Design a buffer that has a pH of 9.71 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base HC₂04 C₂04²- H₂PO4 HPO4²- HCO3 CO3²- Ka 6.4x10-5 6.2x10-8 4.8×10-11 pka 4.19 7.21 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 a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = grams potassium salt of conjugate base = g bo g

Design a buffer that has a pH of 9.71 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base HC₂04 C₂04²- H₂PO4 HPO4²- HCO3 CO3²- Ka 6.4x10-5 6.2x10-8 4.8×10-11 pka 4.19 7.21 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 a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = grams potassium salt of conjugate base = g bo g

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

What is a buffer? Choose 2. a solution that resists changes in pH a solution that neutralizes a basic solution a weak acid-base conjugate pair a solution that neutralizes an acidic solution a strong acid-base conjugate pair
Which of the following would make a good buffer system. Group of answer choices HI/BaI2 HNO3/NaOH CCl3CO2H/ LiCCl3CO2 - This is the correct answer, but why? H3PO4/Na2HPO4 -I chose this one and it is wrong, why is it wrong?
Pp
please answer both for a vote uofront. thanks (Please type answer no write by hend)
Which combination would be preferable to form a buffer? OWeak acid and its conjugate base Weak acid and its conjugate acid Strong acid and a strong base Weak acid and a weak base Strong acid and its conjugate base
Which of the following combinations is not suitable for making a buffer? NH4Cl and NH3 H3PO4 and NaH₂PO4 O NaH₂PO4 and Na₂HPO4 HCIO4 and NaC104 O Na₂CO3 and NaHCO3
Which of the following is not a characteristic of buffer solutions? O They cannot be tailored to maintain a specified pH. O They contain a conjugate base of a weak acid. O They contain a weak acid. O They have a finite capacity for accommodating added acid or base. O They can maintaln their pH, even when small amounts of acid or base are added. QUESTION 10 The capacity of a buffer solution is greater when there are large amounts of a weak acid and its conjugate base in solution. O True O False
A diprotic acid is titrated with a strong base. The pH at the first half-equivalence point is (3.69x10^0). The pH at the second half-equivalence point is (8.9000x10^0). What is the value of ka2? Enter your answer using 3 significant figures.
Buffer is 200 ml of 0.15 M Tris-HCl buffer with a pH of 8.9 Write out the chemical equation for this buffer. Identify which species is the conjugate acid and conjugate base. What is Pka of this equilibrium? Calculate the ratio of the base to acid using the Henderson-Hasselbach equation.
Which of the following acid/base pairs would not make a good buffer system? H2PO4-/ HPO42- HSO3-/Na2SO3 H2CO3/H2CO2- NH4+/NH3 HNO2/NO2-
What is the pH of an aqueous solution containing 75.0 mL of a 0.15M HNO2 solution and 45.0 mL of a .25M KNO2? What is the pH of this solution after 10.0 mL of a 0.20M solution of KOH is added? How would you categorize this problem (i.e. strong acid or weak acid titrated by strong base or weak base, buffer)?