A buffer is made up of 15.0 ml of 0.1 M HC,H,02 and 15.0 ml of 0.1 MNa CH,O, The solution is diluted with 30.0 mL of water. Five drops of 0.1 M HCI is added. What was observed to happen to the pH and why? O pH increases by 0.1, because OH minus reacts with some of the conjugate acid leading to a small increase in pH. pH decreases by 0.1, because H* reacts with some of the conjugate base leading to a small decrease in pH. O pH decreases by 7, because OH minus reacts with all of the conjugate acid leading to a large decrease in pH. O pH decreases by 7, because H* reacts with all of the conjugate base leading to a large decrease in pH. OpH increases by 7. because OH mìnus to a large increase in pH. reacts with all of the conjugate acid leading O pH increases by 7, because H* reacts with all of the conjugate base leading to a large increase in pH. O pH decreases by 0.1, because OH minus reacts with some of the conjugate acid leading to a small decrease in pH. O pH increases by 0.1. because H reacts with some of the conjugate base leading to a small increase in pH.

A buffer is made up of 15.0 ml of 0.1 M HC,H,02 and 15.0 ml of 0.1 MNa CH,O, The solution is diluted with 30.0 mL of water. Five drops of 0.1 M HCI is added. What was observed to happen to the pH and why? O pH increases by 0.1, because OH minus reacts with some of the conjugate acid leading to a small increase in pH. pH decreases by 0.1, because H* reacts with some of the conjugate base leading to a small decrease in pH. O pH decreases by 7, because OH minus reacts with all of the conjugate acid leading to a large decrease in pH. O pH decreases by 7, because H* reacts with all of the conjugate base leading to a large decrease in pH. OpH increases by 7. because OH mìnus to a large increase in pH. reacts with all of the conjugate acid leading O pH increases by 7, because H* reacts with all of the conjugate base leading to a large increase in pH. O pH decreases by 0.1, because OH minus reacts with some of the conjugate acid leading to a small decrease in pH. O pH increases by 0.1. because H reacts with some of the conjugate base leading to a small increase in pH.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 57P

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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.
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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.)
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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?
Two drops of indicator HIn (Ka = 1.0 109), where HIn is yellow and In is blue, are placed in 100.0 mL of 0.10 M HCl. a. What color is the solution initially? b. The solution is titrated with 0.10 M NaOH. At what pH will the color change (yellow to greenish yellow) occur? c. What color will the solution be after 200.0 mL NaOH has been added?
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A buffer solution is prepared from 5.15 g NH4NO3 and 0.10 L of 0.15-M NH3; calculate the pH of the solution.
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?