Consider a solution where fa for a weak acid HAc (acetic acid) is 0.010M. pKa for...
Consider a solution where fa for a weak acid HAc (acetic acid) is 0.010M. pKa for this acid is 4.76
|
pH |
[Ac‒] |
[HA] |
|
13.00 |
0.0100 |
|
|
11.00 |
0.0100 |
|
|
9.00 |
0.0100 |
|
|
8.00 |
0.0100 |
|
|
7.00 |
9.96 X 10‒3 |
|
|
6.00 |
9.58 X 10‒3 |
|
|
5.00 |
6.93 X 10‒3 |
|
|
4.00 |
1.84 X 10‒3 |
|
|
3.00 |
2.21X 10‒4 |
|
|
2.00 |
2.25 X 10‒5 |
|
|
1.00 |
2.26 X 10‒6 |
The formal concentration of the acetic acid was fa = 0.010M. Using the mass balance calculate the value of [HA] at each pH and enter those number in to the table. Please show work.
Homework Answers
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Consider a solution where fa for a weak acid HAc (acetic acid)
is 0.010M. pKa for...
Given that the pKa for the half equivalence point is = 5.5, and the pKa of...
Given that the pKa for the half equivalence point is =
5.5, and the pKa of Acetic acid is 4.76, what is the percent
error?
Is 4.76 the accepted value?
and 5.5 the experimental?
and so...
|4.76-5.5| = -0.74
--------- ----- = 0.15546 ×100% = 15.55%
|4.76|
|4.76|
Please verify I am correct.
Vinegar Titration Curve / / 14.00 13.00 12.00 11.00 10.00 9.00 8.00 E 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 0.00 5.00 10.00 25.00 30.00...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that m the first question. STRATEGY 1. Rearrange the Hendereon-Hasselbalch equation to solve for thfe rabo of base (acetate) to aad (acetic add).[A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration ot acetic acid.
The PH of 0.010M of a weak acid (HA) is PH - 2.40. What is the...
The PH of 0.010M of a weak acid (HA) is PH - 2.40. What is the Ka value of the weak acd? O A 41 x 10²3 B. 1.8 x 10-4 0C 3.5x10-5 0.65 x 10-6 E. 1.6x109
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that in the first question. 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. That is, there are...
1) An acetic acid aqueous solution has a pKa of 4.76 and pH of 3.00. What...
1) An acetic acid aqueous solution has a pKa of 4.76 and pH of 3.00. What is the concentration of acetic acid? 2) An experiment requires you to culture mammalian cells in 10 mL of culture medium buffered to a pH of 7.4 with 25 mM HEPES. After the experiment, the pH dropped to 7.0. How many equivalents of acid must have been produced by the cells to have dropped the pH?
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.20 M buffer solution at pH 5.0? Note that the concentration, pH value, or both may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). [A-V[HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1:...
Resources Ex Give Up? What concentrations of acetic acid (pka = 4.76) and acetate would be...
Resources Ex Give Up? What concentrations of acetic acid (pka = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.92 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [ A HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate...
Question 4. a.) Calculate the pH of a solution initially 0.1 M in acetic acid and 0.02 M in sodium acetate. The pKa for acetic acid is 4.76. b) Calculate the pH of the buffer if you add 10 ml of 0.1M...
Question 4. a.) Calculate the pH of a solution initially 0.1 M in acetic acid and 0.02 M in sodium acetate. The pKa for acetic acid is 4.76. b) Calculate the pH of the buffer if you add 10 ml of 0.1M HCl to 100 ml of the buffer in part a.
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10...
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.5? Note that the concentration and/or pH value may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid Step 1: Rearrange the Henderson Hasselbalch...
Which of the following compounds would make the best buffer at pH 7.5? Acetic acid, pKa=...
Which of the following compounds would make the best buffer at pH 7.5? Acetic acid, pKa= 4.76 N-tris(hydroxymethyl) methylglycine (Tricine), pKa = 8.15 N-2-hydroxyethylpiperazine-N’-ethansulfonic acid, pKa2= 7.6 Glycine, pKa2= 9.9 Tris(hydroxymethyl)aminomethane (Tris), pKa = 8.3 I believe 3 is the correct answer and therefore I am trying to answer the below question with this information. Using the answer that you selected from question 1 above: a. Explain how you would make the buffer starting with 1M HA and 1M A-...
Given that the pKa for the half equivalence point is =
5.5, and the pKa of Acetic acid is 4.76, what is the percent
error?
Is 4.76 the accepted value?
and 5.5 the experimental?
and so...
|4.76-5.5| = -0.74
--------- ----- = 0.15546 ×100% = 15.55%
|4.76|
|4.76|
Please verify I am correct.
Vinegar Titration Curve / / 14.00 13.00 12.00 11.00 10.00 9.00 8.00 E 7.00 6.00 5.00 4.00 3.00 2.00 1.00 0.00 0.00 5.00 10.00 25.00 30.00...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that m the first question. STRATEGY 1. Rearrange the Hendereon-Hasselbalch equation to solve for thfe rabo of base (acetate) to aad (acetic add).[A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration ot acetic acid.
The PH of 0.010M of a weak acid (HA) is PH - 2.40. What is the Ka value of the weak acd? O A 41 x 10²3 B. 1.8 x 10-4 0C 3.5x10-5 0.65 x 10-6 E. 1.6x109
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.9? Note that the concentration and/or pH value may differ from that in the first question. 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [A^-]/[HA]. 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. That is, there are...
What concentrations of acetic acid (pKa = 4.76) and acetate would be required to prepare a 0.20 M buffer solution at pH 5.0? Note that the concentration, pH value, or both may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid). [A-V[HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid. Step 1:...
Resources Ex Give Up? What concentrations of acetic acid (pka = 4.76) and acetate would be required to prepare a 0.15 M buffer solution at pH 4.92 Note that the concentration, the pH, or both values may differ from that in the first question. Strategy 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic acid), [ A HA). 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate...
What concentrations of acetic acid (pKa 4.76) and acetate would be required to prepare a 0.10 M buffer solution at pH 4.5? Note that the concentration and/or pH value may differ from that in the first question. STRATEGY 1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio of base (acetate) to acid (acetic 2. Use the mole fraction of acetate to calculate the concentration of acetate. 3. Calculate the concentration of acetic acid Step 1: Rearrange the Henderson Hasselbalch...
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