Please calculate the following for the buffers below: Phosphate (pH = 7.5) What is the ratio...
Please calculate the following for the buffers below:
-
Phosphate (pH = 7.5)
- What is the ratio of A-/HA in your buffer after your adjusted its pH to the required value?
- How many micromoles of A- and HA are present in the solution?
- If you now add 3mL of 1 NaOH, will you still have a valid buffer?
- CAS (pH = 10.5)
-
If you now add 3mL of 1 NaOH, will you still have a valid buffer?
-
How many micromoles of A- and HA are present in the solution?
-
What is the ratio of A-/HA in your buffer after your adjusted its pH to the required value
-
Homework Answers
The three pka value of phosphoric acid are 2.16, 7.21 and 12.32.
To prepare a buffer of 7.5, we need to use the pka value of 7.5.
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Please calculate the following for the buffers below:
Phosphate (pH = 7.5)
What is the ratio...
what is the ratio of A-/HA in your buffer chosen for part C before adding acid...
what is the ratio of A-/HA in your buffer chosen for part C before adding acid or base? How many micromoles of A- and HA are present in the solution? buffer chosen: citrate pH:4.82 pka:4.75 I need help with the micromoles part of the question. I have already found the ratio as 1.17
± pH Changes in Buffers Part A What is the pH of a buffer prepared by...
± pH Changes in Buffers Part A What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.608 mol of NaA in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10−7. Express the pH numerically to three decimal places. 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. Express...
1. You have a 1L solution of 0.1 M phosphate buffer at pH 2.0. What is...
1. You have a 1L solution of 0.1 M phosphate buffer at pH 2.0. What is the pH of this solution after you add 5 grams of NaOH? Assume there is no volume change and phosphate buffer has the following pKa values: 2.15, 6.82 and 12.38.
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-...
In our experiment, we will be using a portion of the phosphate buffer system that is...
In our experiment, we will be using a portion of the phosphate buffer system that is based upon the following equilibrium: H2PO4- HPO42- + H+ pKa = 7.2 In this case, H2PO4- will act as the acid and HPO42- will act as the base. Materials: 1M NaOH: 40.01 g/L of solution 1M HCl: 83 mL conc. HCl/L of solution Potassium phosphate, dibasic, K2HPO4, MW= 174.18 Potassium phosphate, monobasic, KH2PO4 MW= 136.09 **I already preformed this lab, but I struggled a...
Using a 0.30 M phosphate buffer with a pH of 8.0, you add 0.70 mL of...
Using a 0.30 M phosphate buffer with a pH of 8.0, you
add 0.70 mL of 0.55 M HCl to 52 mL of the buffer. What is
the new pH of the solution? (Enter your answer to three significant
figures.)
Using a 0.30 M phosphate buffer with a pH of 8.0, you add
0.70 mL of 0.55 M NaOH to 52 mL of the buffer. What is the
new pH of the solution? (Enter your answer to three significant...
A.)Using a 0.25 M phosphate buffer with a pH of 7.4, you add 0.70 mL of...
A.)Using a 0.25 M phosphate buffer with a pH of 7.4, you add 0.70 mL of 0.53 M HCl to 52 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) B.)Using a 0.25 M phosphate buffer with a pH of 7.4, you add 0.70 mL of 0.53 M NaOH to 52 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.20 M phosphate buffer with a pH of 6.2, you add 0.77 mL of...
Using a 0.20 M phosphate buffer with a pH of 6.2, you add 0.77 mL of 0.45 M HCl to 48 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) Using a 0.20 M phosphate buffer with a pH of 6.2, you add 0.77 mL of 0.45 M NaOH to 48 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.30 M phosphate buffer with a pH of 6.3, you add 0.72 mL of...
Using a 0.30 M phosphate buffer with a pH of 6.3, you add 0.72 mL of 0.54 M HCl to 60. mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) Using a 0.30 M phosphate buffer with a pH of 6.3, you add 0.72 mL of 0.54 M NaOH to 60. mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.)
Using a 0.20 M phosphate buffer with a pH of 6.4, you add 0.71 mL of...
Using a 0.20 M phosphate buffer with a pH of 6.4, you add 0.71 mL of 0.54 M HCl to 55 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) 49 Using a 0.20 M phosphate buffer with a pH of 6.4, you add 0.71 mL of 0.54 M NaOH to 55 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant...
Using a 0.30 M phosphate buffer with a pH of 8.0, you
add 0.70 mL of 0.55 M HCl to 52 mL of the buffer. What is
the new pH of the solution? (Enter your answer to three significant
figures.)
Using a 0.30 M phosphate buffer with a pH of 8.0, you add
0.70 mL of 0.55 M NaOH to 52 mL of the buffer. What is the
new pH of the solution? (Enter your answer to three significant...
Using a 0.20 M phosphate buffer with a pH of 6.4, you add 0.71 mL of 0.54 M HCl to 55 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant figures.) 49 Using a 0.20 M phosphate buffer with a pH of 6.4, you add 0.71 mL of 0.54 M NaOH to 55 mL of the buffer. What is the new pH of the solution? (Enter your answer to three significant...
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