Question

A 20.4 mL sample of 0.325 M trimethylamine, (CH3)3N, is titrated with 0.353 M perchloric acid....

A 20.4 mL sample of 0.325 M trimethylamine, (CH3)3N, is titrated with 0.353 M perchloric acid. After adding 7.40 mL of perchloric acid, what will be the pH ?

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
A 21.8 mL sample of 0.223 M trimethylamine, (CH3)3N, is titrated with 0.207 M hydrobromic acid....
A 21.8 mL sample of 0.223 M trimethylamine, (CH3)3N, is titrated with 0.207 M hydrobromic acid. At the equivalence point, the pH is
A 25.0 mL sample of a 0.0500 M solution of aqueous trimethylamine is titrated with a...
A 25.0 mL sample of a 0.0500 M solution of aqueous trimethylamine is titrated with a 0.0625 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25°C.
A 25.0 mL sample of a 0.290 M solution of aqueous trimethylamine is titrated with a...
A 25.0 mL sample of a 0.290 M solution of aqueous trimethylamine is titrated with a 0.363 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N=4.19 at 25 degrees C
A 25.0-mL sample of a 0.070 M solution of aqeous trimethylamine is titrated with a 0.088...
A 25.0-mL sample of a 0.070 M solution of aqeous trimethylamine is titrated with a 0.088 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added; pKb of (CH3)3N = 4.19 at 25 C.
1. A 28.5 mL sample of 0.218 M ethylamine, C2H5NH2, is titrated with 0.340 M nitric...
1. A 28.5 mL sample of 0.218 M ethylamine, C2H5NH2, is titrated with 0.340 M nitric acid. After adding 26.9 mL of nitric acid, the pH is _____. 2. A 24.7 mL sample of 0.292 M methylamine, CH3NH2, is titrated with 0.325 M perchloric acid. At the equivalence point, the pH is _____.
A 22.2 mL sample of 0.367 M dimethylamine, (CH3)2NH, is titrated with 0.277 M hydrobromic acid....
A 22.2 mL sample of 0.367 M dimethylamine, (CH3)2NH, is titrated with 0.277 M hydrobromic acid. After adding 10.9 mL of hydrobromic acid, the pH is ______
A 25.0 ml sample of 0.090 M solution of aqueous trimethylamine is nitrated with a 0.11...
A 25.0 ml sample of 0.090 M solution of aqueous trimethylamine is nitrated with a 0.11 M solution of HCl. Calculate the pH of the solution after 10.0, 20.0, and 30.0 mL of acid have been added, pkb of (ch3)3n = 4.19 (part 2, after adding 20.0 mL)
An analytical chemist is titrating 81.1 mL of a 0.5900 M solution of trimethylamine ((CH3)3N) with...
An analytical chemist is titrating 81.1 mL of a 0.5900 M solution of trimethylamine ((CH3)3N) with a 0.1300 M solution of HNO3. The pKb of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 415.2 mL of HNO3 solution to it. Round your answer to 2 decimal places.
1)Calculate the pH during the titration of 20.00 mL of 0.1000 M trimethylamine, (CH3)3N(aq), with 0.1000...
1)Calculate the pH during the titration of 20.00 mL of 0.1000 M trimethylamine, (CH3)3N(aq), with 0.1000 M HNO3(aq) after 19.5 mL of the acid have been added. Kb of trimethylamine = 6.5 x 10-5. 2)Determine the volume in mL of 0.13 M KOH(aq) needed to reach the half-equivalence (stoichiometric) point in the titration of 42 mL of 0.23 M C6H5OH(aq). The Ka of phenol is 1.0 x 10-10. Please explain
Find the pH and concentrations of (CH3)3N and (CH3)3NH+ in a 0.0060 M solution of trimethylamine.
Find the pH and concentrations of (CH3)3N and (CH3)3NH+ in a 0.0060 M solution of trimethylamine.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT