Chapter 16 review
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This document provides a review of key concepts from Chapter 16, including solubility, supersaturated solutions, colligative properties, factors that affect solubility, and calculations involving molarity, molality, mass percent, and volume percent in solution concentration problems. It contains multiple choice and open response questions about these topics.
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The document summarizes key concepts about solutions from chapters 11-13, including:
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- Solubility is affected by intermolecular forces - "like dissolves like" with polar substances dissolving in polar solvents.
- Temperature and pressure can impact solubility, with solubility generally increasing with temperature and gas solubility directly proportional to pressure.
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The document discusses colligative properties of solutions, including vapor pressure lowering, boiling point elevation, and freezing point depression. It explains that these properties depend on the number of dissolved particles in solution, regardless of particle type. Specifically, it states that the decrease in vapor pressure and increase in boiling point or freezing point depression is proportional to the number of particles formed by the solute in solution.
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Colligative properties are physical properties of solutions that depend on the number of solute particles in the solvent rather than the type of particle. They include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. Vapor pressure lowering is used in freeze drying and calibrating humidity meters. Boiling point elevation allows cooking with salt water and sugar boiling. Freezing point depression allows using salt for melting ice and antifreeze. Osmotic pressure is important in plant cell structure and function, sweating, and water purification through reverse osmosis.
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This document discusses colligative properties of solutions, specifically molality and mole fraction. Molality is defined as the number of moles of solute per kg of solvent. Mole fraction is the ratio of moles of solute or solvent to the total moles of solution. Several examples are provided to demonstrate how to calculate molality and mole fraction for different solutions. Practice problems are also included at the end to help reinforce understanding of these concepts.
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Colligative properties depend on the concentration of solute particles but not their identity. The four main colligative properties are vapor pressure lowering, freezing point depression, boiling point elevation, and osmotic pressure. Freezing point depression and boiling point elevation are directly proportional to the molal concentration of the solution. Electrolytes enhance colligative properties because they dissociate into multiple ions in solution, effectively increasing the number of solute particles compared to nonelectrolytes of the same molar concentration.
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Colligative properties such as boiling point elevation, freezing point depression, and osmotic pressure depend only on the number of solute particles in solution, not their identity. The document discusses these properties and how they are affected when solutes dissolve. It explains that boiling point is elevated and freezing point is depressed because solutes lower vapor pressure, requiring more energy for phase changes. Osmotic pressure arises from differences in solute concentration across a semipermeable membrane. The van't Hoff factor accounts for changes in observed properties when solutes dissociate or associate in solution.
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The document discusses key concepts about solutions including:
1) Solutions are homogeneous mixtures of two or more substances where the solute is dispersed uniformly throughout the solvent.
2) For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome interactions between pure components.
3) The enthalpy change of dissolving depends on the energy changes of separating solute and solvent particles and forming new interactions between them.
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The document summarizes key concepts about solutions from chapters 11-13, including:
- Solutions are homogeneous mixtures of two or more substances where the solute is uniformly dispersed in the solvent.
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The document discusses colligative properties of solutions, including vapor pressure lowering, boiling point elevation, and freezing point depression. It explains that these properties depend on the number of dissolved particles in solution, regardless of particle type. Specifically, it states that the decrease in vapor pressure and increase in boiling point or freezing point depression is proportional to the number of particles formed by the solute in solution.
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Colligative properties are physical properties of solutions that depend on the number of solute particles in the solvent rather than the type of particle. They include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. Vapor pressure lowering is used in freeze drying and calibrating humidity meters. Boiling point elevation allows cooking with salt water and sugar boiling. Freezing point depression allows using salt for melting ice and antifreeze. Osmotic pressure is important in plant cell structure and function, sweating, and water purification through reverse osmosis.
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This document discusses colligative properties of solutions, specifically molality and mole fraction. Molality is defined as the number of moles of solute per kg of solvent. Mole fraction is the ratio of moles of solute or solvent to the total moles of solution. Several examples are provided to demonstrate how to calculate molality and mole fraction for different solutions. Practice problems are also included at the end to help reinforce understanding of these concepts.
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Colligative properties depend on the concentration of solute particles but not their identity. The four main colligative properties are vapor pressure lowering, freezing point depression, boiling point elevation, and osmotic pressure. Freezing point depression and boiling point elevation are directly proportional to the molal concentration of the solution. Electrolytes enhance colligative properties because they dissociate into multiple ions in solution, effectively increasing the number of solute particles compared to nonelectrolytes of the same molar concentration.
