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5) Experimental Procedure, Part C.1. Will the addition of NaC₂H₂O₂ to a CH,COOH solution cause the pH to increase or decrease? Explain. See equation 16.14.

5) Experimental Procedure, Part C.1. Will the addition of NaC₂H₂O₂ to a CH,COOH solution cause the pH to increase or decrease? Explain. See equation 16.14.

Chemistry
Chemistry
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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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4. Note the dynamic equilibrium in the opening photo. Which solution changes color when the pH of both solutions is increased? Explain. anottua tek 109d 5) Experimental Procedure, Part C.1. Will the addition of NaC₂H₂O₂ to a CH₂COOH solution cause the pH to increase or decrease? Explain. See equation 16.14. G A state of dynamic equilibrium, Ag₂CO3(s) = 2Ag+ (aq) + CO2(aq), exists in solution. a. What shift, if any, occurs in the equilibrium if more Ag₂CO3(s) is added to the system? What shift, if any, occurs in the equilibrium if AgNO3(aq) is added to the system? G After water is added to the system and equilibrium is reestablished: (i) what change in the number of moles of Ag+ (aq) occurs in the system? Explain. (ii) what change in the concentration of Ag+ (aq) occurs in the system? Explain. d.) What shift occurs in the equilibrium if HCl(aq) is added to the system? Explain. 214 LeChâtelier's Principle; Buffers
Transcribed Image Text:4. Note the dynamic equilibrium in the opening photo. Which solution changes color when the pH of both solutions is increased? Explain. anottua tek 109d 5) Experimental Procedure, Part C.1. Will the addition of NaC₂H₂O₂ to a CH₂COOH solution cause the pH to increase or decrease? Explain. See equation 16.14. G A state of dynamic equilibrium, Ag₂CO3(s) = 2Ag+ (aq) + CO2(aq), exists in solution. a. What shift, if any, occurs in the equilibrium if more Ag₂CO3(s) is added to the system? What shift, if any, occurs in the equilibrium if AgNO3(aq) is added to the system? G After water is added to the system and equilibrium is reestablished: (i) what change in the number of moles of Ag+ (aq) occurs in the system? Explain. (ii) what change in the concentration of Ag+ (aq) occurs in the system? Explain. d.) What shift occurs in the equilibrium if HCl(aq) is added to the system? Explain. 214 LeChâtelier's Principle; Buffers
9 9 9 LV JFROWITE 2 NO₂ N₂O4 hanks IA allow of DH MOO Perform this experiment with a partner. At each circled superscript in the pro- cedure, stop and record your observations on the Report Sheet. Discuss your observa- tions with your lab partner and instructor. Account for the changes in appearance of the solution after each addition in terms of LeChâtelier's principle. Ask your instructor which parts of the Experimental Procedure are to be com- pleted. Prepare a hot water bath for Part E. 1. Formation of metal-ammonia ions. Place ~1 mL (<20 drops) of 0.1 M CuSO4 (or 0.1 M NiCl₂) in a small, clean test tube. Add drops of conc NH, (Caution: strong odor, do not inhale) until a color change occurs and the solution is clear (not colorless). 2. Shift of equilibrium. Add drops of 1 M HCl until the color again changes. 1. Silver carbonate equilibrium. In a 150-mm test tube (Figure 16.5) add ~½ mL (<10 drops) of 0.01 M AgNO3 to -½ mL of 0.1 M Na₂CO3 Add drops of 6 M HNO, (Caution: 6 M HNO3 reacts with the skin!) to the precipitate until evidence of a chemical change occurs. 2. Silver chloride equilibrium. To the clear solution from Part B.1, add -5 drops of 0.1 M HCI. Add drops of conc NH, (Caution! avoid breathing vapors and avoid skin contact) until evidence of a chemical change.* Reacidify the solution with 6 M HNO, (Caution!) and record your observations. What happens if excess conc NH, is again added? Try it. 3. Silver iodide equilibrium. After trying it, add drops of 0.1 M KI 4. Silver sulfide equilibrium. To the mixture from Part B.3, add drops of 0.1 M Na₂S* until evidence of chemical change has occurred. *At this point, the solution should be "clear and colorless." The No₂S solution should be freshly prepared. Figure 16.4 NO₂, a red-brown gas (left), is favored at higher temperatures; N₂O4, a colorless gas (right), is favored at lower temperatures. See equation 16.1. 13a A HOW A. Metal-Ammonia Ions B. Multiple Equilibria with the Silver Ion -0.01 M AgNO3 -6 M HNO3 -0.1 MHCI -conc NH3 -6 M HNO₂ conc NH3 0.1 MKI 0.1 M Na₂S 0.1 M Na₂CO3 Figure 16.5 Sequence of added reagents for the study of silver ion equilibria. Experiment 16 211
Transcribed Image Text:9 9 9 LV JFROWITE 2 NO₂ N₂O4 hanks IA allow of DH MOO Perform this experiment with a partner. At each circled superscript in the pro- cedure, stop and record your observations on the Report Sheet. Discuss your observa- tions with your lab partner and instructor. Account for the changes in appearance of the solution after each addition in terms of LeChâtelier's principle. Ask your instructor which parts of the Experimental Procedure are to be com- pleted. Prepare a hot water bath for Part E. 1. Formation of metal-ammonia ions. Place ~1 mL (<20 drops) of 0.1 M CuSO4 (or 0.1 M NiCl₂) in a small, clean test tube. Add drops of conc NH, (Caution: strong odor, do not inhale) until a color change occurs and the solution is clear (not colorless). 2. Shift of equilibrium. Add drops of 1 M HCl until the color again changes. 1. Silver carbonate equilibrium. In a 150-mm test tube (Figure 16.5) add ~½ mL (<10 drops) of 0.01 M AgNO3 to -½ mL of 0.1 M Na₂CO3 Add drops of 6 M HNO, (Caution: 6 M HNO3 reacts with the skin!) to the precipitate until evidence of a chemical change occurs. 2. Silver chloride equilibrium. To the clear solution from Part B.1, add -5 drops of 0.1 M HCI. Add drops of conc NH, (Caution! avoid breathing vapors and avoid skin contact) until evidence of a chemical change.* Reacidify the solution with 6 M HNO, (Caution!) and record your observations. What happens if excess conc NH, is again added? Try it. 3. Silver iodide equilibrium. After trying it, add drops of 0.1 M KI 4. Silver sulfide equilibrium. To the mixture from Part B.3, add drops of 0.1 M Na₂S* until evidence of chemical change has occurred. *At this point, the solution should be "clear and colorless." The No₂S solution should be freshly prepared. Figure 16.4 NO₂, a red-brown gas (left), is favored at higher temperatures; N₂O4, a colorless gas (right), is favored at lower temperatures. See equation 16.1. 13a A HOW A. Metal-Ammonia Ions B. Multiple Equilibria with the Silver Ion -0.01 M AgNO3 -6 M HNO3 -0.1 MHCI -conc NH3 -6 M HNO₂ conc NH3 0.1 MKI 0.1 M Na₂S 0.1 M Na₂CO3 Figure 16.5 Sequence of added reagents for the study of silver ion equilibria. Experiment 16 211
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