Question

In: Chemistry

III. Buffer Solutions A. Buffer 1 i. Measure out 10.0 mL of 1.0 M CH3COOH and...

III. Buffer Solutions

A. Buffer 1

i. Measure out 10.0 mL of 1.0 M CH3COOH and 25.0 mL of 1.0 M sodium acetate (NaCH3COO) into a beaker

2. What is the concentration of acetic acid in this solution after mixing. (include units) [CH3COOH] ?

3. What is the concentration of acetate ion in this solution after mixing.(include units) [CH3COO-] ?

4. Calculate the expected pH of this buffer solution.

5. Measured pH of this buffer solution pH: 5.31

I have no idea how to do number 2,3,4 and I have to repeat these processes/ questions for different solutions. If you could show me how to do these, I would greatly appreciate it! Thank you so much in advance.

Solutions

Expert Solution

2) . What is the concentration of acetic acid in this solution after mixing.

[CH3COOH] = millimoles of CH3COOH / total volume

                     = 10 x 1 / (10 +25)

                      = 0.286 M

[CH3COOH] = 0.286 M

3. What is the concentration of acetate ion in this solution after mixing

[CH3COO-] = millimoles of CH3COONa / total volume

                     = 25 x 1 / (10 +25)

                      = 0.714 M

[CH3COO-] = 0.714 M

4. Calculate the expected pH of this buffer solution.

millimoles of NaCH3COO = 25 x 1.0 = 25

millimoles of CH3COOH = 10 x 1.0 =10

this mixture is buffer

so

pH = pKa + log [CH3COONa ]/ [CH3COOH]

pH = 4.74 + log (25/10)

pH = 5.14

queen_honey_blossom answered 9 months ago
Next > < Previous

Related Solutions

Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 M CH3COONa. a)...
Calculate the pH of a buffer system containing 1.0 M CH3COOH and 1.0 M CH3COONa. a) Using the Henderson-Hasselbalch equation b) Making no assumptions about quantities (use the quadratic equation) c) Compare and explain your results in a) and b) d) What is the pH of a buffer system after the addition of 0.10 moles of gaseous HCl to a 1.0 L of the solution? Assume that the volume of the solution does not change when the HCl is added....
V. Buffer Solution from Strong Base and Weak Acid Measure out 30.0 mL of 1.0 M...
V. Buffer Solution from Strong Base and Weak Acid Measure out 30.0 mL of 1.0 M CH3COOH and 5.0 mL of 1.0 M NaOH into a beaker. 1. Calculate the total volume. (include units) Vol _________ 2. What is the concentration of acetic acid in this solution after mixing. (include units) [CH3COOH] _______ 3. What is the concentration of sodium hydroxide in this solution after mixing. (include units) [NaOH] __________ 4. Calculate the expected pH of this buffer solution. pH...
Buffer Solution from Strong Base and Weak Acid Solution= 30.0 mL of 1.0 M CH3COOH 5.0...
Buffer Solution from Strong Base and Weak Acid Solution= 30.0 mL of 1.0 M CH3COOH 5.0 mL of 1.0 M NaOH 1. Calculate the total volume. 35 mL 2. What is the concentration of acetic acid in this solution after mixing? (include units) 3. What is the concentration of sodium hydroxide in this solution after mixing (include units) 4. Calculate the expected pH of this buffer solution. 5. Measured pH of this buffer solution. 3.89
A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of...
A buffer is prepared by adding 150 mL of 1.0 M NaOH to 250 mL of 1.0 M NaH2PO4. How many moles of HCl must be added to this buffer solution to change the pH by 0.25 units? Assume the total volume remains unchanged at 400 mL. For H2PO4-, Ka = 6.3 × 10-8.
find the pH of a 40 mL buffer solution + 1.0 mL of 6.0 M HCl...
find the pH of a 40 mL buffer solution + 1.0 mL of 6.0 M HCl (aq) I know this question is pretty simple, but do I need to know what the buffer is made of? Is it important? if not how would I set up the ICE table? thank you!
You prepare a buffer solution from 10.0 mL of 0.100 M MOPS (3-morpholinopropane-1-sulfonic acid) and 10.0...
You prepare a buffer solution from 10.0 mL of 0.100 M MOPS (3-morpholinopropane-1-sulfonic acid) and 10.0 mL of 0.085 M NaOH. Next, you add 1.00 mL of 1.71 × 10-5 M lidocaine to this mixture Denoting lidocaine as L, calculate the fraction of lidocaine present in the form LH .
You prepare a buffer solution from 10.0 mL of 0.100 M MOPS (3-morpholinopropane-1-sulfonic acid) and 10.0...
You prepare a buffer solution from 10.0 mL of 0.100 M MOPS (3-morpholinopropane-1-sulfonic acid) and 10.0 mL of 0.079 M NaOH. Next, you add 1.00 mL of 1.65 × 10-5 M lidocaine to this mixture Denoting lidocaine as L, calculate the fraction of lidocaine present in the form LH . ka=6.3e-8 kb=8.7e-7
You prepare a buffer solution from 10.0 mL of 0.100 M MOPS (3-morpholinopropane-1-sulfonic acid) and 10.0...
You prepare a buffer solution from 10.0 mL of 0.100 M MOPS (3-morpholinopropane-1-sulfonic acid) and 10.0 mL of 0.079 M NaOH. Next, you add 1.00 mL of 5.67 × 10^-5 M lidocaine to this mixture. Denoting lidocaine as L, calculate the fraction of lidocaine present in the form LH+. MOPS Ka = 6.3 × 10^–8. Lidocaine Kb = 8.7 × 10^–7 (Hint: First calculate the pH of the solution from the amount of MOPS added. Start by finding the number...
A 250.00 mL buffer solution is 0.250 M acetic acid (CH3COOH) and 0.100 M sodium acetate...
A 250.00 mL buffer solution is 0.250 M acetic acid (CH3COOH) and 0.100 M sodium acetate (NaCH3COO). The Ka of acetic acid is 1.8 • 10-5 at 25 o C. Calculate the pH of the resulting buffer solution when 10.00 mL of a 0.500 M aqueous HCl solution is added to this mixture.
A student creates a buffer mixing 50. mL of 1.0 M Acetic Acid with 25 mL...
A student creates a buffer mixing 50. mL of 1.0 M Acetic Acid with 25 mL of 1.0 M Sodium Hydroxide. The buffer is then mixed with 10. mL of 2.0 M hydrobromic acid. What is the pH of the final solution? The Ka of acetic acid is 1.8 x 10-5
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT