Question

What is the pH of the solution that results from adding 50.00 mL of 0.1000 M...

What is the pH of the solution that results from adding 50.00 mL of 0.1000 M Acetic Acid with 10.00 mL of 0.1000 M NaOH

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 50.00 mL aliquot of a 0.1000 M propenoic acid solution, H2CCHCO2H, is titrated with 0.1250...
A 50.00 mL aliquot of a 0.1000 M propenoic acid solution, H2CCHCO2H, is titrated with 0.1250 M NaOH. Calculate the pH when 25.00 mL of NaOH is added. Ka = 5.52 × 10−5 pKa= -log(Ka) So pKa = 4.2581 Propenoic Acid= 0.1*0.05= 0.005 mols NaOH= 0.125*0.025= 0.003125 mols pH= 4.2581 + log(0.003125/0.005) pH=4.05 Is this answer correct?
Do the calculations for the titration of 50.00 mL of a 0.1000 M solution of H2SO3...
Do the calculations for the titration of 50.00 mL of a 0.1000 M solution of H2SO3 with a 0.2000 M solution of NaOH. Calculate the pH after the addition of 0.00, 12.50, 25.00, 37.50, 50.00, and 60.00 mL of NaOH. Ka1(H2SO3)=1.23×10-2; Ka2(HSO3-)=6.60×10-8. Please show all of your work.Thanks!
What is the pH of a solution that results from adding 158 mL of 0.244 M...
What is the pH of a solution that results from adding 158 mL of 0.244 M NaOH to 158 mL of 0.683 M HF? (Ka of HF = 7.2E-4) Ph= _________ Will give credit for the answer, thank you!
Calculate the pH during the titration of 50.00 mL of 0.1000 M phosphoric [H3PO4; Ka1=7.1 x...
Calculate the pH during the titration of 50.00 mL of 0.1000 M phosphoric [H3PO4; Ka1=7.1 x 10^(-3), Ka2=6.3 x 10^(-8), Ka3=4.2 x 10^(-13)] after adding 33.42 mL of 0.1000 M NaOH.
50.00 mL of 0.1000 M ammonia is titrated with 0.1000 M HCl.What is the pH of...
50.00 mL of 0.1000 M ammonia is titrated with 0.1000 M HCl.What is the pH of the solution when half the volume of HCl required for full reaction, is added? Kb of ammonia is 1.75 *10-5
a) What is the pH of a solution prepared by adding 25.0 mL of 0.10 M...
a) What is the pH of a solution prepared by adding 25.0 mL of 0.10 M acetic acid (Ka=1.8 x 10^-5) and 20.0 mL of 0.10 M sodium acetate? b) What is the pH after the addition of 1.0 mL of 0.10 M HCl to 20 mL of the solution above? c) What is the pH after the addition of 1.0 mL of 0.10 M NaOH to 20 mL of the original solution?
Calculate the pH of the solution that results from adding 20.0 mL of 0.200M NaOH to...
Calculate the pH of the solution that results from adding 20.0 mL of 0.200M NaOH to 50.0 mL of 0.135 M HNO2. (The answer is 3.51)
A 50.00 ml aliquot of 0.1000 M benzoic acid (Ka= 6.28x10^-5) was titrated with 0.2500 M...
A 50.00 ml aliquot of 0.1000 M benzoic acid (Ka= 6.28x10^-5) was titrated with 0.2500 M KOH. Calculate the pH of the solution after the addition of 5.00 ml of base.
6.) A 50.00 mL sample of 0.1000 M pyridine is titrated with 0.2000 M hydrochloric acid....
6.) A 50.00 mL sample of 0.1000 M pyridine is titrated with 0.2000 M hydrochloric acid. Show your calculations for the pH of the solution after the addition of each of the four total volumes of 0.2000 M hydrochloric acid in items a-d below. a.) 0.00 mL b.) 20.00 mL c.) 25.00 mL d.) 26.00 mL
Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka...
Find the pH during the titration of 20.00 mL of 0.1000 M butanoic acid, CH3CH2CH2COOH (Ka = 1.54 × 10−5), with 0.1000 M NaOH solution after the following additions of titrant. a. 20.10 mL: pH = b. 26.00 mL: pH = c. 13.00 mL pH =
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT