Question

The next three (3) problems deal with the titration of 381 mL of 0.501 M carbonic...

The next three (3) problems deal with the titration of 381 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.7 M NaOH.
What is the pH of the solution at the 2nd equivalence point?

What will the pH of the solution be when 0.1381 L of 1.7 M NaOH are added to the 381 mL of 0.501 M carbonic acid?

How many mL of the 1.7 M NaOH are needed to raise the pH of the carbonic acid solution to a pH of 5.935?

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
The next three (3) problems deal with the titration of 371 mL of 0.501 M carbonic...
The next three (3) problems deal with the titration of 371 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.9 M NaOH. 1)What is the pH of the solution at the 2nd equivalence point? 2)What will the pH of the solution be when 0.1282 L of 1.9 M NaOH are added to the 371 mL of 0.501 M carbonic acid? 3) How many mL of the 1.9 M NaOH are...
The next three (3) problems deal with the titration of 411 mL of 0.501 M carbonic...
The next three (3) problems deal with the titration of 411 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 2.1 M KOH. All answers to three significant digits. What is the pH of the solution at the 2nd equivalence point? What will the pH of the solution be when 0.1677 L of 2.1 M KOH are added to the 411 mL of 0.501 M carbonic acid? How many mL of...
The next three (3) problems deal with the titration of 301 mL of 0.501 M carbonic...
The next three (3) problems deal with the titration of 301 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.5 M KOH. How many mL of the 1.5 M KOH are needed to raise the pH of the carbonic acid solution to a pH of 6.635?
The next three (3) problems deal with the titration of 301 mL of 0.501 M carbonic...
The next three (3) problems deal with the titration of 301 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.3 M KOH. How many mL of the 1.3 M KOH are needed to raise the pH of the carbonic acid solution to a pH of 6.635? Could someone show their work for this. I've been trying to solve this for the last hour, but I can't seem to get the...
The titration of 321 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7,...
The titration of 321 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.5 M KOH. How many mL of the 1.5 M KOH are needed to raise the pH of the carbonic acid solution to a pH of 6.755? I tried many times, but I just dont get the answers right. How do I do this?
Consider a the titration of 0.629 L of 0.879 M carbonic acid (H2CO3) with 1.61 M...
Consider a the titration of 0.629 L of 0.879 M carbonic acid (H2CO3) with 1.61 M NaOH. What is the pH at the second equivalence point of the titration?
Consider a the titration of 0.907 L of 0.909 M carbonic acid (H2CO3) with 1.63 M...
Consider a the titration of 0.907 L of 0.909 M carbonic acid (H2CO3) with 1.63 M NaOH. What is the pH at the second equivalence point of the titration?
Henry's law constant for CO2 at 38oC is 2.28 x 10–3 mol/L\cdot⋅atm. Calculate the pH of...
Henry's law constant for CO2 at 38oC is 2.28 x 10–3 mol/L\cdot⋅atm. Calculate the pH of a solution of CO2 at 38oC in equilibrium with the gas at a partial pressure of 3.20 atm. Assume that all dissolved CO2 is in the form of carbonic acid (H2CO3). Ka1 = 4.3 x 10–7 and Ka2 = 5.6 x 10–11 for carbonic acid.
Consider a the titration of 0.531 L of 0.969 M ascorbic acid (H2C6H6O6) with 1.91 M...
Consider a the titration of 0.531 L of 0.969 M ascorbic acid (H2C6H6O6) with 1.91 M NaOH. What is the pH at the second equivalence point of the titration? ka1: 7.9*10^-5 ka2: 1.6*10^-12
16.5 mL of 0.168 M diprotic acid (H2A) was titrated with 0.118 M KOH. The acid...
16.5 mL of 0.168 M diprotic acid (H2A) was titrated with 0.118 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10. At what added volume (mL) of base does the first equivalence point occur? 20.8 mL of 0.146 M diprotic acid (H2A) was titrated with 0.14 M KOH. The acid ionization constants for the acid are Ka1=5.2×10−5 and Ka2=3.4×10−10. At what added volume (mL) of base does the second equivalence point occur? Consider the titration of...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT