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  • Content from 2019 and Older

Piersa, Amanda

  • Regents Chemistry 2020
    • Unit 1: Atomic Structure
    • Unit 2a: Matter
    • Unit 2b: Energy
    • Unit 3: Periodic Table
    • Unit 4a: Writing Formulas and Naming Compounds
    • Unit 4b: Balancing Equations and Classifying Chemical Reactions
  • Prentice Hall Review Book KEYS
  • Content from 2019 and Older
    • Math and Measurement
    • Matter and Energy
    • Behavior of Gases
    • Atomic Structure
    • Nuclear Chemistry
    • Periodic Table
    • F & E and Chemical Reactions
    • The Mole- Math of Chemistry
    • Chemical Bonding
    • Solutions Chemistry
    • Acids and Bases
    • Kinetics and Equilibrium
    • Electrochemistry (Redox)
    • Organic Chemistry
  • Notes
    Solutions and Solubility Factors 2019
    Table F and Solubility 2019
    Types of Solutions and Table G 2019
    Molarity Concentration and Parts Per Million 2019 Notes
    Colligative Properties 2019 Notes
     
    Solutions Review Book Question Answers
     
    Assigned as HW on 3/28/19: Review Book p. 120 # 1-12
    1. 4.
    2. 2.
    3. 3. Potassium chloride, KCl dissociates and dissolves in water therefore both K+ and Cl- act as the solute dissolving in the water solvent.
    4. 4. Anything that is aqueous means its been dissolved in water and is ALWAYS a homogeneous mixture.
    5. 4. Water (H2O) is a bent molecule with asymmetrical charge distribution making it polar. Polar substances dissolve polar and ionic substances because like polarities are soluble (like dissolves like)
    6. 3. All components of a solution pass through a filter paper and cone because the solvent has fully dissolved the solute.
    7. 2. Metallic substances do not dissolve, ionic substances will only dissolve in polar solvents and color has no impact on dissolving. Covalent substances are the only substances that can be nonpolar.
    8. 1. As temperature increases, gas molecules move more rapidly and escape from solution, becoming less soluble.
    9. 1. Pressure only affects gases in solution.
    10. 1. The partial positive hydrogen ends of a water molecule attract to the positive sodium ion while the partial negative end of the water molecule attracts to the negative chloride ion.
    11.  2. Opposite charges attract.
    12. 3. For a gas to be most soluble and remain dissolved in a solvent it needs high pressure and low temperatures. The high pressure forces the gas into solution and the low temperature restricts gas molecule motion.
     
    Magic Sand-Polarity Activity and Answer Key Assigned as CW on 3/29/19 and 4/1/19
     
    Table G MC WS and Answer Key Assigned as HW on 4/1/19
     
    Table G Practice and Answer Key.pdf Assigned as CW on 4/2/19
     
    Molarity Concentration Activity Assigned as CW on 4/4/19 and 4/5/19
     
    Introduction to Solutions WS Answer Key Assigned as a Do Now on 4/8/19 and 4/9/19
     
    Molarity Concentration MC WS Assigned as HW on 4/8/19
    Molarity Concentration MC WS Answer Key
     
    Molarity and PPM Concentrations practice Assigned as HW on 4/9/19
     
    Colligative Properties MC WS Assigned as CW on 4/11/19
    Colligative Properties MC WS Answer Key
     
    Solutions Unit Review Packet 2019 Distributed on 4/11/19
    Solutions Unit Review Packet 2019 Answer Key
     
     
     
    ___________________________________________________________________________________________________________
     
     
    OLD MATERIALS
    Molarity Concentration, Dilutions and PPM 2018.pdf
    Colligative Properties 2018
     
    R Chem Table G Worksheets Answer keys Assigned as HW on 4/12/18

    Table F and Table G Practice Answer Keys.pdf Assigned as CW on 4/13/18

    R Chem Solutions Molarity Activity Answer Key Assigned as CW on 4/16/18-4/17/18

    R Book p 128 Q# 24-29 Molarity Conc. Answer Key Assigned as HW on 4/16/18

    Solutions Packet Questions Answer Key Assigned as HW on 4/17/18

    R Chem Colligative Properties HW Sheet 1 & R Chem R Book Colligative Prop Answer Key Assigned as HW on 4/18/18

