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.5 moles x 111g/mole = 55.5 g 2.0 x .250 = .5 moles %3D # 5-8 : Calculate the number of moles and the number of gram of each solution : 6.500 ml Of 2.0M KNO3 5. 1.0 L of .50M NaCl 8. 2.0 L of .30M Na2SO4 7. 250 ml of 0.1M CaCl2 9. What is the volume (in liters) ofa .20M solution that contains .30 moles of Na2SO4 dissolved in it ? Making Dilutions: Chemists often use more concentrated solutions to make more dilute solutions. The number of moles of solute does not change when a soultion is diluted. Number of moles before dilution = Number of moles after dilution Since moles Molarity (M) x liters ( V), then : M1 x V1 M2 x V2 %D Example : How would you prepare 100 ml of .4OM MGSO4 form a solution of 2.0 M MgSO4 ? M2 = .40M V2 = 100 ml %3D %3D 2.0 x V1 = .40 x 100 Vi = .40 x 100 = 20 ml %3D %3D 2.0 So, you would measure out 20 ml of the original solution, then add enough water to it to bring the volume to 100 ml. Important: You can do these dilution problems in either ml or liters, but the Vị and V2 must both be in the same units ( either both ml or both liters; don't mix them up ). Calculate the volumes you must dilute to make : 10. 500 ml of .50 M NaCl from 2.0 M original stock solution. 11. 2.0 L of .20M MgSO4 from .50 M stock solution. 12. 50 ml of .2M KNO3 from 4.0 M stock solution.

.5 moles x 111g/mole = 55.5 g 2.0 x .250 = .5 moles %3D # 5-8 : Calculate the number of moles and the number of gram of each solution : 6.500 ml Of 2.0M KNO3 5. 1.0 L of .50M NaCl 8. 2.0 L of .30M Na2SO4 7. 250 ml of 0.1M CaCl2 9. What is the volume (in liters) ofa .20M solution that contains .30 moles of Na2SO4 dissolved in it ? Making Dilutions: Chemists often use more concentrated solutions to make more dilute solutions. The number of moles of solute does not change when a soultion is diluted. Number of moles before dilution = Number of moles after dilution Since moles Molarity (M) x liters ( V), then : M1 x V1 M2 x V2 %D Example : How would you prepare 100 ml of .4OM MGSO4 form a solution of 2.0 M MgSO4 ? M2 = .40M V2 = 100 ml %3D %3D 2.0 x V1 = .40 x 100 Vi = .40 x 100 = 20 ml %3D %3D 2.0 So, you would measure out 20 ml of the original solution, then add enough water to it to bring the volume to 100 ml. Important: You can do these dilution problems in either ml or liters, but the Vị and V2 must both be in the same units ( either both ml or both liters; don't mix them up ). Calculate the volumes you must dilute to make : 10. 500 ml of .50 M NaCl from 2.0 M original stock solution. 11. 2.0 L of .20M MgSO4 from .50 M stock solution. 12. 50 ml of .2M KNO3 from 4.0 M stock solution.

General Chemistry - Standalone book (MindTap Course List)
General Chemistry - Standalone book (MindTap Course List)
11th Edition
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Chapter12: Solutions
Section: Chapter Questions
Problem 12.119QP
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.5 moles x 111g/mole = 55.5 g 2.0 x .250 = .5 moles %3D # 5-8 : Calculate the number of moles and the number of gram of each solution : 6.500 ml Of 2.0M KNO3 5. 1.0 L of .50M NaCl 8. 2.0 L of .30M Na2SO4 7. 250 ml of 0.1M CaCl2 9. What is the volume (in liters) ofa .20M solution that contains .30 moles of Na2SO4 dissolved in it ? Making Dilutions: Chemists often use more concentrated solutions to make more dilute solutions. The number of moles of solute does not change when a soultion is diluted. Number of moles before dilution = Number of moles after dilution Since moles Molarity (M) x liters ( V), then : M1 x V1 M2 x V2 %D Example : How would you prepare 100 ml of .4OM MGSO4 form a solution of 2.0 M MgSO4 ? M2 = .40M V2 = 100 ml %3D %3D 2.0 x V1 = .40 x 100 Vi = .40 x 100 = 20 ml %3D %3D 2.0 So, you would measure out 20 ml of the original solution, then add enough water to it to bring the volume to 100 ml. Important: You can do these dilution problems in either ml or liters, but the Vị and V2 must both be in the same units ( either both ml or both liters; don't mix them up ). Calculate the volumes you must dilute to make : 10. 500 ml of .50 M NaCl from 2.0 M original stock solution. 11. 2.0 L of .20M MgSO4 from .50 M stock solution. 12. 50 ml of .2M KNO3 from 4.0 M stock solution.
Transcribed Image Text:.5 moles x 111g/mole = 55.5 g 2.0 x .250 = .5 moles %3D # 5-8 : Calculate the number of moles and the number of gram of each solution : 6.500 ml Of 2.0M KNO3 5. 1.0 L of .50M NaCl 8. 2.0 L of .30M Na2SO4 7. 250 ml of 0.1M CaCl2 9. What is the volume (in liters) ofa .20M solution that contains .30 moles of Na2SO4 dissolved in it ? Making Dilutions: Chemists often use more concentrated solutions to make more dilute solutions. The number of moles of solute does not change when a soultion is diluted. Number of moles before dilution = Number of moles after dilution Since moles Molarity (M) x liters ( V), then : M1 x V1 M2 x V2 %D Example : How would you prepare 100 ml of .4OM MGSO4 form a solution of 2.0 M MgSO4 ? M2 = .40M V2 = 100 ml %3D %3D 2.0 x V1 = .40 x 100 Vi = .40 x 100 = 20 ml %3D %3D 2.0 So, you would measure out 20 ml of the original solution, then add enough water to it to bring the volume to 100 ml. Important: You can do these dilution problems in either ml or liters, but the Vị and V2 must both be in the same units ( either both ml or both liters; don't mix them up ). Calculate the volumes you must dilute to make : 10. 500 ml of .50 M NaCl from 2.0 M original stock solution. 11. 2.0 L of .20M MgSO4 from .50 M stock solution. 12. 50 ml of .2M KNO3 from 4.0 M stock solution.
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