Chemistry: An Atoms-Focused Approach
14th Edition
ISBN: 9780393912340
Author: Thomas R. Gilbert, Rein V. Kirss, Natalie Foster
Publisher: W. W. Norton & Company
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What is the effect of dilution on the pH of a buffer and the buffer’s capacity?
Buffer capacity refers to the amount of acid or base a buffer can absorb without a significant pH
change. It is governed by the concentrations of the conjugate acid and base components of the
buffer. A 0.5 M buffer can "absorb" five times as much acid or base as a 0.1 M buffer for a given
pH change. In this problem you begin with a buffer of known pH and concentration and calculate
the new pH after a particular quantity of acid or base is added.
4.
You are given 60 mL of 0.50 M phosphate buffer, pH = 6.83, to test. The starting composition of
the buffer, both in terms of the concentration and the molar quantity of the two major phosphate
species, is:
Concentration of HPO,²: 0.304 M
Molar quantity of HPO,: 18.2 mmol
Concentration of H,PO*: 0.196 M
Molar quantity of H,PO = 11.8 mmol
You add 1.7 mL of 1.00 M HCl to the buffer. Calculate the molar quantity of H,O* added as
HCl, and the final molar quantity of HPO, and H,PO,¯ at equilibrium.
a.
b. What is the new HPO/H,PO,¯ ratio, and the…
A series of carbonic acid or carbonate buffers regulate pH in blood within the human body. The kidneys and the lungs work together to help maintain a blood pH of 7.4 by affecting the components of the buffers in the blood.
What conjugate acid/base pair is the main component in the buffer? Write out the chemical reaction that the conjugate pair undergoes in water.
What is the ratio of the acid to the base?
What is the ideal pH range for this buffer?
Is the pH of blood within the ideal range of the buffer? If it is not, what is the physiological reason that the body would have for still using a carbonate buffer as opposed to another conjugate pair?
Chapter 15 Solutions
Chemistry: An Atoms-Focused Approach
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- Calculate the pH of these buffers.arrow_forwardThe titration curves for two acids with the same base are shown on this graph. (a) Which is the curve for the weaker acid? Explain your choice. (b) Give the approximate pH at the equivalence point for the titration of each acid. (c) Explain why the pH at the equivalence point differs for each acid. (d) Explain why the starting pH values of the two acids differ. (e) Which indicator or indicators, phenolphthalein, bromthymol blue, or methyl red, could be used for the titration of Acid 1? For the titration of Acid 2? Explain your choices.arrow_forwardA 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)?arrow_forward
- Without doing calculations, determine the pH of a buffer made front equimolar amounts of these acid-base pairs. (a) Nitrous acid and sodium nitrite (b) Ammonia and ammonium chloride (c) Formic acid and potassium formatearrow_forwardWhat is the effect of dilution on the pH of a buffer and the buffer’s capacity? explainarrow_forwardA chemistry graduate student is given 450. mL of a 1.70M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,= 4.9 × 10 ". What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.97? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.arrow_forward
- A student was required to prepare 250.0 mL of a cyanoacetic acid/sodium cyanoacetate buffer in which the concentration of the weak acid component was 0.06 M and the concentration of the conjugate base was 0.028 M. The student was supplied with 0.512 M cyanoacetic acid and 1.0M NaOH to perform this task. What volume (in mL) of the acid would the student need to prepare this buffer solution? Hint: assume that all of the conjugate base comes directly from the reaction of NaOH with the weak acid (in other words, there is negligible dissociation of the weak acid). Please enter answers with 2 decimal places.arrow_forwardIn a laboratory experiment, a student has 1 L of solution containing a weak base at a concentration of 0.300 M. In order to create a buffer, a strong acid is added, which converts some of the base in the solution to its conjugate weak acid to create a buffer. If the student wants to create the most effective buffer that can be equally resistant to both acids and bases how many moles of strong acid should the student add to the buffer? (Please provide your answer to 3 decimal places.)arrow_forwardA buffer is made using 100.0 mL of 0.100 M CH3 CH2 COOH (propanoic acid) and 100.0 mL of 0.100 M NACH3 CH2 COO (sodium propanoate). A) Explain in your own words what will occur (at the molecular level) when an nitric acid is added to the buffer? What would be the effect on the pH? B) Explain in your own words what will occur when LIOH is added tot he buffer? What would be the effect on the [H+]?arrow_forward
- A buffer is made using 100.0 mL of 0.100 M CH;CH,COOH (propanoic acid) and 100.0 mL of 0.100 M NaCH;CH,COO (sodium propanoate). A) Explain in your own words what will occur (at the molecular level) when an nitric acid is added to the buffer? What would be the effect on the pH? B) Explain in your own words what will occur when LIOH is added tot he buffer? What would be the effect on the [H+]?arrow_forwardExplain how a saturated solution of potassium acid tartrate can be considered to be a buffer even though it is not a solution of conjugate weak acid-weak base pair?arrow_forwardA chemistry graduate student is given 125. mL of a 1.00 M methylamine (CH ,NH,) solution. Methylamine is a weak base with K,=4.4× 10 *. What mass of CH,NH,Br should the student dissolve in the CH,NH, solution to turn it into a buffer with pH =11.05? You may assume that the volume of the solution doesn't change when the CH,NH,Br is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.arrow_forward
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