    __________________________________________________________________________________________________________________________
    Extra Review Materials
    Introduction to Solutions
    Introduction to Solutions- Answer Key
     
    Table F MC WS and Answer Key
     
    Extra Table F and Table G Problems
    Extra Table F and Table G Problems –Answer Key
     
     Concentrations of Solutions Mixed Practice
     Concentrations of Solutions Mixed Practice- Answer Key
     
    Extra Practice for Solutions with Answers
     
    Solutions Review 1 
    Solutions Review 1- Answer Key
     
    Solutions Review 2
    Solutions Review 2- Answer Key
     
     
    OLD MATERIALS
    ___________________________________________________________________________________________________________
     Solutions Unit Worksheets and Answer Keys
     
    Magic Sand-Polarity Activity and Answer Key
    Introduction to Solutions Questions and Answer Key
     
    Table F Practice 1 and Answer Key
    Table F MC Question Set and Answer Key
     
    Table G-Solubility Curves Practice 1 and Answer Key
    Table G-Solubility Curves MC Set and Answer Key
     
    Molarity Practice 1 and Answer Key
    Molarity Practice 2 and Answer Key
    Molarity Practice 3 and Answer Key
    Concentration Formulas Practice and Answer Key 
     
    Colligative Properties Article and Answer Key 
    Colligative Properties Activity 
    Colligative Properties MC Questions and Answer Key
     
    Solutions Unit Review Packet and Answer Key
     
    Extra Review Materials
    Introduction to Solutions
    Introduction to Solutions- Answer Key
     
    Extra Table F and Table G Problems
    Extra Table F and Table G Problems –Answer Key
     
    Concentrations of Solutions Mixed Practice
    Concentrations of Solutions Mixed Practice- Answer Key
     
    Extra Practice for Solutions with Answers
     
    Solutions Review 1 
    Solutions Review 1- Answer Key
     
    Solutions Review 2
    Solutions Review 2- Answer Key
     ________________________________________________________________________________________________________
    OLD MATERIALS
     
    Solutions Worksheet Answer Keys
     
    Polar Nature of Substances Answer Key  Classwork activity on 3/21/16 and 3/22/16
     
    Introduction to Solutions Questions Answer Key  Classwork on 3/22/16
     
    Set 1- Solubility Guidelines for Aqueous Solutions Answer Key  Classwork on 3/23/16
      
     __________________________________________________________________________________________________________
    Solutions Review Book Question Answers
     
    HW 3/28/16: Review Book p. 120 # 1-12and p. 123 #13-23
    1. 4.
    2. 2.
    3. 3. Potassium chloride, KCl dissociates and dissolves in water therefore both K+ and Cl- act as the solute dissolving in the water solvent.
    4. 4. Anything that is aqueous means its been dissolved in water and is ALWAYS a homogeneous mixture.
    5. 4. Water (H2O) is a bent molecule with asymmetrical charge distribution making it polar. Polar substances dissolve polar and ionic substances because like polarities are soluble (like dissolves like)
    6. 3. All components of a solution pass through a filter paper and cone because the solvent has fully dissolved the solute.
    7. 2. Metallic substances do not dissolve, ionic substances will only dissolve in polar solvents and color has no impact on dissolving. Covalent substances are the only substances that can be nonpolar.
    8. 1. As temperature increases, gas molecules move more rapidly and escape from solution, becoming less soluble.
    9. 1. Pressure only affects gases in solution.
    10. 1. The partial positive hydrogen ends of a water molecule attract to the positive sodium ion while the partial negative end of the water molecule attracts to the negative chloride ion.
    11.  2. Opposite charges attract.
    12. 3. For a gas to be most soluble and remain dissolved in a solvent it needs high pressure and low temperatures. The high pressure forces the gas into solution and the low temperature restricts gas molecule motion.
    13. 2. Use Table G. The solubility of a gas will decrease as temperature increases because the particles have more KE and escape the solvent more easily.
    14. 4. The solubility of a solid solute in solution increases as temperature increases.
    15. 3. According to Table G, 39 g of KCl must be dissolved in 100 g of water to make a saturated solution. An additional 25 g must be added to the 14 g of solute already dissolved.
    16. 1. Table G
    17. 1. The lowest amount of solute dissolves for this salt at 50°C when compared to the other salts.
    18. 4. The solubility of KNO3 increases as temperature increases according to Table G. Trial 4 should be higher than 70 g not lower.
    19. 4. According to table G, 45 g of KCl dissolves in 100 g of water to make a saturated solution at 60°C, therefore 90 g will dissolve in 200 g of water.
    20. 3. Barium sulfate (BaSO4) is insoluble because Ba+2 is an exception to sulfate forming soluble compounds.
    21. 2. Lead (II) iodide (PbCl2) is insoluble because any halide when paired with a Pb+2 ion will be insoluble.
    22. 1. All compounds present, both the reactants and products after the double replacement reaction are soluble in water because of the presence of a group 1 ion. All ions are present in solution because everything is soluble in water. (Na2CrO4 + K2CO3 --> K2CrO4 + Na2CO3) 
    23. 2. 40 g of KNO3 at 25°C produces a saturated solution. The solute amount is on the solubility curve for KNO3 at this temperature)
     ______________________________________________________________________________________________________________
     
