Question

3. Determine the pH of a buffer that contains 0.5 mole HOCl and 0.5 mole NaOCl...

3. Determine the pH of a buffer that contains 0.5 mole HOCl and 0.5 mole NaOCl in a total volume of 1.0 L. The Ka of HOCl is 3.5 x 10^-8.

4. Write a net ionic Equation for what happens when NaOH is added into the solution in number 3.

5. Determine the pH when 0.1 mole NaOH is added to the solution in number 3. Assume the total volume does not change.


6. Determine the pH when 0.1 mole NaOH is added to 1.0 L of water

7. Did adding NaOH to the HOCl and NaOCl solution behave differently than adding NaOH to water? briefly explain.

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
given 100ml of buffer that is .50M in HOCl and .40 M in NaOCl what is...
given 100ml of buffer that is .50M in HOCl and .40 M in NaOCl what is the pH after 10ml of 1.0M NaOH has been added?( Ka for HOCl=3.5*10^_8)
Given that Buffer A contains 200.0 mL 0.050 M HOCl and 400.0 mL 0.030 M NaOCl,...
Given that Buffer A contains 200.0 mL 0.050 M HOCl and 400.0 mL 0.030 M NaOCl, calculate 1. The pH of the buffer solution. 2. The pH of the solution after adding 10.0 mL 0.50 M HCl. 3. The pH of the solution after adding 20.0 mL 0.40 M NaOH
500 mL of a buffer solution contains 0.050 mol NaHSO3 and 0.031 mol Na2SO3. (a) What...
500 mL of a buffer solution contains 0.050 mol NaHSO3 and 0.031 mol Na2SO3. (a) What is the pH of the solution? (b) Write the net ionic equation for the reaction that occurs when NaOH is added to this buffer. (c) Calculate the new pH after 10. mL of 1.0 M NaOH is added to the buffer solution. d) calculate the buffer capacity (f) Calculate the new pH after 10. mL of 1.0 M NaOH is added to 500. mL...
Part A What is the pH of a buffer prepared by adding 0.809 mol of the...
Part A What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.406 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. Part B What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. What is the pH after 0.195 mol of NaOH is added to the buffer...
What is the pH of a buffer prepared by adding 0.809 mol of the weak acid...
What is the pH of a buffer prepared by adding 0.809 mol of the weak acid HA to 0.305 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7.? What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid? What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume...
A buffer solution contains 0.52 mol of hypochlorous acid (HClO) and 0.39 mol of sodium hypochlorite...
A buffer solution contains 0.52 mol of hypochlorous acid (HClO) and 0.39 mol of sodium hypochlorite (NaOCl) in 3.00 L. The Ka of hypochlorous acid (HClO) is Ka = 3e-08. (a) What is the pH of this buffer? pH =__________. (b) What is the pH of the buffer after the addition of 0.21 mol of NaOH? (assume no volume change) pH = ___________. (c) What is the pH of the original buffer after the addition of 0.20 mol of HI?...
Part A: What is the pH of a buffer prepared by adding 0.607 mol of the...
Part A: What is the pH of a buffer prepared by adding 0.607 mol of the weak acid HA to 0.507 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. Part B: What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Part C: What is the pH after 0.195 mol of NaOH is added to...
Part A.) What is the pH of a buffer prepared by adding 0.708 mol of the...
Part A.) What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.406 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. Part B.) What is the pH after 0.150 mol of HCl is added to the buffer from Part A? Assume no volume change on the addition of the acid. Part C.) What is the pH after 0.195 mol of NaOH is added to...
1.) A buffer solution contains 0.455 M NH4Cl and 0.295 M NH3 (ammonia). Determine the pH...
1.) A buffer solution contains 0.455 M NH4Cl and 0.295 M NH3 (ammonia). Determine the pH change when 0.085 mol NaOH is added to 1.00 L of the buffer. pH after addition − pH before addition = pH change = 2.) Determine the pH change when 0.044 mol HNO3 is added to 1.00 L of a buffer solution that is 0.462 M in HF and 0.218 M in F-. pH after addition − pH before addition = pH change =
1) A buffer solution contains 0.388 M NH3. Determine the pH change when 0.088 mol NaOH...
1) A buffer solution contains 0.388 M NH3. Determine the pH change when 0.088 mol NaOH is added to 1.00 L of the buffer. 2) Determine the pH change when 0.070 mol HBR is added to 1.00 L of a buffer that is 0.49u M HF and 0.302 M in F-. Please show work
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT