QUESTION 3How many moles of solid NaF would have to be added to 1.0 L of 0.152 M HF solution to achieve a buffer of pH 3.4? Assume there is no volume change.Ka for HF = 7.2 × 10-4QUESTION 4sodium acetateWhat molar ratio of sodium acetate to acetic acid,is required to create a buffer solution having a pH of 5.04 at 25°C?Ka for HC2H302 is 1.8 × 10 -5.acetic acid

Answered: Image /qna-images/answer/12d17adc-79b5-4f41-9533-9ffec20d8d17.jpg

QUESTION 3 How many moles of solid NaF would have to be added to 1.0 L of 0.152 M HF solution to achieve a buffer of pH 3.4? Assume there is no volume change. Ka for HF = 7.2 x 10 -4 QUESTION 4 sodium acetate What molar ratio of sodium acetate to acetic acid, is required to create a buffer solution having a pH of 5.04 at 25°C? Ka for HCH302 is 1.8 x 10 -5. acetic acid

QUESTION 3 How many moles of solid NaF would have to be added to 1.0 L of 0.152 M HF solution to achieve a buffer of pH 3.4? Assume there is no volume change. Ka for HF = 7.2 x 10 -4 QUESTION 4 sodium acetate What molar ratio of sodium acetate to acetic acid, is required to create a buffer solution having a pH of 5.04 at 25°C? Ka for HCH302 is 1.8 x 10 -5. acetic acid

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter14: Acid-base Equilibria

Section: Chapter Questions

Problem 100E: What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution...

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What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution with a pH of 9.26? (Him: Assume a negligible change in volume as the solid is added.)
View Policies Current Attempt in Progress Suppose we titrate 20.0 mL of 0.100M HCHO2 (K, = 1.8 × 10-4) with 0.100 M NaOH. Calculate the pH. Before any base is added: pH = i When half of the HCHO, has been neutralized: pH = After a total of 15.0 mL of base has been added: pH = At the equivalence point: pH =
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Question 4 of 5 How many moles of HCI need to be added to 200.0 mL of a 0.200 M solution of NaF to make a buffer with a pH of 3.40? (Ka for HF is 6.8 x 10 4) +/- 7.
Calculate the number of grams of ammonium chloride that must be added to 2.00 L of a 0.500 M ammonia solution to obtain a buffer of pH = 9.20. Assume the volume of the solution does not change as the solid is added. Kb for ammonia is 1.80 * 10-5. (a) 60.7 g (b) 30.4 g (c) 1.52 g (d) 0.568 g (e) 1.59 * 10-5
D Question 5 Which of the following gives a buffer solution when equal volumes of the two solutions are mixed? (select all that apply) 0.10 M NH3 and 0.10 M HCI 0.20 M NH3 and 0.10 M HCI 0.10 M NH4Cl and 0.10 M NH3 0.20 M NH4Cl and 0.10 M NaOH
Question 5 of 20 Determine the mass of solid NaCH3CO0 that must be dissolved in an existing 500.0 mL solution of 0.200 M CH3COOH to form a buffer with a pH equal to 5.00. The value of Ka for CH;COOH is 1.8 x 10-5 1 3 NEXT > Let x represent the original concentration of CH3COO" in the water. Based on the given values, set up the ICE table in order to determine the unknown. CH;COOH(aq)+ H2O(1) 1, H3O*(aq) + CH;COO (aq) Initial (M) Change (M) Equilibrium (M) 5 RESET 0.200 5.00 -5.00 1.0 x 10-9 -1.0 x 10-9 1.0 x 10-5 -1.0 x 10-5 1.8 x 10-5 -1.8 x 10-5 x +5.00 x -5.00 x + 1.0 x 10-9 x - 1.0 x 10-9 x + 1.0 x 1 x - 1.0 x 10- x + 1.8 x 10-5 x - 1.8 x 105 2.
Question 10 Which of the following statements about buffered solu- tions are true? Select all that apply. A Buffer solutions resist changes in the concentration of hyd roxide ions. A buffer solution may be made up of a strong acid and one of its salts. C Buffer solutions will not change very much if a small amou nt of strong acid is added to it. Buffer solutions will not change pH very much if a small a mount of weak base is added to it.
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