Question

Suppose you are performing an experiment that requires a constant pH of 9.00. 1) Which buffer...

Suppose you are performing an experiment that requires a constant pH of 9.00.

1) Which buffer system would be most appropriate? HOBr−NaOBr or HOCl−NaOCl? Ka for HOBr is 2.0×10−9, Ka for HOCl is 3.5×10−8.

For this question, the appropiate buffer is HOBR-NaOBr, though I'm not sure why.

2) Calculate the ratio of conjugate base to weak acid required to prepare a buffer with pH= 9.00.

I tried using the Henderson-Hasselbach equation for this but came up with the wrong answer according to my online homework. Any help would be appreciated!

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
You were asked to prepare a buffer with a pH of 9.00. Table 1: Weak Acid...
You were asked to prepare a buffer with a pH of 9.00. Table 1: Weak Acid Ka pKa Lactic Acid (HC3H5O3) 1.4 x 10-4 3.85 Acetic Acid (HC2H3O2) 1.8 x 10-5 4.74 Carbonic Acid (H2CO3) 4.4 x 10-7 6.36 Dihydrogen (H2PO4-) 6.2 x 10-8 7.21 Ammonium ion (NH4+) 5.6 x 10-10 9.25 Hydrogen Carbonate (HCO3+) 4.7 x 10-11 10.32 A. Using Table 1, what buffer system will you use? B. Your lab supervisor asked you to use 0.050 mol of...
You want to make 100 mL of 0.20 M Acetic Acid buffer with pH=4.0 You are...
You want to make 100 mL of 0.20 M Acetic Acid buffer with pH=4.0 You are given a stock solution of 1.0 M acetic acid and a bottle of sodium acetate salt (MW= 82 g/mol). The formula for the dissociation of acetic acid is shown here (CH3COOH <--> CH3COO- + H+) The henderson hasselbach equation is : pH=pKa +log [A-]/[HA]. What is the ratio of [A-]/[HA] when your buffer pH is 4.0? Determine the concentration of weak acid and conjugate...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT