April Week 1, 2 - Reversible Reactions and Equilibrium
Learning Target: C5.3x Equilibrium, C5.3a, C5.3b, C5.3c..State Le Chatelier's principle. Apply Le Chatelier's principle to determine whether the forward or reverse reaction is favored when a stress such as concentration, temperature, or pressure is applied to an
equilibrium system. Discuss the common-ion effect in the context of Le Chatelier's principle
Read, Take Notes and Check your Understanding.
P. 497: Define reversible reaction. Give an example.
Define chemical equilibrium. Give an example.
P. 498: Explain and draw Figure 3.
P. 499. Define static equilibrium. Define dynamic equilibrium.
P. 501: Section Review: Answer questions 1,2,3,4.
P. 502: Define equilibrium constant. Summarize and understand Skills Toolkit.
P. 505: Copy Table 2 and apply your understanding of determining Keq.
P 506: Read Sample Problem B. Do practice 1, 2.
P. 511: Section Review: Answer question 1, 2, 3.
P. 521: Do number 521.
P 523: Answer question 31, 33.
P. 512: Define Le Chatelier's principle.
P. 513: How does change in concentration alter the equilibrium constant?
P. 514: How does the change in temperature affects equilibrium system?
P. 516: How does pressure changes alter systems in equilibrium?
P. 517: Define common-ion effect. Give an example.
P. 518: Give an example of a practical uses of Le Chatelier's principle.
P. 522: Do 20, 21, 22, 23, 24, 25, 26, 26, 27, 29.
P. 527: Answer Standardized Test Prep.
Learning Target: C5.3x Equilibrium, C5.3a, C5.3b, C5.3c..State Le Chatelier's principle. Apply Le Chatelier's principle to determine whether the forward or reverse reaction is favored when a stress such as concentration, temperature, or pressure is applied to an
equilibrium system. Discuss the common-ion effect in the context of Le Chatelier's principle
Read, Take Notes and Check your Understanding.
P. 497: Define reversible reaction. Give an example.
Define chemical equilibrium. Give an example.
P. 498: Explain and draw Figure 3.
P. 499. Define static equilibrium. Define dynamic equilibrium.
P. 501: Section Review: Answer questions 1,2,3,4.
P. 502: Define equilibrium constant. Summarize and understand Skills Toolkit.
P. 505: Copy Table 2 and apply your understanding of determining Keq.
P 506: Read Sample Problem B. Do practice 1, 2.
P. 511: Section Review: Answer question 1, 2, 3.
P. 521: Do number 521.
P 523: Answer question 31, 33.
P. 512: Define Le Chatelier's principle.
P. 513: How does change in concentration alter the equilibrium constant?
P. 514: How does the change in temperature affects equilibrium system?
P. 516: How does pressure changes alter systems in equilibrium?
P. 517: Define common-ion effect. Give an example.
P. 518: Give an example of a practical uses of Le Chatelier's principle.
P. 522: Do 20, 21, 22, 23, 24, 25, 26, 26, 27, 29.
P. 527: Answer Standardized Test Prep.
answers_to_section_review_pages_522-523_1.pdf | |
File Size: | 295 kb |
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answers_to_problems_page_521-522.pdf | |
File Size: | 158 kb |
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answers_to_chapter_review_page_522-_le_chatelier.pdf | |
File Size: | 396 kb |
File Type: |
answers_to_section_2_review_page_511.pdf | |
File Size: | 196 kb |
File Type: |
answers_to_practice_problems_b_in_page_506.pdf | |
File Size: | 222 kb |
File Type: |
April Week 3, 4 - Solutions
Learning Targets. 2.A.3:h Electrolytes and properties of water. 1.D.3:c, 2.A.3:i, 2.A.3:j . Molarity and preparation of solutions. 6.C.3:d Precipitation reactions and solubility rules. Solubility and the dissolving process ]
Read, Take Notes and Check your Understanding.
P 468: Define solubility,
Explain figure 8. Why is vitamin C soluble in water?
P. 469: Explain figure 9: Why is vitamin A a fat-soluble vitamin?
P. 470: Define miscible and immiscible.
Explain figure 10.
P. 471: Explain figure 11: How does the surface area speeds up the dissolving process?
P. 472: Explain figure 12. How does temperature affect the solubility of solids?
Define dissociation, hydration.
P. 473: Explain figure 13.
Explain how both enthalpy and entropy change during dissociation and hydration.
Table 2: Know some solubility rules.
P. 492: Answer questions 89-94.
P. 474: Define saturated solution.
Define unsaturated solution.
Explain figure 15.
P. 475: Define supersaturated solution.
P. 476: Define solubility equilibrium.
Explain figure 17.
Define dynamic equilibrium.
Explain figure 18 and how gases can dissolve in liquids.
P. 477: State Henry's Law.
Distinguish between non-electrolyte, weak electrolyte and strong electrolyte;
Electrical Conductivity in Solutions.
P. 478: Define conductivity.
Define electrolyte.
Explain figure 19.
P. 479: Define non-electrolyte
Explain figure 20.
