Question

A 350.0 mL buffer solution is 0.170 M in HF and 0.170 M in NaF. A)...

A 350.0 mL buffer solution is 0.170 M in HF and 0.170 M in NaF.

A) What mass of NaOH could this buffer neutralize before the pH rise above 4.00?

B) If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOH could be handled before the pH rises above 4.00?

Science   Chemistry   
0 0
Add a commentTranscribed image text
Next >

Homework Answers

Answer #1

A)

moles of HF = 350 x 0.170 / 1000 = 0.0595 mol

moles of NaF = 0.0595 mol

pH = pKa + log [salt + C / acid - C]

4.00 = 3.20 + log [0.0595 + C / 0.0595 - C]

[0.0595 + C / 0.0595 - C] = 6.3096

0.0595 + C = 0.375 - 6.3096 C

C = 0.0432

moles of NaOH = 0.0432 mol

mass of NaOH = 1.73 g

b)

moles of HF = NaF = 0.126

4.00 = 3.20 + log [0.126 + C / 0.126 - C]

[0.126 + C / 0.126 - C] = 6.3096

0.126 + C = 0.795 - 6.3096 C

C = 0.0915

moles of NaOH = 0.0915

mass of NaOH = 3.66 g

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 350.0 −mL buffer solution is 0.140 M in HFand 0.140 M in NaF.What mass of...
A 350.0 −mL buffer solution is 0.140 M in HFand 0.140 M in NaF.What mass of NaOH could this buffer neutralize before the pH rises above 4.00?If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOHcould be handled before the pH rises above 4.00?
A 360.0 −mL buffer solution is 0.160 M in HFand 0.160 M in NaF. Part A)...
A 360.0 −mL buffer solution is 0.160 M in HFand 0.160 M in NaF. Part A) What mass of NaOH could this buffer neutralize before the pH rises above 4.00? Part B) If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOHcould be handled before the pH rises above 4.00?
2) A 350.0 −mL buffer solution is 0.140 M in HFand 0.140 M in NaF. What...
2) A 350.0 −mL buffer solution is 0.140 M in HFand 0.140 M in NaF. What mass of NaOH could this buffer neutralize before the pH rises above 4.00? If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOHcould be handled before the pH rises above 4.00? 3) A 5.65 −g sample of a weak acid with Ka=1.3×10−4 was combined with 5.20 mL of 6.10 M NaOH and the...
1) What mass of ammonium chloride should be added to 2.50 L of a 0.160 M...
1) What mass of ammonium chloride should be added to 2.50 L of a 0.160 M NH3 in order to obtain a buffer with a pH of 9.55? 2) A 350.0 −mL buffer solution is 0.140 M in HFand 0.140 M in NaF. What mass of NaOH could this buffer neutralize before the pH rises above 4.00? If the same volume of the buffer was 0.360 M in HF and 0.360 M in NaF, what mass of NaOHcould be handled...
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.
A 130.0 −mL buffer solution is 0.110 M in NH3 and 0.130 M in NH4Br. If...
A 130.0 −mL buffer solution is 0.110 M in NH3 and 0.130 M in NH4Br. If the same volume of the buffer were 0.265 M in NH3 and 0.390 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?
A buffer is prepared by adding 42.1 mL of 2.4 M NaF to 30.3 mL of...
A buffer is prepared by adding 42.1 mL of 2.4 M NaF to 30.3 mL of 0.18 M HF. What is the pH of the final solution?
A 130.0 mL buffer solution is 0.105 molL−1 in NH3 and 0.125 molL−1 in NH4Br. What...
A 130.0 mL buffer solution is 0.105 molL−1 in NH3 and 0.125 molL−1 in NH4Br. What mass of HCl will this buffer neutralize before the pH falls below 9.00?If the same volume of the buffer were 0.270 molL−1 in NH3 and 0.395 molL−1 in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?
A 130.0 mL buffer solution is 0.105 molL−1 in NH3 and 0.125 molL−1 in NH4Br. What...
A 130.0 mL buffer solution is 0.105 molL−1 in NH3 and 0.125 molL−1 in NH4Br. What mass of HCl will this buffer neutralize before the pH falls below 9.00? I GOT THE ANSWER TO BE 0.11g Part 2 IS MY PROBLEMIf the same volume of the buffer were 0.270 molL−1 in NH3 and 0.395 molL−1 in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?
A 120.0 −mL buffer solution is 0.260 M in NH3 and 0.390 M in NH4Br, what...
A 120.0 −mL buffer solution is 0.260 M in NH3 and 0.390 M in NH4Br, what mass of HCl could be handled before the pH fell below 9.00?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT