a) How many grams of sodium acetate, NACH3COO (molar mass: 82.0343 g/mol) should be combined with 0.10 M acetic acid, CH3COOH (pka = 4.74) to prepare a 0.50 L acetate buffer of pH 5.10. You may use the Henderson-Hasselbalch equation shown below. (3 points) [conjugate base] pH = pKa + log Tweak acid]

a) How many grams of sodium acetate, NACH3COO (molar mass: 82.0343 g/mol) should be combined with 0.10 M acetic acid, CH3COOH (pka = 4.74) to prepare a 0.50 L acetate buffer of pH 5.10. You may use the Henderson-Hasselbalch equation shown below. (3 points) [conjugate base] pH = pKa + log Tweak acid]

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 34QAP: A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of...

See similar textbooks

Similar questions

Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
A buffer is composed of formic acid and its conjugate base, the formate ion. (a) What is the pH of a solution that has a formic acid concentration of 0.050 M and a sodium formate concentration of 0.035 M? (b) What must the ratio of acid to conjugate base be to have a pH value 0.50 units higher than the value calculated in part (a)?
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
You wish to prepare a buffer consisting of acetic acid and sodium acetate with a total acetic acid plus acetate concentration of 250 mM and a pH of 5.0. What concentrations of acetic acid and sodium acetate should you use? Assuming you wish to make 2 liters of this buffer, how many moles of acetic acid and sodium acetate will you need? How many grams of each will you need (molecular weights: acetic acid 60.05 g mol^-1, sodium acetate, 82.03 g mol^-1)?
You make a 200mM potassium phosphate buffer (pKa of 7.20) with monobasic potassium phosphate (molecular weight 136.09 g/mol) and dibasic potassium phosphate (174.20 g/mol). For 100mL of buffer, at a pH of 7.20, how many grams of monobasic potassium phosphate are needed? Please walk through this step-by-step.
You prepare a buffer by mixing 0.15 mol propanoic acid (pKa = 4.87) and 0.25 mol sodium propionate. You than add 0.025 mol of sodium hydroxide (NaOH) to the buffer mixture (assume there is no change in volume). What would the pH be after addition of NaOH? The answer is pH = 5.21 but I do not know how to get that answer.
How many grams of sodium fluoride should be added to 40.0 mL of 0.223 M hydrofluoric acid solution to produce a buffer of pH 4.70 with a total diluted volume of 500. mL? The Ka for hydrofluoric acid is 7.20x10-4. Group of answer choices 0.0103 g 0.129 g 13.6 g 27.2 g 170. g
A 1.0-LL buffer solution initially contains 0.30 molmol of NH3NH3 (Kb=1.76×10−5)(Kb=1.76×10−5) and 0.30 molmol of NH4ClNH4Cl. What mass of the correct reagent should you add? Express your answer using two significant figures.
Suppose there is 1.00 L of an aqueous buffer containing 0.0600 mol of benzoic acid (pKa = 4.20) and 0.0400 mol of benzoate (the conjugate base of benzoic acid). What volume of 2.50 M NaOH would be required to make the pH of this buffer solution equal to 4.93? Group of answer choices 7.5 mL 18 mL 21 mL 32 mL 8.1 mL 3.2 × 102 mL 5.6 mL91
You are making a potassium phosphate buffer that has 50 mM total phosphate (weighed out as KH2PO4), 160 mM KCl, and 7 mM dithiothreitol. You need 377 mL of buffer, which will be titrated to pH 50. What volume of a 2 M KH2PO4 stock solution should you add to the flask before diluting it to the final volume for your buffer? Report the volume in mL to the nearest 0.1 mL.
Your goal is to make a buffer with a pH of 4.75 from acetic acid and sodium acetate. Assume the pKa for acetic acid is 4.74. What is the volume of 1 M sodium acetate added to make your buffer? Report your answer to the tenths place. To do this, we use the Henderson-Hasselbach Equation pH = pkA + log (base/acid) where pkA = 4.74 for acetic acid, pH = target pH and [base] /[acid] = x/(1-x) since we don't know the concentration of the base, we will call it x the acid is just 1-x, assuming the two add up to 100% solve for x, and then you know the mL of base and acid to add.