a solution with a pH of 11.36? Kb = 1.8x10-5 -What is the pH of a 0.014M solution of NaF? Ka for HF = 6.8 x 10-4 -What is the other product of the aqueous base dissociation reaction of ethyl amine? C2H5NH2(aq) + H2O(l) ⇌ ________ + OH-(aq)
The pH of an ammonia solution is 9.00. What is the concentration in mol L-1 of...
The pH of an ammonia solution is 9.00. What is the concentration in mol L-1 of this ammonia solution given that Kb for ammonia is 1.78 x 10-5?
For the diprotic weak acid H2A, Ka1= 3.5 x 10^-6 & Ka2= 5.5 x 10^-9 What...
For the diprotic weak acid H2A, Ka1= 3.5 x 10^-6 & Ka2= 5.5 x 10^-9 What is the pH of a 0.0450 M solution of H2A? & What are the equilibrium concentrations of H2A & A2- in this solution? Please explain
53. What is the pH of a 0.4283 M aqueous solution of ammonia? Kb (NH3) =...
53. What is the pH of a 0.4283 M aqueous solution of ammonia? Kb (NH3) = 1.8x10-5
What is the pH of a solution of 3.4 M H2A (Ka1 = 1.0 × 10^-6...
What is the pH of a solution of 3.4 M H2A (Ka1 = 1.0 × 10^-6 and Ka2 is 1.0 × 10^-10)? Please explain step by step
An 80.9 mL sample of a 0.100 M solution of a diprotic acid, H2A, is titrated...
An 80.9 mL sample of a 0.100 M solution of a diprotic acid, H2A, is titrated with 0.100 M KOH. For H2A, Ka1 = 8.09 x 10^-5 and Ka2 = 8.09 x 10^-10. A) Calculate the concentration of A2- prior to the addition of any KOH. B) What is the pH of the initial solution? C) What is the pH exactly halfway to the first equivalence point? D) What is the pH exactly halfway between the first and second equivalence...
What is the pH of 0.30 M ammonia solution? Kb of Ammonia is 1.8 x 10...
What is the pH of 0.30 M ammonia solution? Kb of Ammonia is 1.8 x 10 NH3 (aq) + H20 (l) NH; (aq) + OH-(aq)
The concentration of your solution is 0.0400 M. You measure the pH to be 8.824. What...
The concentration of your solution is 0.0400 M. You measure the pH to be 8.824. What is the kb based on this measurement? Express your answer in scientific notation (X.XXE-X).
What is the pH of a solution made by adding 1.451 moles of ammonia (NH3, Kb...
What is the pH of a solution made by adding 1.451 moles of ammonia (NH3, Kb = 1.8 x 10-5) to 537 mL of distilled water?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT