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AASonic We have a buffer when we have a mixture of HA and A. Consider a buffer with equal amounts of Acetic Acid (pKa 4.76) and Acetate (For example, 25.0 mls of 0.100 M HAc and 25.0 mls of 0.100 M Ac-). What is the pH of this buffer? Let's calculate the pH change upon addition of 5.00 mls of 0.100 M HCl. Uslng our reaction from part 3, fill in the initial moles of each species, then use stoichiometry to calculate change and final. 5) НА H + A> Initial Change Final Calculate the pH An alternate way to make a buffer is to mix a strong base with a weak acid. Let's look at how 6) this works. Consider a solution of 25.0 mls of 0.200 M Acetic Acid. Add to it 25.0 mLs of 0.100 M NaOH. Using our reaction from part 2, fill in initial moles of each species. Use stoichiometry to calculate change/final. Compare the final moles and concentrations to the initial buffer in part 5 A +H20 ОН + HA Initial Change Final Calculate the pH and the % of dissociation for your assigned solution(s) of acetic acid and add point(s) to table on board and to grapbs (on back). initial [HA] [H*] % Dissociation 1.00 M 0.75 M 0.50 M 0.25 M .00131 2.88 1.3 0.10 M 0.050 M 0.010 M

AASonic We have a buffer when we have a mixture of HA and A. Consider a buffer with equal amounts of Acetic Acid (pKa 4.76) and Acetate (For example, 25.0 mls of 0.100 M HAc and 25.0 mls of 0.100 M Ac-). What is the pH of this buffer? Let's calculate the pH change upon addition of 5.00 mls of 0.100 M HCl. Uslng our reaction from part 3, fill in the initial moles of each species, then use stoichiometry to calculate change and final. 5) НА H + A> Initial Change Final Calculate the pH An alternate way to make a buffer is to mix a strong base with a weak acid. Let's look at how 6) this works. Consider a solution of 25.0 mls of 0.200 M Acetic Acid. Add to it 25.0 mLs of 0.100 M NaOH. Using our reaction from part 2, fill in initial moles of each species. Use stoichiometry to calculate change/final. Compare the final moles and concentrations to the initial buffer in part 5 A +H20 ОН + HA Initial Change Final Calculate the pH and the % of dissociation for your assigned solution(s) of acetic acid and add point(s) to table on board and to grapbs (on back). initial [HA] [H*] % Dissociation 1.00 M 0.75 M 0.50 M 0.25 M .00131 2.88 1.3 0.10 M 0.050 M 0.010 M

Chemistry
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
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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can you give me the example for initial HA: 1.00M in table?

AASonic We have a buffer when we have a mixture of HA and A. Consider a buffer with equal amounts of Acetic Acid (pKa 4.76) and Acetate (For example, 25.0 mls of 0.100 M HAc and 25.0 mls of 0.100 M Ac-). What is the pH of this buffer? Let's calculate the pH change upon addition of 5.00 mls of 0.100 M HCl. Uslng our reaction from part 3, fill in the initial moles of each species, then use stoichiometry to calculate change and final. 5) НА H + A> Initial Change Final Calculate the pH An alternate way to make a buffer is to mix a strong base with a weak acid. Let's look at how 6) this works. Consider a solution of 25.0 mls of 0.200 M Acetic Acid. Add to it 25.0 mLs of 0.100 M NaOH. Using our reaction from part 2, fill in initial moles of each species. Use stoichiometry to calculate change/final. Compare the final moles and concentrations to the initial buffer in part 5 A +H20 ОН + HA Initial Change Final
Transcribed Image Text:AASonic We have a buffer when we have a mixture of HA and A. Consider a buffer with equal amounts of Acetic Acid (pKa 4.76) and Acetate (For example, 25.0 mls of 0.100 M HAc and 25.0 mls of 0.100 M Ac-). What is the pH of this buffer? Let's calculate the pH change upon addition of 5.00 mls of 0.100 M HCl. Uslng our reaction from part 3, fill in the initial moles of each species, then use stoichiometry to calculate change and final. 5) НА H + A> Initial Change Final Calculate the pH An alternate way to make a buffer is to mix a strong base with a weak acid. Let's look at how 6) this works. Consider a solution of 25.0 mls of 0.200 M Acetic Acid. Add to it 25.0 mLs of 0.100 M NaOH. Using our reaction from part 2, fill in initial moles of each species. Use stoichiometry to calculate change/final. Compare the final moles and concentrations to the initial buffer in part 5 A +H20 ОН + HA Initial Change Final
Calculate the pH and the % of dissociation for your assigned solution(s) of acetic acid and add point(s) to table on board and to grapbs (on back). initial [HA] [H*] % Dissociation 1.00 M 0.75 M 0.50 M 0.25 M .00131 2.88 1.3 0.10 M 0.050 M 0.010 M
Transcribed Image Text:Calculate the pH and the % of dissociation for your assigned solution(s) of acetic acid and add point(s) to table on board and to grapbs (on back). initial [HA] [H*] % Dissociation 1.00 M 0.75 M 0.50 M 0.25 M .00131 2.88 1.3 0.10 M 0.050 M 0.010 M
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