Question

Write a procedure so a lab mate could prepare 100 mL of buffer solution of that...

Write a procedure so a lab mate could prepare 100 mL of buffer solution of that pH from two solids. Your procedure should clearly indentify which glassware and chemicals you will use to prepare the solution. Assume that you will use the sodium salt of the conjugate base to prepare the solution. Our desired pH is 7.5 and the weak acid I chose is Sodium hydrogen sulfite with pKa of 7.21.

Use Henderson-Hasselbalch equation to determine molequantities of the weak acid and its conjugate base that you will need to prepare the solution.

Calculate the masses of the weak acids and its conjugate base needed to get the correct pH.

Write a 5-8 step detailed procedure that explains how to actually prepare the buffer solution.

Homework Answers

Answer #1

The conjugate base of hydrogen sulphite is sulphate.

Now, using the Henderson-Hasselbach equation, we can calculate the acid/base ratio:

If you choose sodium hydrogen sulphite and sodium sulphate.

  

The mass ratio is:

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
You need to prepare a buffer for biochemistry lab. The required solution is 0.5Msodium phosphate, pH...
You need to prepare a buffer for biochemistry lab. The required solution is 0.5Msodium phosphate, pH 7.0. Use the Henderson-Hasselbalch equation to calculate the number of moles and grams of moobasic sodium phosphate ( NaH2PO4) and dibasic sodium phosphate ( Na2HPO4) necessary to make 1 liter of solution. The pKa for this buffer is 7.21
Prepare a buffer by direct addition. Consider how best to prepare one liter of a buffer...
Prepare a buffer by direct addition. Consider how best to prepare one liter of a buffer solution with pH = 3.62 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32 How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate...
Consider how best to prepare one liter of a buffer solution with pH = 8.09 using...
Consider how best to prepare one liter of a buffer solution with pH = 8.09 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32 How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate base, to produce 1.00 L of...
Consider how best to prepare one liter of a buffer solution with pH = 6.55 using...
Consider how best to prepare one liter of a buffer solution with pH = 6.55 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32 How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of its conjugate base, to produce 1.00 L of...
you need to prepare a buffer solution with a ph of 7.8. A lab mate tells...
you need to prepare a buffer solution with a ph of 7.8. A lab mate tells you to use N-2- hydroxyethylpiperazine-N'-2-ethanesulfonic acid(HEPES), a sulfonic acid with a pka of 7.5. since you know that the buffer pka should be close to the desired pH, this sounds good. You make the solution according to the following recipe, which is supposed to make 600 ml of a 0.5 M solution: dissolve 0.2 moles of HEPES in 400 ml of water. add 0.1...
Consider how best to prepare one liter of a buffer solution with pH = 10.92 using...
Consider how best to prepare one liter of a buffer solution with pH = 10.92 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32 How many grams of the potassium salt of the weak acid must be combined with how many grams of the potassium salt of its conjugate base, to produce 1.00 L of...
Consider how best to prepare one liter of a buffer solution with pH = 11.12 using...
Consider how best to prepare one liter of a buffer solution with pH = 11.12 using one of the weak acid/conjugate base systems shown here. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 x 10-5 4.19 H2PO4- HPO42- 6.2 x 10-8 7.21 HCO3- CO32- 4.8 x 10-11 10.32    How many grams of the potassium salt of the weak acid must be combined with how many grams of thepotassium salt of its conjugate base, to produce 1.00 L of...
To prepare 100 mL of 25 mM Tris buffer at pH 8.0, calculate the amount of...
To prepare 100 mL of 25 mM Tris buffer at pH 8.0, calculate the amount of Tris base and Tris·HCl needed to make the buffer. (Hint: find out the pKa of Tris·HCl and use the Henderson-Hasselbalch Equation.) Describe how do you want to make the solution, including how much water to add, how to adjust pH, etc.
2) Two students want to prepare 2.0 L of a buffer solution which must be buffered...
2) Two students want to prepare 2.0 L of a buffer solution which must be buffered at a pH of 4.75. Student A wants to use acetic acid (CH3COOH, Ka = 1.8 x 10-5) and sodium acetate to prepare the buffer solution, while student B wants to use formic acid (HCOOH, Ka = 1.8 x 10-4) and sodium formate. Which student chose the better conjugate acid-base pair to prepare the buffer? Why? Explain the step-by- step procedure that the students...
Prepare a buffer by acid–base reactions. Consider how to prepare a buffer solution with pH =...
Prepare a buffer by acid–base reactions. Consider how to prepare a buffer solution with pH = 9.31 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.316-M solution of weak acid with 0.351 M potassium hydroxide. Weak Acid Conjugate Base Ka pKa HNO2 NO2- 4.5 x 10-4 3.35 HClO ClO- 3.5 x 10-8 7.46 HCN CN- 4.0 x 10-10 9.40 How many L of the potassium hydroxide solution would have to be added...