     HW 3/29/16: Review Book p. 132-134 # 1-20, 31, 36, 37
    1. 2.
    2. 1.
    3. 2.
    4. 2. Substances with covalent bonding can be nonpolar. Ionic substances are NEVER nonpolar because oppositely charged ions are present. Metallic substances will not dissolve in solvents. Their free moving electrons makes them constantly polar.
    5. 2.
    6. 3. The more particles dissolved in a water, the higher the BP and the lower the FP will be.
    7. 1. Table G
    8. 2. Supersaturated solutions are unstable and any disturbance will cause the entire solute to crystallize.
    9. 3. Gases are most soluble at high pressure because it forces the molecules into solution and low temperatures because the molecules move less and less likely to escape the solvent.
    10. 2. Lower temperatures means less molecule movement so the molecules stay in solution more readily (higher solubility)
    11. 1. Lower temperature means less molecular motion and less ability for a liquid to escape as a gas to create vapor pressure.
    12. 1. BP elevation and FP depression with the addition of solute to water.
    13. 2. Table G.
    14. 4.
    15. 3.
    16. 3.
    17. 3.
    18. 3.
    19. 2.
    20. 3.
    31. Answer= 285.46 g. 74.54 grams dissolved in 1000 g (1 L) of water is unsaturated. According to Table G, 36 g saturated 100 g of water, so 360 grams are needed to saturate 1000 g of water. To be saturated an additional 285.46 g of solute must be added to the 1000 g of water.
    36. The solution the scientist made is unsaturated (44 g of HCl in 200 g of water). According to Table G, 72 g saturates 100 g of water so 144 g of HCl are needed to saturate 200 g of water.
    37. The particles are evenly distributed in the solution making it a homogeneous mixture.
     
    __________________________________________________________________________________________________________
    HW on 4/8/16 Review Book p. 129 #38-43, p. 133 #23, 29
     
    38. 1. NaCl contains an ionic bond and the presence of solute in solution lowers freezing point and increases boiling point.
    39. 3. Salt dissociates in solution so the number of ions increases and any particles lower the freezing point and increase the boiling point of a substance.
    40. 4. NaOH is the only substance that dissociates into ions and will yield twice the amount of particles as the other substances resulting in the lowest freezing point. The more particles in solution, the lower the freezing point.
    41. 2. 
    42. 4. This solution has the higher of the two concentrations and yields more ions in solution.
    43. 1. CH3OH is an organic alcohol with covalent bonds and will not dissociate in solution therefore it WILL NOT CONDUCT because no mobile ions are present.
    23. 1.
    29. Solution C. It yields the most ions in solution. B and D will not dissociate and A only dissociates into 2 ions while Ba(OH)2 yields 3 ions in solution.
     
     ____________________________________________________________________________________________________________
     
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