Question

A buffer solution based upon ascorbic acid (H2C6H6O6) was created by treating 1.00 L of a...

A buffer solution based upon ascorbic acid (H2C6H6O6) was created by treating 1.00 L of a 1.00 M ascorbic acid solution with NaOH until a pH of 3.473 was achieved (assuming no volume change). To this buffer 1.300 moles of NaOH were added (assume no volume change). What is the final pH of this solution?
For this problem we can assume the 5% assumption is valid.

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 buffer solution based upon ascorbic acid (H2C6H6O6) was created by treating 1.00 L of a...
A buffer solution based upon ascorbic acid (H2C6H6O6) was created by treating 1.00 L of a 1.00 M ascorbic acid solution with NaOH until a pH of 3.473 was achieved (assuming no volume change). To this buffer 1.300 moles of NaOH were added (assume no volume change). What is the final pH of this solution? For this problem we can assume the 5% assumption is valid.
A buffer solution based upon ascorbic acid (H2C6H6O6) was created by treating 1.00L of a 1.00...
A buffer solution based upon ascorbic acid (H2C6H6O6) was created by treating 1.00L of a 1.00 M ascorbic acid solution with NaOH until a pH of 3.602 was achieved (assuming no volume change). To this buffer 1.370 moles of NaOH were added (assume no volume change). What is the final pH of this solution? For this problem we can assume the 5% assumption is valid.
A buffer solution based upon sulfurous acid was created by treating 1L of 1M sulfurous acid...
A buffer solution based upon sulfurous acid was created by treating 1L of 1M sulfurous acid with NaOH until a pH of 1.347 was achieved (assuming no volume change). To this buffer 1.170 moles of NaOH were added (assume no volume change). What is the final pH of this solution? Assume 5% assumption is valid.
To a 1.00 L buffer solution made of 1.65 M nitrous acid (HNO2) and 1.01M potassium...
To a 1.00 L buffer solution made of 1.65 M nitrous acid (HNO2) and 1.01M potassium nitrite (KNO2) was added 0.625 moles of NaOH (assume no volume change to the solution). What is the final pH of this buffer assuming Ka nitrous acid = 4.00e-4
To a 1.00 L buffer solution made of 1.95 M hypochlorous acid (HClO) and 1.03 M...
To a 1.00 L buffer solution made of 1.95 M hypochlorous acid (HClO) and 1.03 M potassium hypochlorite (KClO) was added 0.509 moles of NaOH (assume no volume change to the solution). What is the final pH of this buffer assuming Ka hypochlorous acid = 2.90e-8?
A buffer solution contains 0.27 mol of ascorbic acid (HC6H7O6) and 0.76 mol of sodium ascorbate...
A buffer solution contains 0.27 mol of ascorbic acid (HC6H7O6) and 0.76 mol of sodium ascorbate (NaC6H7O6) in 8.20 L. The Ka of ascorbic acid (HC6H7O6) is Ka = 8e-05. (a) What is the pH of this buffer? pH =    (b) What is the pH of the buffer after the addition of 0.08 mol of NaOH? (assume no volume change) pH =   (c) What is the pH of the original buffer after the addition of 0.39 mol of HI? (assume...
A buffer solution contains 0.56 mol of ascorbic acid (HC6H7O6) and 0.54 mol of sodium ascorbate...
A buffer solution contains 0.56 mol of ascorbic acid (HC6H7O6) and 0.54 mol of sodium ascorbate (NaC6H7O6) in 5.70 L. The Ka of ascorbic acid (HC6H7O6) is Ka = 8e-05. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.10 mol of NaOH? (assume no volume change) (c) What is the pH of the original buffer after the addition of 0.30 mol of HI? (assume no volume change)
Consider a the titration of 0.729 L of 0.519 M ascorbic acid (H2C6H6O6) with 1.69 M...
Consider a the titration of 0.729 L of 0.519 M ascorbic acid (H2C6H6O6) with 1.69 M NaOH. What is the pH at the second equivalence point of the titration?
A 1.00 L buffer solution is composed of 0.250 M HF and 0.250 M NaF. Calculate...
A 1.00 L buffer solution is composed of 0.250 M HF and 0.250 M NaF. Calculate the 13)______ pH of the solution after the addition of 0.150 moles of solid NaOH. Assume no volume change upon the addition of base. The Ka for HF is 3.5 × 10-4.
Consider the titration of 0.953 L of 0.591 M ascorbic acid (H2C6H6O6) with 1.58 M NaOH....
Consider the titration of 0.953 L of 0.591 M ascorbic acid (H2C6H6O6) with 1.58 M NaOH. What is the pH at the second equivalence point of the titration?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT