HomeworkLib
Question

When 1.00 L of 0.45 M acetic acid (pKa = 4.74) is mixed with the exact...

When 1.00 L of 0.45 M acetic acid (pKa = 4.74) is mixed with the exact volume of 0.55 M NaOH required to convert the acid to its conjugate base, at the endpoint the solution will have a:

A. pH < pKa

B. pH > 7.00

C. pH = pKa

D. pH = 7.00

E. pH < 7.00

science   chemistry   
0 0
Add a comment Improve this question Transcribed image text
Next > < Previous
Sort answers by oldest

Homework Answers

Answer #1

moles of NaOH = molarity * volume

= 0.55 * 1 (same volume)

= 0.55

moles of acetic acid = 0.45 * 1

= 0.45

remaning moles of NaOH = 0.55 - 0.45

= 0.10

so, pH will be greater than 7.

any query please comment

if satisfied please rate it thanks

0 0
Add a comment
Know the answer?
Add Answer to:
When 1.00 L of 0.45 M acetic acid (pKa = 4.74) is mixed with the exact...
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. Our experts will answer your question WITHIN MINUTES for Free.
Similar Homework Help Questions

  • A 1.00 L buffer solution with pH = 4.74 is composed of 0.30 mol acetic acid...

    A 1.00 L buffer solution with pH = 4.74 is composed of 0.30 mol acetic acid and 0.30 mol sodium acetate. A) Determine the pKa of acetic acid B) If 0.030 mol of NaOH is added, determine the pH of the solution

  • Acetic acid has a pKa of 4.74. A stock solution of 1.0 M acetic acid is...

    Acetic acid has a pKa of 4.74. A stock solution of 1.0 M acetic acid is available. A stock solution of 2.0 M potassium acetate is available. Show all the calculations and explain how to make 560.0 mL of 250. mM acetate buffer that has a pH = 5.0. (Hint: first make a 250 mM potassium acetate solution and a 250 mM acetic acid solution. Then determine how much of each to use.). pH = pKa + log {[acetate]/[acetic acid]}

  • Solution A is a 1.00 L buffer solution that is 1.196 M in acetic acid and...

    Solution A is a 1.00 L buffer solution that is 1.196 M in acetic acid and 1.196 M in sodium acetate. Acetic acid has a pKa of 4.74. What is the pH change of this solution upon addition of 0.1 mol of HCl? Enter your answer numerically to three significant figures.

  • Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pKa...

    Suppose there is 1.00 L of an aqueous buffer containing 60.0 mmol of acetic acid (pKa = 4.76) and 40.0 mmol of acetate. Calculate the pH of this buffer. pH = What volume of 5.00 M NaOH would be required to increase the pH to 4.93? volume: 1 volume: mL TOOLS x10

  • Solution C is a 1.00 L buffer solution that is 1.240 M in acetic acid and...

    Solution C is a 1.00 L buffer solution that is 1.240 M in acetic acid and 0.56 Min sodium acetate. Acetic acid has a pKa of 4.74. What is the pH change of this solution upon addition of 0.07700 mol of HCI? Enter a negative number to 3 decimal places.

  • Acetic acid and its conjugate base acetate can form an acid-base buffer.  The pKa of acetic acid...

    Acetic acid and its conjugate base acetate can form an acid-base buffer.  The pKa of acetic acid is 4.75. How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the pH to 4.90 ? ___mL?

  • Acetic acid and its conjugate base acetate can form an acid-base buffer. The pKa of acetic...

    Acetic acid and its conjugate base acetate can form an acid-base buffer. The pKa of acetic acid is 4.75. 1st attempt FeedbackSee HintSee Periodic Table How much 10.0 M HNO3 must be added to 1.00 L of a buffer that is 0.0100 M acetic acid and 0.100 M sodium acetate to reduce the pH to 5.05 ?

  • Your task is to prepare a buffer solution of 1.00 L of 0.250 M acetic acid...

    Your task is to prepare a buffer solution of 1.00 L of 0.250 M acetic acid and solid sodium hydroxide. Start by writing the equation for the reaction that will form the buffer (hint: you must have both acetic acid and acetate ion in the solution; where will the acetate ion come from? Neglecting the volume change on addition of NaOH (MM 40.0 g/mol), what mass is required to produce a buffer of pH 3.75? What pH will the buffer...

  • A) A beaker with 1.80×102 mL of an acetic acid buffer with a pH of 5.000...

    A) A beaker with 1.80×102 mL of an acetic acid buffer with a pH of 5.000 is sitting on a benchtop. The total molarity of acid and conjugate base in this buffer is 0.100 M. A student adds 5.50 mL of a 0.340 M HCl solution to the beaker. How much will the pH change? The pKa of acetic acid is 4.740. B)You need to produce a buffer solution that has a pH of 5.37. You already have a solution...

  • For acetic acid pKa =4.74. A buffer solution was made using 0.30 mole of acetic acid...

    For acetic acid pKa =4.74. A buffer solution was made using 0.30 mole of acetic acid and an unspecified and amount of sodium acetatein water to make 2.00 liters of solution. The solution pH was 4.91. Calculate the number of moles of sodium acetate used.

ADVERTISEMENT
Free Homework Help App
Download From Google Play
Scan Your Homework
to Get Instant Free Answers
Need Online Homework Help?
Ask a Question
Get Answers For Free
Most questions answered within 3 hours.
ADVERTISEMENT
ADVERTISEMENT