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5. Circle all of the following solutions that are buffered solutions. Justify your answer. (Ka (HC,H,O,) = 1.8 x 105; K,(NH,)= 1.8 x 105) a. 0.333 mol HC₂H₂O₂ and 0.111 mol KC₂H₂O₂ in 1.00 L solution b. 0.175 mol NaOH and 0.250 mol NH4Cl in 1.00 L solution c. 0.300 mol NaC₂H₂O₂ and 0.225 mol HCl in 1.00 L solution d. 0.200 mol HC₂H₂O, and 0.200 mol KOH in

5. Circle all of the following solutions that are buffered solutions. Justify your answer. (Ka (HC,H,O,) = 1.8 x 105; K,(NH,)= 1.8 x 105) a. 0.333 mol HC₂H₂O₂ and 0.111 mol KC₂H₂O₂ in 1.00 L solution b. 0.175 mol NaOH and 0.250 mol NH4Cl in 1.00 L solution c. 0.300 mol NaC₂H₂O₂ and 0.225 mol HCl in 1.00 L solution d. 0.200 mol HC₂H₂O, and 0.200 mol KOH in

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases
Section16.10: The Lewis Concept Of Acids And Bases
Problem 2.5ACP: To measure the relative strengths of bases stronger than OH, it is necessary to choose a solvent...
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Solutions to question 5 please
1. Identify the Lewis acid and the Lewis base in the following reaction: Agt(aq) + 2NH₂ (aq) à Ag(NH3)₂+(aq) 2. Identify the stronger acid of the following pairs of acids. Justify your answer from theory. a. HC1O,(aq) vs. HC1O,(aq) b. HClO,(aq) vs. HIO,(aq) 3. Identify the stronger Brønsted-Lowry base of the following pairs of bases. Justify your answer from theory. a. HS (aq) vs. HO (aq) b. NH₂ vs. F- 4. Calculate the pH of a mixture that contains both 0.255 mol HC₂H3O₂ and 0.165 mol NaC₂H₂O₂ in 1.00 L solution both before and after adding 0.035 mol HCl to the mixture (assume no volume change upon adding these moles of HCl) (Ka (HC₂H₂O₂) = 1.8 x 10-5)? 5. Circle all of the following solutions that are buffered solutions. Justify your answer. (Ka (HC,H,O,) = 1.8 x 10; K,(NH,)= 1.8 x 105) a. 0.333 mol HC₂H₂O₂ and 0.111 mol KC₂H₂O₂ in 1.00 L solution b. 0.175 mol NaOH and 0.250 mol NH₂Cl in 1.00 L solution c. 0.300 mol NaC₂H₂O₂ and 0.225 mol HCl in 1.00 L solution d. 0.200 mol HC₂H₂O2 and 0.200 mol KOH in 1.00 L solution 6. Calculate the number of moles of NaOH that must be added to 1.0 L of 0.50 M HC₂H3O₂ to produce a solution buffered at pH=4.00. Assume no volume change upon adding the NaOH. (K₂ (HC₂H₂O₂) = 1.8 x 10-5)
Transcribed Image Text:1. Identify the Lewis acid and the Lewis base in the following reaction: Agt(aq) + 2NH₂ (aq) à Ag(NH3)₂+(aq) 2. Identify the stronger acid of the following pairs of acids. Justify your answer from theory. a. HC1O,(aq) vs. HC1O,(aq) b. HClO,(aq) vs. HIO,(aq) 3. Identify the stronger Brønsted-Lowry base of the following pairs of bases. Justify your answer from theory. a. HS (aq) vs. HO (aq) b. NH₂ vs. F- 4. Calculate the pH of a mixture that contains both 0.255 mol HC₂H3O₂ and 0.165 mol NaC₂H₂O₂ in 1.00 L solution both before and after adding 0.035 mol HCl to the mixture (assume no volume change upon adding these moles of HCl) (Ka (HC₂H₂O₂) = 1.8 x 10-5)? 5. Circle all of the following solutions that are buffered solutions. Justify your answer. (Ka (HC,H,O,) = 1.8 x 10; K,(NH,)= 1.8 x 105) a. 0.333 mol HC₂H₂O₂ and 0.111 mol KC₂H₂O₂ in 1.00 L solution b. 0.175 mol NaOH and 0.250 mol NH₂Cl in 1.00 L solution c. 0.300 mol NaC₂H₂O₂ and 0.225 mol HCl in 1.00 L solution d. 0.200 mol HC₂H₂O2 and 0.200 mol KOH in 1.00 L solution 6. Calculate the number of moles of NaOH that must be added to 1.0 L of 0.50 M HC₂H3O₂ to produce a solution buffered at pH=4.00. Assume no volume change upon adding the NaOH. (K₂ (HC₂H₂O₂) = 1.8 x 10-5)
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