Question

If 6.5% of a 0.0100 M solution of an organic base, R2NH, was found to have...

If 6.5% of a 0.0100 M solution of an organic base, R2NH, was found to have reacted with H2O, what would be the Kb of that base?

Homework Answers

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
A 0.0100 M solution of a weak base has pH = 9.78 at T = 25...
A 0.0100 M solution of a weak base has pH = 9.78 at T = 25 C. What is the numerical value for Kb for the weak base?
A 50.00-mL solution of 0.0229 M trimethylamine (Kb = 6.5 × 10–5) is titrated with a...
A 50.00-mL solution of 0.0229 M trimethylamine (Kb = 6.5 × 10–5) is titrated with a 0.0178 M solution of hydrochloric acid as the titrant. What is the pH of the base solution after 13.35 mL of titrant have been added? (Kw = 1.00 × 10–14)
The pH of a 1.00 M solution of urea, and weak organic base, is 7.050. Calculate...
The pH of a 1.00 M solution of urea, and weak organic base, is 7.050. Calculate the Ka of protonated urea.
Pyridine is an organic base that reacts with water as follows: C5H5N(aq) + H2O(l) <---> C5H5NH+(aq)...
Pyridine is an organic base that reacts with water as follows: C5H5N(aq) + H2O(l) <---> C5H5NH+(aq) +OH-(aq) Kb=1.58*10^-9 for pyridine. What is the concentration of the C5H5NH+ ion in a solution initially 1.0M in pyridine? What is the pH of the solution? Clearly state and check any approximations you make.
A solution contains 0.0100 M Pb2 (aq) and 0.0100 M Sr2 (aq). If we add SO42–(aq),...
A solution contains 0.0100 M Pb2 (aq) and 0.0100 M Sr2 (aq). If we add SO42–(aq), what will be the concentration of Pb2 (aq) when SrSO4(s) begins to precipitate?
Determine the pH of a 0.0100 M solution of NH4NO3.
Determine the pH of a 0.0100 M solution of NH4NO3.
10 mL of 0.0100 M HCl are added to 23 mL of 0.0100 M acetic acid....
10 mL of 0.0100 M HCl are added to 23 mL of 0.0100 M acetic acid. What is the pH of the resulting solution?
The pH of a 0.032 M solution of a weak base is 9.83. What is the...
The pH of a 0.032 M solution of a weak base is 9.83. What is the pKb for this base? That is the -log(Kb).
A solution contains 0.0350 M Ca2 and 0.0100 M Sr2 .What is the concentration of the...
A solution contains 0.0350 M Ca2 and 0.0100 M Sr2 .What is the concentration of the first cation when the second starts to precipitate?
5. What is the pH of a solution of 0.0100 M HCl dissolved in 0.01334 M...
5. What is the pH of a solution of 0.0100 M HCl dissolved in 0.01334 M potassium carbonate when taking solution activity into account? 6. What would be the uncertainty of a 0.5000 M solution of Fe3+ prepared from solid iron (III) sulfate with a ±0.01 g balance and a 250.00 ±0.08 mL volumetric flask? i need the work for both questions by 12:15pm 2/25/16 PLEASE!
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT