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8. Add 5.0 mL of 0.30 Pb(NO), to a test tube. Measure 10.0 mL of 0.30 M hydrochloric acid in a graduated cylinder.

8. Add 5.0 mL of 0.30 Pb(NO), to a test tube. Measure 10.0 mL of 0.30 M hydrochloric acid in a graduated cylinder.

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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Explain step by step Q 9 by showing me the calculation please
PART C 8. Add 5.0 mL of 0.30 Pb(NO), to a test tube. Measure 10.0 mL of 0.30 M hydrochloric acid in a graduated cylinder. 9. Pour the hydrochloric acid into a small beaker and use a disposable pipette to add it to the test tube dropwise with stirring until a white precipitate just begins to form after stirring. There should be a minimum amount of precipitate present in the test tube. Make observations of the system as you go. Record the total volume of HCI added once you have a lasting precipitate. (2.3ml) 10. Put the test tube into the hot water bath for a couple of minutes. Record your observations. 11. Cool the test tube under running cold water. Record your observations. 12. Add 1 ml. increments of deionized water to the test tube until the precipitate just dissolves. Record this volume. (6mL) PART C 6. Explain why PbC1, did not precipitate immediately upon addition of HCI. 7. Is Reaction 3 exothermic or endothermic? Explain your choice. 8. Explain why the PbC1, dissolved in water in Step 12. 9. Calculate the value of the equilibrium constant for Reaction 3. Do not forget to use the total volume when you calculate your ion concentrations. 2+ • Pbck(2)/(s) = P₂²+ + 2√√(99)
Transcribed Image Text:PART C 8. Add 5.0 mL of 0.30 Pb(NO), to a test tube. Measure 10.0 mL of 0.30 M hydrochloric acid in a graduated cylinder. 9. Pour the hydrochloric acid into a small beaker and use a disposable pipette to add it to the test tube dropwise with stirring until a white precipitate just begins to form after stirring. There should be a minimum amount of precipitate present in the test tube. Make observations of the system as you go. Record the total volume of HCI added once you have a lasting precipitate. (2.3ml) 10. Put the test tube into the hot water bath for a couple of minutes. Record your observations. 11. Cool the test tube under running cold water. Record your observations. 12. Add 1 ml. increments of deionized water to the test tube until the precipitate just dissolves. Record this volume. (6mL) PART C 6. Explain why PbC1, did not precipitate immediately upon addition of HCI. 7. Is Reaction 3 exothermic or endothermic? Explain your choice. 8. Explain why the PbC1, dissolved in water in Step 12. 9. Calculate the value of the equilibrium constant for Reaction 3. Do not forget to use the total volume when you calculate your ion concentrations. 2+ • Pbck(2)/(s) = P₂²+ + 2√√(99)
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