Question

A 0.10 M butanoic acid (butyric acid) solution has a pH of 5.2. To the nearest...

A 0.10 M butanoic acid (butyric acid) solution has a pH of 5.2. To the nearest hundredth of a unit, what fraction of the butanoic acid/butanoate molecules are in the basic form? (The pKa of butanoic acid is 4.82.)

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

Henderson - Hasselbalch equation is

pH = pKa + log( [ Base ] /[ acid ])

pH = 5.20

pKa of butanoic acid = 4.82

Butanate is the basic form

Butanoic acid is the acid form

5.20 = 4.82 + log([Butanate]/[Butanoic acid ])

log([Butanate]/[Butanoic acid ]) = 0.38

[ Butanate ]/ [ Butanoic acid ] = 2.40

So , for 1mole of Butanoic acid 2.40 mole of Butanate

[ Butanate ] = 2.40 × [ Butanoic acid ]

[Butanoic acid] + [Butanate] = 0.10M

[ Butanoic acid ] + 2.40[ Butanoic acid ] =0.10M

3.40[ Butanioc acid ] = 0.10M

[ Butanoic acid ] = 0.0294M

[ Butanate ] = 0.10M - 0.0294M =0.0706M

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
An analytical chemist is titrating 138.2 mL of a 1.100 M solution of butanoic acid (HC3H7CO2)...
An analytical chemist is titrating 138.2 mL of a 1.100 M solution of butanoic acid (HC3H7CO2) with a 0.6000 M solution of KOH. The pKa of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 294.3 mL of the KOH solution to it. Please round to 2 decimal places.
A 1.37 L buffer solution consists of 0.136 M butanoic acid and 0.337 M sodium butanoate....
A 1.37 L buffer solution consists of 0.136 M butanoic acid and 0.337 M sodium butanoate. Calculate the pH of the solution following the addition of 0.070 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 × 10-5. pH =
A 1.45 L buffer solution consists of 0.134 M butanoic acid and 0.344 M sodium butanoate....
A 1.45 L buffer solution consists of 0.134 M butanoic acid and 0.344 M sodium butanoate. Calculate the pH of the solution following the addition of 0.063 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 × 10-5.
A 1.49 L buffer solution consists of 0.186 M butanoic acid and 0.258 M sodium butanoate....
A 1.49 L buffer solution consists of 0.186 M butanoic acid and 0.258 M sodium butanoate. Calculate the pH of the solution following the addition of 0.062 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 × 10-5.
A 1.35 L buffer solution consists of 0.173 M butanoic acid and 0.309 M sodium butanoate....
A 1.35 L buffer solution consists of 0.173 M butanoic acid and 0.309 M sodium butanoate. Calculate the pH of the solution following the addition of 0.076 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 × 10-5.
A 1.36 L buffer solution consists of 0.184 M butanoic acid and 0.331 M sodium butanoate....
A 1.36 L buffer solution consists of 0.184 M butanoic acid and 0.331 M sodium butanoate. Calculate the pH of the solution following the addition of 0.068 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The Ka of butanoic acid is 1.52 × 10^-5.
Determine the pH (to two decimal places) of a solution prepared by adding 59.7 mL of...
Determine the pH (to two decimal places) of a solution prepared by adding 59.7 mL of 0.356 M butanoic acid (C3H7COOH) to 0.923 g of sodium butanoate (NaC3H7COO). Assume the volume of the solution does not change and that the 5% approximation is valid. Ka butanoic acid is 4.82
Consider a 2×10−2 M  solution of the weak acid butanoic acid , for which pKa =  4.83 ....
Consider a 2×10−2 M  solution of the weak acid butanoic acid , for which pKa =  4.83 . You can search for the structure of this compound online, although precise knowledge of the structure is not needed. Your answers need to be within 5% of the correct answer to be considered correct. Don't round or you will fall outside the 5% margin of error. Part A: Calculate  [H+] (units in M) Part B: Calculate the concentration of butanoate ions (units in M) Part...
The pH of a 1.0 L solution of 0.10 M lactic acid is 4.34. What is...
The pH of a 1.0 L solution of 0.10 M lactic acid is 4.34. What is the new pH of the solution if 40 mL of 1.0 M HCl is added? The pKa of lactic acid is 3.86.
A 0.10 M HCl solution has a pH of 1.00. A 0.10 M NaOH solution has...
A 0.10 M HCl solution has a pH of 1.00. A 0.10 M NaOH solution has a pH of 13.00. A 1.0 L solution in which 0.010 moles of compound Z is dissolved has a pH of 12.00. Compound Z is a strong acid strong base weak acid weak base
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT