Question

1. What is the pH after 20 ml of 0.1 M KOH is added to 10...

1. What is the pH after 20 ml of 0.1 M KOH is added to 10 ml of 0.2 M HClO? (Ka for HClO = 3.0 x 10-8)?

A. 10.2           

B. 3.8

C. 13.0           

D. 4.3

E. 9.7

32. Calculate the pH of a solution that is 1.00 M HF, 1.00 M HCl, and 1.439 MNaF. (Ka = 7.2 10–4)

3.14

3.30

2.48

2.98

0.25

Homework Answers

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
33. Calculate the pH of a solution that is 1.00 M HF, 2.00 M HCl, and...
33. Calculate the pH of a solution that is 1.00 M HF, 2.00 M HCl, and 1.439 MNaF. (Ka = 7.2 10–4) 3.14 3.30 2.48 2.98 0.25 34. If the solid CuF2 has a solubility of 0.0020 mol/L, what is the value of Ksp? 1.8 x 10-7 4.0 x 10-6 3.2 x 10-8 8.0 x 10-9 none of the above
a) What is the resulting concentration (M) of the solution containing 0.25 mL of 6M HCl...
a) What is the resulting concentration (M) of the solution containing 0.25 mL of 6M HCl and 12.50 mL distilled water? (0.0.75 pt.) b) What is the pH of this solution containing the HCl? (0.05 pt.) c) If 0.25 mL of 6M HCl is added in 4 mL of 0.2 M ClO- buffer solution, what is the final pH of the buffer (Ka HClO = 3.0 x 10-8)? (0.075 pt) d) If the Ka of the HClO is 3.0 x...
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 100mL sample of.20 M HF is titrated with 0.10 M KOH. Determine the pH of...
A 100mL sample of.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 60.0 mL of KOH. Ka (HF) = 3.5*10^-4
50 mL of 0.100 M HF is titrated with 55 mL of 0.100 M KOH. What...
50 mL of 0.100 M HF is titrated with 55 mL of 0.100 M KOH. What is the pH of the solution. Ka of HF = 6.8 x 10-4
1) Rank the following titrations in order of increasing pH at the halfway point to equivalence...
1) Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH). 100.0 mL of 0.100 M KOH by 0.100 M HCl 100.0 mL of 0.100 M HC3H5O2 (Ka = 1.3 x 10-5) by 0.100 M NaOH 100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100 M HCl 100.0 mL of 0.100 M HF (Ka = 7.2 x 10-4) by 0.100 M NaOH...
What will be the pH at the equivalence point in the titration of 45.00 mL of...
What will be the pH at the equivalence point in the titration of 45.00 mL of 0.115 M NaClO with 0.106 M HCl? ClO–(aq) + HCl(aq) → HClO(aq) + Cl–(aq) Ka(HClO)=3.0·10-8 You only need to provide the final answer (pH).
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH...
A 50.0-mL volume of 0.15 M HBr is titrated with 0.25 M KOH. Calculate the pH after the addition of 13.0 mL of KOH.
Rank the following titrations in order of increasing pH at the equivalence point of the titration...
Rank the following titrations in order of increasing pH at the equivalence point of the titration (1 = lowest pH and 5 = highest pH). 100.0 mL of 0.100 M C2H5NH2 (Kb = 5.6 x 10-4) by 0.100 M HCl 100.0 mL of 0.100 M HF (Ka = 7.2 x 10-4) by 0.100 M NaOH 100.0 mL of 0.100 M HC3H5O2 (Ka = 1.3 x 10-5) by 0.100 M NaOH 200.0 mL of 0.100 M H2NNH2 (Kb = 3.0 x...
A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the...
A 100.0 mL sample of 0.20 M HF is titrated with 0.10 M KOH. Determine the pH of the solution after the addition of 95 mL of KOH. The Ka of HF is 3.5 × 10-4.
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT