Question 1 of 16 A student must make a buffer solution with a pH of 7.00. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, K, - 1.34 x 10,3.00 M O ammonium citrate, K₂=4.06 x 107, 2.00 M O acetic acid, K₂= 1.75 x 10,5.00 M Osodium dihydrogen phosphate monohydrate, K₁= 6.23 x 10", 2.00 M Determine which conjugate base is the best option to make a buffer at the specified pH. O sodium propionate, CH₂CH₂COONa O sodium citrate dihydrate, C,H,O,Na, -2H₂O O disodium hydrogen phosphate heptahydrate, Na,HPO, 7H₂O sodium acetate trihydrate, CH,COONa-3H₂O The final volume of buffer solution must be 100.00 mL. and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 7.00? mass= Based on this information, what volume of acid should the student measure to make the buffer solution? volume= mL

Question 1 of 16 A student must make a buffer solution with a pH of 7.00. Determine which weak acid is the best option to make a buffer at the specified pH. O propionic acid, K, - 1.34 x 10,3.00 M O ammonium citrate, K₂=4.06 x 107, 2.00 M O acetic acid, K₂= 1.75 x 10,5.00 M Osodium dihydrogen phosphate monohydrate, K₁= 6.23 x 10", 2.00 M Determine which conjugate base is the best option to make a buffer at the specified pH. O sodium propionate, CH₂CH₂COONa O sodium citrate dihydrate, C,H,O,Na, -2H₂O O disodium hydrogen phosphate heptahydrate, Na,HPO, 7H₂O sodium acetate trihydrate, CH,COONa-3H₂O The final volume of buffer solution must be 100.00 mL. and the final concentration of the weak acid must be 0.100 M. Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 7.00? mass= Based on this information, what volume of acid should the student measure to make the buffer solution? volume= mL

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter14: Acid- Base Equilibria

Section: Chapter Questions

Problem 4RQ: A good buffer generally contains relatively equal concentrations of weak acid and conjugate base. If...

See similar textbooks

Similar questions

2. If an acetic acid/sodium acetate buffer solution is prepared from 100. mL of 0.10 M acetic acid what volume of 0.10 M sodium acetate must be added to have a pH of 4.00? 100. mL 50. mL 36 mL 18 mL
You want to make a buffer with a pH of 10.00 from NH4+/NH3. (a) What must the [ NH4+ ]/[ NH3 ]ratio be? (b) How many moles of NH4Cl must be added to 465 mL of an aqueous solution of 1.24 M NH3 to give this pH? (c) How many milliliters of 0.236 M NH3 must be added to 2.08 g of NH4Cl to give this pH? (d) What volume of 0.499 M NH3 must be added to 395 mL, of 0.109 M NH4Cl to give this pH?
What is the pH of a buffer that is 0.175 M in a weak acid and 0.200 M in the acids conjugate base? The acids ionization constant is 5.7 104.
A sodium hydrogen carbonate-sodium carbonate buffer is to be prepared with a pH of 9.40. (a) What must the [ HCO3 ]/[ CO32 ]ratio be? (b) How many moles of sodium hydrogen carbonate must be added to a liter of 0.225 M Na2CO3 to give this pH? (c) How many grams of sodium carbonate must be added to 475 mL of 0.336 M NaHCO3 to give this pH? (Assume no volume change.) (d) What volume of 0.200 M NaHCO3 must be added to 735 mL of a 0.139 M solution of Na2CO3 to give this pH? (Assume that volumes are additive.)
8-94 Suppose you wish to make a buffer whose pH is 8.21. You have available 1 L of 0.100 M NaH2PO4 and solid Na2HPO4. How many grams of the solid Na2HPO4 must be added to the stock solution to accomplish this task? (Assume that the volume remains 1 L.)
Each symbol in the box below represents a mole of a component in one liter of a buffer solution; represents the anion (X-), = the weak acid (HX), = H+, and =OH. Water molecules and the few H+ and OH- ions from the dissociation of HX and X- are not shown. The box contains 10 mol of a weak acid, , in a liter of solution. Show what happens upon (a) the addition of 2 mol of OH- (2 ). (b) the addition of 5 mol of OH- (5 ). (c) the addition of 10 mol of OH- (10 ). (d) the addition of 12 mol of OH- (12 ). Which addition (a)-(d) represents neutralization halfway to the equivalence point?
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.)
Which of the indicators in Fig. 14-8 could be used for the titrations in Exercises 61 and 63?
Enough water is added to the buffer in Question 30 to make the total volume 5.00 L. (a) Calculate the pH of the buffer. (b) Calculate the pH of the buffer after adding 0.0250 mol of HCl to 0.376 L of the buffer. (c) Calculate the pH of the buffer after adding 0.0250 mol of KOH to 0.376 L of the buffer. (d) Compare your answers to Question 30 (a-c) with your answers to (a-c) of this problem. (e) Comment on the effect of dilution on the pH of a buffer and on its buffer capacity. Â
8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI solution require the same amount of 1.0 M NaOH to hit a titration end point? Explain.
Consider the weak acids in Table 13.2. Which acid-base pair would be best for a buffer at a pH of (a) 3.0(b) 6.5 (c) 12.0
Calculate the pH after 0.010 mole of gaseous HCl is added to 250.0 mL of each of the following buffered solutions. a. 0.050 M NH3/0.15 M NH4Cl b. 0.50 M NH3/1.50 M NH4Cl Do the two original buffered solutions differ in their pH or their capacity? What advantage is there in having a buffer with a greater capacity?