Question

Ka for hypochlorous acid, HClO, is 3.0x10^-8. Calculate the pH after 10.0, 20.0, 30.0, and 40.0mL...

Ka for hypochlorous acid, HClO, is 3.0x10^-8. Calculate the pH after 10.0, 20.0, 30.0, and 40.0mL of .100M NaOH have been added to 40.0 mL of .100M HClO. Please show all calculations

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
Ka for hypochlorous acid HCLO is 3.0x10-8. Calculate the pH after 10.0, 20.0, 30.0, and 40.0...
Ka for hypochlorous acid HCLO is 3.0x10-8. Calculate the pH after 10.0, 20.0, 30.0, and 40.0 ml of 100 m NaOH have been added to 40.0 ml of 0.100 m HCLO?
Ka for hypochlorous acid, HClO is 3.0x10^-8. Calculate the pH after 10.0, 20.0, 30.0 and 40.0...
Ka for hypochlorous acid, HClO is 3.0x10^-8. Calculate the pH after 10.0, 20.0, 30.0 and 40.0 mol 0.100 M NaOH have been added to 40.0 mL of 0.100 M HClO.
The Ka for hypochlorous acid, HClO, is 3.0 x 10-8.Calculate the pH after 13.0 mL of...
The Ka for hypochlorous acid, HClO, is 3.0 x 10-8.Calculate the pH after 13.0 mL of 0.100 M NaOH have been added to 30.0 mL of 0.100 M HClO
A 30.0 mL sample of 0.05 M HCLO is titrated by 0.0250 M KOH solution. Ka...
A 30.0 mL sample of 0.05 M HCLO is titrated by 0.0250 M KOH solution. Ka for HCLO is 3.5 x 10-8. Calculate the pH when no base has been added, the pH when 30.0 mL of the base has been added ,. the pH at the equivalence point and the pH when an additional 4.00 mL of the KOH solution has been added beyond the equivalence point
What is the pH of a 0.10 M solution of KClO, Ka (HClO) = 3.0x10^8
What is the pH of a 0.10 M solution of KClO, Ka (HClO) = 3.0x10^8
A 30.0 mL sample of 0.05 M HCLO is titrated by 0.0250 M KOH solution. Ka...
A 30.0 mL sample of 0.05 M HCLO is titrated by 0.0250 M KOH solution. Ka for HCLO is 3.5 x 10-8. Calculate..... a. the pH when no base has been added b. the pH when 30.0 mL of the base has been added c. the pH at the equivalence point d. the pH when an additional 4.00 mL of the KOH solution has been added beyond the equivalence point
A 25.0 mL sample of a 0.115 M solution of acetic acid is titrated with a...
A 25.0 mL sample of a 0.115 M solution of acetic acid is titrated with a 0.144 M solution of NaOH. Calculate the pH of the titration mixture after 10.0, 20.0, and 30.0 mL of base have been added. (The Ka for acetic acid is 1.76 x 10^-5). 10.0 mL of base = 20.0 mL of base = 30.0 mL of base =
Calculate the pH after 10.0 mL of 0.400 M NaOH is added to 20.0 mL of...
Calculate the pH after 10.0 mL of 0.400 M NaOH is added to 20.0 mL of 0.50 M CH3COOH.(Ka of CH3COOH is 1.8 * 10−5) The answer is supposed to be 4.57, but I'm getting 4.37. I'm so close but need a little guidance.
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?
What is the pH of 40 mL of a 0.10M solution of HClO with a Ka...
What is the pH of 40 mL of a 0.10M solution of HClO with a Ka of 3.0 x 10-8 after 10mL of 0.20M NaOH has been added?
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT