Question

2. Determine the ratio of base to acid required to prepare a buffer solution with a...

2. Determine the ratio of base to acid required to prepare a buffer solution with a pH of 8.5. The Ka of the acid is 4.9 x 10^-10.

__________ mole of base for every __________ mole of acid

Homework Answers

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
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...
Prepare a buffer by acid–base reactions. Close Problem Consider how to prepare a buffer solution with...
Prepare a buffer by acid–base reactions. Close Problem 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...
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...
A buffer solution was made by mixing equal volumes of 0.200 M NaHSO3 solution and 0.100...
A buffer solution was made by mixing equal volumes of 0.200 M NaHSO3 solution and 0.100 M NaOH solution. (Ka of the weak acid, bisulfite(HSO3-), is 6.3 x 10-8 ) (a)       What is the pH of the above solution? (b)        If you added strong base NaOH to the above buffer solution until the pH reached 8.00, what is the mole ratio of the base to the acid. (i.e. [SO32-]/[HSO3-])?
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 to prepare a buffer solution with pH = 3.66 (using one of the weak...
Consider how to prepare a buffer solution with pH = 3.66 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.305-M solution of weak acid with 0.271 M sodium 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 sodium hydroxide solution would have to be added to the acid solution of your...
Consider how to prepare a buffer solution with pH = 9.52 (using one of the weak...
Consider how to prepare a buffer solution with pH = 9.52 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.417-M solution of weak acid with 0.284 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. How many L of the potassium hydroxide solution would have to be added to the acid solution of your...
Consider how to prepare a buffer solution with pH = 9.32 (using one of the weak...
Consider how to prepare a buffer solution with pH = 9.32 (using one of the weak acid/conjugate base systems shown here) by combining 1.00 L of a 0.427-M solution of weak acid with 0.284 M sodium 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 sodium hydroxide solution would have to be added to the acid solution of your...
Determine the volumes of each solution you would use to prepare a 1.0L of a pH...
Determine the volumes of each solution you would use to prepare a 1.0L of a pH 5.00 buffer. Choose solutions from the following list. For the answer, list the solution and the volume of that solution. 0.10 M HCOOH Ka = 1.8 x 10-4 0.10 M HCOONa 0.10 M CH3COOH Ka = 1.8 x 10-5 0.10 M CH3COONa 0.10 M HCN Ka = 4.9 x 10-10 0.10 M NaCN
2. Buffer capacity refers to the amount of acid or base a buffer can “absorb” without...
2. Buffer capacity refers to the amount of acid or base a buffer can “absorb” without a significant pH change. It is governed by the concentrations of the conjugate acid and base forms of the buffer. A 0.5 M buffer will require five times as much acid or base as a 0.1 M buffer for given pH change. In this problem you begin with a buffer of known pH and concentration and calculate the new pH after a particular quantity...
ADVERTISEMENT
Need Online Homework Help?

Get Answers For Free
Most questions answered within 1 hours.

Ask a Question
ADVERTISEMENT