How many grams of sodium acetate (salt) and acetic acid (acid) would be required to prepare 1 L of acetate buffer with a total buffer concentration of 0.6 moles/litre, given a mole fraction of salt (Xsalt) and acid (Xacid) of 0.75 and 0.25, respectively? [The molecular weight of sodium acetate (salt) is 82 g/mole and the molecular weight of acetic acid (acid) is 60 g/mole]. O a. sodium acetate = 110.7 g; acetic acid = 51 g b. sodium acetate = 27 g; acetic acid = 12.3 g C. sodium acetate = 29 g; acetic acid = 5.5 g d. sodium acetate = 36.9 g; acetic acid = 9g O e. sodium acetate = 12.3 g; acetic acid = 9 g

How many grams of sodium acetate (salt) and acetic acid (acid) would be required to prepare 1 L of acetate buffer with a total buffer concentration of 0.6 moles/litre, given a mole fraction of salt (Xsalt) and acid (Xacid) of 0.75 and 0.25, respectively? [The molecular weight of sodium acetate (salt) is 82 g/mole and the molecular weight of acetic acid (acid) is 60 g/mole]. O a. sodium acetate = 110.7 g; acetic acid = 51 g b. sodium acetate = 27 g; acetic acid = 12.3 g C. sodium acetate = 29 g; acetic acid = 5.5 g d. sodium acetate = 36.9 g; acetic acid = 9g O e. sodium acetate = 12.3 g; acetic acid = 9 g

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 37QAP: Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at...

See similar textbooks

Similar questions

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)?
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
When 40.00 mL of a weak monoprotic acid solution is titrated with 0.100-M NaOH, the equivalence point is reached when 35.00 mL base has been added. After 20.00 mL NaOH solution has been added, the titration mixture has a pH of 5.75. Calculate the ionization constant of the 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)?
A buffer is prepared by adding 2.50g of lithium fluoride to 125 mL of 0.648M hydrofluoric acid. You may assume there is no change in volume after the substances are mixed. 3. If 50.0 mL of 0.0750M nitric acid is added to the original buffer, what would be the pH?
A 0.600 g sample of a pure, weak diprotic acid gives end points at 20.0 mL and 40.0 mL when it is titrated with 0.100 M NaOH. What is the molar mass of the weak acid?
How will you prepare 500 ml of 0.750 M citrate buffer with pH of 4.25 from solid citric acid (C6H8O7) and solid sodium citrate (Na3C6H5O7).The Ka of citric acid is 7.40 x 10-4
The solubility products of Fe(OH)2 and Fe(OH)3 are 10-17 and 10-38 respectively. If the concentrationsof Fe2+ and Fe3+ are each 10-5, at what pH will each hydroxide just begin to precipitate? A compound containing chlorine is titrated with a solution of 0.075 M Ag2SO4. If 0.250 g of thesample requires 22.07 ml of Ag2SO4 to reach the endpoint, what is the mass percent of chlorine in thesample?
The solubility products of Fe(OH)2 and Fe(OH)3 are 10^-17 and 10^-38 respectively. If the concentrationsof Fe2+ and Fe3+ are each 10^-5, at what pH will each hydroxide just begin to precipitate?
What is the proper unit of molar ratio of weak acid and its conjugate base in a buffer solution? Is it mol to mol or part to part? Or is it unitless? I need to express the answer 1.45/1 = [A]/[HA] to the right unit. See image for more details. the buffer is acetic acid/sodium acetate buffer.
A buffer solution is prepared by dissolving 1.50 g each of benzoic acid, HC7H5O2, and sodium benzoate, NaC7H5O2, in 150.0 mL of solution. (MM of benzoic acid=122.22g/mol, sodium benzoate=144.11g/mol) Ka=6.3x10-5 What is the pH of this buffer solution? Which buffer component must be added, and in what quantity, to change the buffer pH to 4.00? What quantity of 2.0 M NaOH or 2.0 M HCl must be added to the original buffer to change the pH to 4.00?
A mixture of equal volumes of 0.1M solution of ethanoic acid and sodium ethanoate is a buffer solution. Give another example of a buffer solution. What is the main characteristic of buffer solutions?