P. 480: Define hydronium ion.
Explain figure 21: Write the reaction of acetic acid with water.
Why is acetic acid a weak electrolyte?
Write the reaction of hydrogen chloride with water.
Why is hydrochloric acid a strong electrolyte?
What does the term strong electrolyte mean?
Tap Water Conduct Electricity.
P. 480: Explain figure 22.
P. 481: What makes water a good conductors?
Colligative Properties
P. 481: Explain the effect of adding salt on the freezing point and boiling point of water.
Define freezing-point depression.
Define boiling-point elevation.
Only the Concentration of Dissolved Particles is Important.
P. 482: Define colligative property.
Figure 24. Compare the number of dissolved particles.
Dissolved Solutes Lower the Vapor Pressure of the Solvent
P. 483: Explain the effect of adding solute on the vapor pressure of solvent.
How does adding solute affect the freezing point and boiling point?
Figure 25: Explain the solute effects on the vapor pressure of a pure substance.
Surfactants
P. 483: Define surfactant, detergent, soap, emulsion.
Write the typical formula of the surfactant, sodium palmitate (soap).
Figure 26; Draw how soap acts as an emulsifying agent.
P. 485: Explain figure 27.
Predict what would happen if we add a detergent.
Hard Water Limits Soap's Detergent Ability.
P. 485: Explain how salts of calcium, magnesium and iron (II) in hard water form an insoluble substance (precipitate, s). Write the equation.
How can we rinse the insoluble substance?
Synthetic Detergents Outperform Soaps in Hard Water.
P. 485: Explain how synthetic detergents are better than soap in hard water.
Why is it important for a detergent to be biodegradable?
P. 486: Explain figure 28.
Draw both structures. How are they different?
Explain how the different polar ends affect the formation of a precipitate with the ions (magnesium, calcium and iron (II)) that are normally present in hard water.
Learning Targets. 2.A.3:h Electrolytes and properties of water. 1.D.3:c, 2.A.3:i, 2.A.3:j . Molarity and preparation of solutions. 6.C.3:d Precipitation reactions and solubility rules. Solubility and the dissolving process ]
Read, Take Notes and Check your Understanding.
P 468: Define solubility,
Explain figure 8. Why is vitamin C soluble in water?
P. 469: Explain figure 9: Why is vitamin A a fat-soluble vitamin?
P. 470: Define miscible and immiscible.
Explain figure 10.
P. 471: Explain figure 11: How does the surface area speeds up the dissolving process?
P. 472: Explain figure 12. How does temperature affect the solubility of solids?
Define dissociation, hydration.
P. 473: Explain figure 13.
Explain how both enthalpy and entropy change during dissociation and hydration.
Table 2: Know some solubility rules.
P. 492: Answer questions 89-94.
P. 474: Define saturated solution.
Define unsaturated solution.
Explain figure 15.
P. 475: Define supersaturated solution.
P. 476: Define solubility equilibrium.
Explain figure 17.
Define dynamic equilibrium.
Explain figure 18 and how gases can dissolve in liquids.
P. 477: State Henry's Law.
Distinguish between non-electrolyte, weak electrolyte and strong electrolyte;
Electrical Conductivity in Solutions.
P. 478: Define conductivity.
Define electrolyte.
Explain figure 19.
P. 479: Define non-electrolyte
Explain figure 20.
P. 480: Define hydronium ion.
Explain figure 21: Write the reaction of acetic acid with water.
Why is acetic acid a weak electrolyte?
Write the reaction of hydrogen chloride with water.
Why is hydrochloric acid a strong electrolyte?
What does the term strong electrolyte mean?
Tap Water Conduct Electricity.
P. 480: Explain figure 22.
P. 481: What makes water a good conductors?
Colligative Properties
P. 481: Explain the effect of adding salt on the freezing point and boiling point of water.
Define freezing-point depression.
Define boiling-point elevation.
Only the Concentration of Dissolved Particles is Important.
P. 482: Define colligative property.
Figure 24. Compare the number of dissolved particles.
Dissolved Solutes Lower the Vapor Pressure of the Solvent
P. 483: Explain the effect of adding solute on the vapor pressure of solvent.
How does adding solute affect the freezing point and boiling point?
Figure 25: Explain the solute effects on the vapor pressure of a pure substance.
Surfactants
P. 483: Define surfactant, detergent, soap, emulsion.
Write the typical formula of the surfactant, sodium palmitate (soap).
Figure 26; Draw how soap acts as an emulsifying agent.
P. 485: Explain figure 27.
Predict what would happen if we add a detergent.
Hard Water Limits Soap's Detergent Ability.
P. 485: Explain how salts of calcium, magnesium and iron (II) in hard water form an insoluble substance (precipitate, s). Write the equation.
How can we rinse the insoluble substance?
Synthetic Detergents Outperform Soaps in Hard Water.
P. 485: Explain how synthetic detergents are better than soap in hard water.
Why is it important for a detergent to be biodegradable?
P. 486: Explain figure 28.
Draw both structures. How are they different?
Explain how the different polar ends affect the formation of a precipitate with the ions (magnesium, calcium and iron (II)) that are normally present in hard water.