EBK INTRODUCTION TO CHEMISTRY
5th Edition
ISBN: 9781260162165
Author: BAUER
Publisher: MCGRAW HILL BOOK COMPANY
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Chapter 13, Problem 98QP
Interpretation Introduction
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If phenolphthalein has been added to 100 mL of a clear solution and the solution does not change color when the phenolphthalein is added, what can we deduce about the pH of the solution?
The phenolphthalein pH indicator is clear and colorless in an acidic solution, but it turns a pink in a basic solution. Knowing this, you examine two clear and colorless solutions. One, you are told is acidic and the other is basic. Furthermore, you are told that the acidic solution contains phenolphthalein. So which is which? You don’t know because both solutions are colorless. To find out, you add a drop of Solution 1 to Solution 2. A pink color appears for a moment, but then disappears. This tells you that
Select one:
a. you now need to try adding Solution 2 to Solution 1.
b. Solution 2 is acidic.
c. Solution 1 is acidic.
d. both solutions are now neutralized.
What happens if you add a little bit of a strong acid or strong base to a buffer's acidity? How does this compare to an acidic solution that hasn't been buffered?
Chapter 13 Solutions
EBK INTRODUCTION TO CHEMISTRY
Ch. 13 - How do acids and bases differ from other...Ch. 13 - Prob. 2QCCh. 13 - Prob. 3QCCh. 13 - Prob. 4QCCh. 13 - Prob. 5QCCh. 13 - Prob. 6QCCh. 13 - Prob. 1PPCh. 13 - Prob. 2PPCh. 13 - Prob. 3PPCh. 13 - Prob. 4PP
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Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Which of the following acids and its conjugate base would you use to make a buffer with a pH of 3.00? Explain your reasons: formic acid, lactic acid, nitrous acid.arrow_forwardSulfanilic acid (NH2C6H4SO3H) is used in manufacturing dyes. It ionizes in water according to the equilibrium equation NH2C6H4SO3H(aq)+H2O(l)NH2C6H4SO3(aq)+H3O+(aq)Ka=5.9104 A buffer is prepared by dissolving 0.20 mol of sulfanilicacid and 0.13 mol of sodium sulfanilate (NaNH2C6H4SO3) in water and diluting to 1.00 L. Compute the pH of the solution. Suppose 0.040 mol of HCl is added to the buffer.Calculate the pH of the solution that results.arrow_forwardMethyl orange, HMO, is a common acid-base indicator. In solution it ionizes according to the equation: HMOaqH+aq+MO-aqredyellow If methyl orange is added to distilled water, the solution turns yellow. If 1 drop or two of 6 M HCl is added to the yellow solution, it turns red. If to that solution one adds a few drops of 6 M NaOH, the color reverts to yellow. a. Why does adding 6 M HCl to the yellow solution of methyl orange tend to cause the color to change to red? Note that in solution HCl exists as H+ and Cl- ions. b. Why does adding 6 M NaOH to the red solution tend to make it turn back to yellow? Note that in solution NaOH exists as Na+ and OH- ions. How does increasing OH- shift Reaction 3 in the discussion section? How would the resulting change in H+ affect the dissociation reaction of HMO?arrow_forward
- A buffer solution has a pH value of 9.8. Which value in the set of pH values 8.79.79.89.910.9 is the most likely value for the buffer solution pH after a. a small amount of strong acid has been added? b. a small amount of strong base has been added?arrow_forwardExplain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.arrow_forward. Write the formulas for three combinations of weak acid and salt that would act as buffered solutions. For each of your combinations, write chemical equations showing how the components of the buffered solution would consume added acid and base.arrow_forward
- a.Calculate the pH of a buffer that is 0.1M in lactic acid, C2H4(OH)COOH, and 0.1M in sodium lactate, C2H4(OH)COONa. b.What is the pH of a buffer that is 1M in lactic acid and 1M in sodium lactate? c.What is the difference between the buffers described in parts a and b?arrow_forwardExplain why the hydrolysis of salts makes it necessary to have available in a laboratory more than one acid-base indicator for use in titrations.arrow_forwardsWhat happens when an acid is added to a solution containing the HF/F buffer system?arrow_forward
- What term is used to describe the formation of ions, in aqueous solution, from a. a molecular compound b. an ionic compoundarrow_forwardWhen might a pH meter be better than an indicator to determine the end point of an acid-base titration?arrow_forwardUsing the diagrams shown in Problem 10-117, which of the solutions would have the greatest buffer capacity, that is, greatest protection against pH change, when the following occurs? a. A strong acid is added to the solution. b. A strong base is added to the solution.arrow_forward
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