Consider the generic dissociation equation... HA + H20 H3O* + A° .where HA is a weak acid Based on what you know about buffers, explain in detail how this reaction acts as an acid buffer to keep the pH of the solution constant even when a strong acid is added to the solution. Your answer should refer to the reaction above to discuss buffers, how they work, why strong acids/bases cannot be used as buffers, and how Le Chatelier's principle impacts why buffers work.

Consider the generic dissociation equation... HA + H20 H3O* + A° .where HA is a weak acid Based on what you know about buffers, explain in detail how this reaction acts as an acid buffer to keep the pH of the solution constant even when a strong acid is added to the solution. Your answer should refer to the reaction above to discuss buffers, how they work, why strong acids/bases cannot be used as buffers, and how Le Chatelier's principle impacts why buffers work.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 8ALQ: You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major...

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You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
A 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)?
A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric acid. Assume no volume change after NaF is added. Calculate the pH of this 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.
Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from one another. Explain the chemistry involved in the various steps of the figure.
Consider exactly one litre of a propanoic acid buffer solution, containing 0.600 M C3H5OOH and 0.252 M C3H5OO- . 1.1 Determine the pH of the buffer solution. - You may use “HA” to denote the formula of the acid. - You may make certain assumptions to simplify your calculations - Ka for hydrofluoric acid is 1.3 × 10−5 . 3.2 Determine by means of a full calculation the change in pH of the buffer solution that will result when 100. mL of a 1.00 × 10−2 M HCℓ solution is added to it. You must indicate all the relevant reaction equations in your working.
A 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.
You want to prepare 1.00 L of a buffer solution with a pH of 3.5. You are given an 0.45 M solution of nitrous acid, HNO2, and an 0.68 M solution of NaOH. What volume of each of these solutions must be mixed in order to get the desired buffer solution? Use the simultaneous equations method to solve this problem. If the buffer solution prepared in a. also contained ~10-6M Ni2+ and ~10-6 M Pb2+ , could those metal ions be separated from each other by saturating the solution with H2S? Explain your answer by showing the necessary calculations.
1. You are taking samples at a contaminated mine site from a carbonate aquifer to determine the concentration of dissolved lead in the sample. To preserve the sample, you acidify it to pH 5. How much HCl, in equivalents/L, must be added to this sample to make it pH 5 if the total carbonate concentration is 102 M and the initial pH is 10? Note that the total carbonate is the sum of all of the carbonate species ([H2CO3]+[HCO3] + [CO2]) present in the sample. What are the acid-base pairs responsible for buffering in this sample?
weak acid = sodium bisulfate monohydrate, ?a=1.20×10−2,Ka=1.20×10−2, 3.00 M conjugate base= sodium sulfate decahydrate, Na2SO4⋅10H2O The final volume of buffer solution must be 100.00 mL and the final concentration of the weak acid must be 0.100 M. 1.) Based on this information, what mass of solid conjugate base should the student weigh out to make the buffer solution with a pH of 1.00? mass= 2.)Based on this information, what volume of acid should the student measure to make the buffer solution? volume=
A buffer system works to keep pH within a narrow range. Buffer systemsare critical in all living cells/tissues. If pH were to measurably shift in a cell,what category of biological molecules would be most impacted, andwhat term refers to the resulting loss of their functional shapes? A buffer is a substance that, when it ionizes in water, creates a buffersystem. The substance and one of its ions represent a weak acid and aweak base. These form a pH-controlled equilibrium. Based on thedefinitions of acid and base, if [H+] increases, which would combine withthe H+, preventing a pH shift? If [H+] decreases, whichwould release H+ to counter a pH change? Check the one characteristic below that is important in a buffer system. maintains a neutral pH prevents pH from dropping prevents pH from rising minimizes change in p
What are buffers in terms of acid-base equilibria, give an example, and can abuffer capacity be overwhelmed?