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xample #4) 50mL of 1.5M HCl is mixed with 60mL of 1.0M KOH

xample #4) 50mL of 1.5M HCl is mixed with 60mL of 1.0M KOH

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
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Example #4) 50mL of 1.5M HCI is mixed with 60mL of 1.0M KOH HCI + KOH → H₂O + KCI AHf in kJ/mol -286 -164 -419 -480 Note: this is the same reaction as example #3, so the AH reaction should be the same Substance H₂O HCI KCI KOH AHreaction=AHproducts- AHreactants AHreaction = -biki Let's calculate the limiting reagent to determine how many mols of water will be formed: Here's the first reactant: 50mL of 1.5M HCI 50 * 1.5. 1000 1.5 = 0.075 mol Hel Let's do this for the second reactant, 60mL of 1.0M KOH 60 1000 * 1 = 0.obmolkott Calculate the amount of energy released: Call 0.06 * -61 = -3.66 kg
Transcribed Image Text:Example #4) 50mL of 1.5M HCI is mixed with 60mL of 1.0M KOH HCI + KOH → H₂O + KCI AHf in kJ/mol -286 -164 -419 -480 Note: this is the same reaction as example #3, so the AH reaction should be the same Substance H₂O HCI KCI KOH AHreaction=AHproducts- AHreactants AHreaction = -biki Let's calculate the limiting reagent to determine how many mols of water will be formed: Here's the first reactant: 50mL of 1.5M HCI 50 * 1.5. 1000 1.5 = 0.075 mol Hel Let's do this for the second reactant, 60mL of 1.0M KOH 60 1000 * 1 = 0.obmolkott Calculate the amount of energy released: Call 0.06 * -61 = -3.66 kg
LAB NINE: Solubility Before we begin the worksheet, let's do some safety for our (hypothetical) compounds that are being "used". Hazardous Chemical Silver Nitrate Ammonium hydroxide Iron (III) chloride Copper (II) carbonate Sodium carbonate Aluminum Nitrate calcium bromide Potassium Phosphate Flammable (Flash Point) Toxic XX x Corrosive XX XX X Details of Hazard X X Eye, skin irritation Eye, skin irritation Eye, skin irritation Eye, skin irritation Eye X X x lx Oxidizing X X X Eye irritation, skin irritation Eye irritation, skin irritation Eye, skin irritation Eye irritation, skin irritation Many of the systems studied in this course involve solutions. It is therefore important that you become familiar with the qualitative and quantitative aspects of solubility and solutions. This experiment will demonstrate some of the factors affecting the solubility of a substance, changes occurring in the formation of a solution, and methods of expressing the relative amount of solute in a solution. If we mix solid AgNO3 with water, it dissolves and forms a strong electrolyte solution. Silver chloride, on the other hand, is almost completely insoluble. If we mix solid AgCl with water, virtually all of it remains as a solid within the liquid water. Whether a particular compound is soluble or insoluble depends on several factors. Predicting whether a compound will dissolve in water is not easy. The best way to do it is to conduct experiments to test whether a compound will dissolve in water, and then develop some rules based on those experimental results. We call this method the empirical method. Now, make sure to look up solubility rules either online or in your textbook, and use them to investigate the following reactions. AgNO3(aq) Soluble AgCl(s) Insoluble NO3 Ag -CI- Ag+
Transcribed Image Text:LAB NINE: Solubility Before we begin the worksheet, let's do some safety for our (hypothetical) compounds that are being "used". Hazardous Chemical Silver Nitrate Ammonium hydroxide Iron (III) chloride Copper (II) carbonate Sodium carbonate Aluminum Nitrate calcium bromide Potassium Phosphate Flammable (Flash Point) Toxic XX x Corrosive XX XX X Details of Hazard X X Eye, skin irritation Eye, skin irritation Eye, skin irritation Eye, skin irritation Eye X X x lx Oxidizing X X X Eye irritation, skin irritation Eye irritation, skin irritation Eye, skin irritation Eye irritation, skin irritation Many of the systems studied in this course involve solutions. It is therefore important that you become familiar with the qualitative and quantitative aspects of solubility and solutions. This experiment will demonstrate some of the factors affecting the solubility of a substance, changes occurring in the formation of a solution, and methods of expressing the relative amount of solute in a solution. If we mix solid AgNO3 with water, it dissolves and forms a strong electrolyte solution. Silver chloride, on the other hand, is almost completely insoluble. If we mix solid AgCl with water, virtually all of it remains as a solid within the liquid water. Whether a particular compound is soluble or insoluble depends on several factors. Predicting whether a compound will dissolve in water is not easy. The best way to do it is to conduct experiments to test whether a compound will dissolve in water, and then develop some rules based on those experimental results. We call this method the empirical method. Now, make sure to look up solubility rules either online or in your textbook, and use them to investigate the following reactions. AgNO3(aq) Soluble AgCl(s) Insoluble NO3 Ag -CI- Ag+
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