The question is attached 2C. Properties of a Buffered SolutionpH of buffer (half-neutralized unknown) before the addition of other(strong acid)1.871.831.91pH of water with 5 drops of HC1||pH of buffer with 5 drops of HCIpH of buffer with 5 drops of NaOHpH of distilled water before the addition of other reagents2.37(Strong base)reagents6.51.86| Expected to belowerpH of water with 5 drops of NaOH10.51Balanced equations demonstrating buffering action using HA and NaA as the buffer:be)malvita

Answered: Image /qna-images/answer/bef8010e-c500-4cc1-96fb-3f039caa87fa.jpg

C. Properties of a Buffered Solution pH of buffer (half-neutralized unknown) before the addition of other: (strong acid) 1.83 pH of buffer with 5 drops of HCI pH of buffer with 5 drops of NaOH 1.91 pH of distilled water before the addition of other reagents 2.37 pH of water with 5 drops of HCl (Strong base) reagents 6.5 1.86 10.51 pH of water with 5 drops of NaOH Balanced equations demonstrating buffering action using HA and NaA as the buffer: Expected to be lower

C. Properties of a Buffered Solution pH of buffer (half-neutralized unknown) before the addition of other: (strong acid) 1.83 pH of buffer with 5 drops of HCI pH of buffer with 5 drops of NaOH 1.91 pH of distilled water before the addition of other reagents 2.37 pH of water with 5 drops of HCl (Strong base) reagents 6.5 1.86 10.51 pH of water with 5 drops of NaOH Balanced equations demonstrating buffering action using HA and NaA as the buffer: Expected to be lower

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 2ALQ: A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt...

See similar textbooks

Similar questions

The species called glacial acetic acid is 98% acetic acid by mass (d=1.0542g/mL). What volume of glacial acetic acid must be added to 100.0 mL of 1.25 M NaOH to give a buffer with a pH of 4.20?
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.)
A chemist needs a buffer with pH 4.35. How many milliliters of pure acetic acid (density = 1.049 g/mL) must be added to 465 mL of 0.0941 M NaOH solution to obtain such a buffer?
A chemist needs a buffer with pH 3.50. How many milliliters of pure formic acid (density = 1.220 g/mL) must be added to 375 mL of 0.0857 M NaOH solution to obtain such a buffer?
Ammonia gas is bubbled into 275 mL of water to make an aqueous solution of ammonia. To prepare a buffer with a pH of 9.56, 15.0 g of NH4Cl are added. How many liters of NH3; at 25C and 0.981 atm should be used to prepare the buffer? Assume no volume changes and ignore the vapor pressure of water.
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?
A 0.400-g sample of propionic acid was dissolved in water to give 50.0 mL of solution. This solution was titrated with 0.150 M NaOH. What was the pH of the solution when the equivalence point was reached?
A friend asks the following: Consider a buffered solution made up of the weak acid HA and its salt NaA. If a strong base like NaOH is added, the HA reacts with the OH to form A. Thus the amount of acid (HA) is decreased, and the amount of base (A) is increased. Analogously, adding HCI to the buffered solution forms more of the acid (HA) by reacting with the base (A). Thus how can we claim that a buffered solution resists changes in the pH of the solution? How would you explain buffering to this friend?