Question

What is the pH at equivalence point when 100 mL of a 0.175 M solution of...

What is the pH at equivalence point when 100 mL of a 0.175 M solution of acetic acid (CH3COOH) is titrated with 0.10 M NaOH to its end point?

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
What is the pH at the equivalence point when 55.0 mL of a 0.300 M solution...
What is the pH at the equivalence point when 55.0 mL of a 0.300 M solution of acetic acid (CH3COOH) is titrated with 0.100 M NaOH to its end point?
Consider an experiment where 35.0 ml of 0.175 M acetic acetic acid, HC2H3O3, is titrated with...
Consider an experiment where 35.0 ml of 0.175 M acetic acetic acid, HC2H3O3, is titrated with 0.25 M NaOH. What is the pH at the equivalence point of this titration? The Ka for acetic acid is 1.8 x 10-5.   Thanks!
a.) What is the pH at the equivalence point when a HF solution is titrated with...
a.) What is the pH at the equivalence point when a HF solution is titrated with NaOH? Choose from: less than 7, 7, or greater than 7. b.)Calculate the pH at the equivalence point when a 200. ml 0.050M HF solution that is titrated with 0.040M NaOH solution? (Ka HF = 7.2 x 10-4)
What is the pH at the equivalence point in the titration of 100 mL of 0.10...
What is the pH at the equivalence point in the titration of 100 mL of 0.10 M HCN (CN- Kb = 2.0 × 10–5) with 0.10 M NaOH (100 mL)?
A 25.0 mL sample of an acetic acid solution in titrated with a 0.09984 M NaOH...
A 25.0 mL sample of an acetic acid solution in titrated with a 0.09984 M NaOH solution. The equivalence point is reached when 37.5 mL of the base is added. Calculate the concentration of acetic acid in the 25.0 mL sample. Calculate the pH at the equivalence point (Ka acetic acid = 1.75x10^-5)
A 22.5 mL sample of an acetic acid solution is titrated with a 0.175M NaOH solution....
A 22.5 mL sample of an acetic acid solution is titrated with a 0.175M NaOH solution. The equivalence point is reached when 37.5 mL of the base is added. What was the concentration of acetic acid in the original (22.5mL) sample? What is the pH of the equivalence point? Ka acetic acid= 1.75E-5
When 10.0 mL of 0.10 M HCOOH is titrated with .10 M NaOH, at the equivalence...
When 10.0 mL of 0.10 M HCOOH is titrated with .10 M NaOH, at the equivalence point of the pH the solution will be: A) Greater than 7 B) 7.00 C) Less than 7
A 0.860 M solution of NaOH is used to titrate the following solutions to the equivalence...
A 0.860 M solution of NaOH is used to titrate the following solutions to the equivalence point. How many milliliters of NaOH do you need when titrating against a concentration for Acetic Acid is 0.900 M. After determining the mL of NaOH, calculate the pH for both a. and b. a. 50.0 mL of 0.0750 M HCl b. 40.0 mL of CH3COOH How many millilters of NaOH do you need when titrating aginst
What is the pH at the equivalence point when 50.00 mL of 0.112 M hydroxyacetic acid...
What is the pH at the equivalence point when 50.00 mL of 0.112 M hydroxyacetic acid is titrated with 0.0580 M KOH? (Assume Ka = 1.47???10?4, and Kw = 1.01???10?14.)
25.00 mL of 0.1 M acetic acid are titrated with 0.05 M NaOH. Calculate the pH...
25.00 mL of 0.1 M acetic acid are titrated with 0.05 M NaOH. Calculate the pH of the solution after addition of 25 mL of NaOH. Ka(CH3COOH) = 1.8 x 10-5.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT