Design a buffer that has a pH of 3.35 using one of the weak acid/conjugate base systems shown below.Weak Acid Conjugate BaseKapkaHC2O4H2PO4C2042-HPO2-6.4×10-54.196.2x10-87.21HCO3CO32-4.8x10-1110.32How many grams of the sodium salt of the weak acid must be combined with how many grams of the sodium salt of itsconjugate base, to produce 1.00 L of a buffer that is 1.00 M in the weak base?grams sodium salt of weak acid =ggrams sodium salt of conjugate base=g

For the first part, to create a buffer with a desired pH, we can use the Henderson-Hasselbalch…

Answered: Design a buffer that has a pH of 3.35…

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...

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Design a buffer that has a pH of 4.66 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ka pKa HC2O4- C2O42- 6.4 × 10-5 4.19 H2PO4- HPO42- 6.2 × 10-8 7.21 HCO3- CO32- 4.8 × 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 a buffer that is 1.00 M in the weak base?grams potassium salt of weak acid = grams potassium salt of conjugate base =
Which of the following will give a buffer with a pH near 4.76 when the acid and conjugate base are mixed in equimolar proportions? Acid NH4* (from ammonia) HC₂H3O2 (acetic acid) HF (hydrofluoric acid) CH3CH₂NH3 (from ethylamine) acetic acid. b) ethylamine c) ammonia d) hydrofluoric acid e) none Ka 5.69 10-10 1.75 10-5 6.810-4 2.12 10-11
Pp
Ka of acetic acid equals 1.8*10^-5 The buffer solution is 50 mL of 0.2 M CH3CO2H and 50 mL of 0.2 M NaCH3CO2together in a beaker. What is the theoretical pH of each soluton? a. 50 mL of boiled deionized water + 5 mL of 0.2 M HClb. 50 mL of boiled deionized water + 5 mL of 0.2 M NaOHc. 50 mL of buffer + 5 mL of 0.2 M HCld. 50 mL of buffer + 5 mL of 0.2 M NaOH
Design a buffer that has a pH of 6.70 using one of the weak acid/conjugate base systems shown below. Weak Acid Conjugate Base Ką pKa HC,04 C,0,²- 6.4 x 10-5 4.19 H,PO4 HPO,2- 6.2 x 10-8 7.21 HCO3 co,?- 4.8 × 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 a buffer that is 1.00 M in the weak base? grams potassium salt of weak acid = grams potassium salt of conjugate base =
Find the ph of a buffer solution that is made by mixing 30ml of 1M NaA and 30ml of 1M HA. Find the ph when 2ml of 1M HCl is added to 30ml of this buffer solution. Given (Ka = 2.11*10^-5)
Which acid would be best to use when preparing a buffer with a pH of 4.76? A list of Ka values can be found in this table. Ohypoiodous acid O hydrazoic acid Ochloroacetic acid O formic acid
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 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
Assuming equal concentrations of conjugate base and acid, which one of the following mixtures is best suited for preparing a buffer solution with pH of 4.74? Question 2 options: NH3 / NH4Cl (Ka = 5.6 × 10–10) NaNO2 / HNO2 (Ka = 4.5 × 10–4) CH3COONa / CH3COOH (Ka = 1.8 × 10–5) NaCl / HCl NaOCl / HOCl (Ka = 3.2 × 10–8)
Which of the following acid/base pairs would not make a good buffer system? H2PO4-/ HPO42- HSO3-/Na2SO3 H2CO3/H2CO2- NH4+/NH3 HNO2/NO2-
ortant values if needed for this question. Design a buffer that has a pH of 4.66 using one of the weak base/conjugate acid systems shown below. Ka pka 2.4x10-11 10.62 1.7x10-8 7.77 6.7x10-6 5.17 Weak Base Kb Conjugate Acid 4.2x 10-4 CH3NH3+ CH3NH₂ C6H1503N 5.9x107 C6H1503NH+ C5H5N 1.5x109 C5H5NH+ How many grams of the chloride salt of the conjugate acid must be combined with how many grams of the weak base, to produce 1.00 L of a buffer that is 1.00 M in the weak base? grams chloride salt of conjugate acid = grams weak base =

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