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Colligative properties such as boiling point elevation, freezing point depression, and osmotic pressure depend only on the number of solute particles in solution, not their identity. The document discusses these properties and how they are affected when solutes dissolve. It explains that boiling point is elevated and freezing point is depressed because solutes lower vapor pressure, requiring more energy for phase changes. Osmotic pressure arises from differences in solute concentration across a semipermeable membrane. The van't Hoff factor accounts for changes in observed properties when solutes dissociate or associate in solution.
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The document discusses key concepts about solutions including:
1) Solutions are homogeneous mixtures of two or more substances where the solute is dispersed uniformly throughout the solvent.
2) For a solution to form, the intermolecular forces between solute and solvent particles must be strong enough to overcome interactions between pure components.
3) The enthalpy change of dissolving depends on the energy changes of separating solute and solvent particles and forming new interactions between them.
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3. A saturated solution is one in equilibrium with undissolved solute where dissolution and crystallization occur at equal rates. Unsaturated and supersaturated solutions contain less or more solute respectively.
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Soluion and colligative propertries 2017
it is based on CBSE, ICSE, HSC ,JEE, NEET, AIPMT, MTCET.
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for buy ppt pay by paytm acount- 8879919898. price-Rs99 only/-
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1. Henry's law relates the pressure of a gas in a solution to its solubility. It has applications.
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The document provides an overview of colligative properties of solutions, which are physical properties that depend on the number of solute particles in solution rather than the chemical identity of the solute. Examples of colligative properties discussed include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. Formulas are provided to calculate these colligative properties based on variables like molality, vapor pressure of the pure solvent, and temperature.
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1. A solution is a homogeneous mixture of one or more solutes dissolved in a solvent. Solubility refers to the ability of a solute to dissolve in a solvent.
2. Henry's law states that the amount of gas that dissolves in a liquid is directly proportional to the partial pressure of the gas above the liquid at a constant temperature.
3. Colligative properties depend on the number of solute particles in solution, not their identity, and include vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
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Colligative properties depend only on the number of dissolved particles in solution and not on their identity. The key colligative properties are vapor pressure lowering, boiling point elevation, and freezing point depression. Vapor pressure lowering occurs because solute particles decrease the number of solvent particles that can evaporate from the surface. Boiling point elevation and freezing point depression occur because adding solute particles lowers the vapor pressure of the solvent, requiring more energy for evaporation or freezing. The degree of change in boiling point or freezing point depends on the molality of the solution.
Soluion and colligative propertries 2017
it is based on CBSE, ICSE, HSC ,JEE, NEET, AIPMT, MTCET.
class 12 chemistry.
for buy ppt pay by paytm acount- 8879919898. price-Rs99 only/-
for more detail go my site
www.akchem.blogspot.com
Nyb F09 Unit 2 Slides 1 25
The document discusses colligative properties of solutions, which depend only on the number of solute particles and not their type. It describes how adding solute particles lowers vapor pressure and freezing point and raises boiling point of the solvent. Specifically, it provides equations to calculate boiling point elevation, freezing point depression, and osmotic pressure based on molality and van't Hoff factor of the solution.
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kelter_ch11
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Çözelti Hazırlama
A 0.12 M solution of CuCl can be prepared by diluting a 0.29 M CuCl solution. The key steps are:
1) The original solution is 10 mL of 0.29 M CuCl. This contains 0.29 moles/L x 0.01 L = 0.0029 moles of CuCl.
2) The final solution volume is not specified, but the moles of CuCl must remain 0.0029 moles.
3) Using the dilution equation, the final volume can be calculated as 0.0029 moles / 0.12 M = 0.024 L or 24 mL.
4) Add water to the original 10 mL solution to
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Chapter 16 review
- 1. Chapter 16 Review =“Solutions ” Pre-AP Chemistry Charles Page High School Stephen L. Cotton
- 2. Chapter 16 Review If the solubility of a particular solute is 10 g/100 g H2O at 20 oC, which of the following would represent a supersaturated solution of that solute: a) 9 g/100 g H2O at 20 oC, or b) 11 g/100 g H2O at 20 oC. If a crystal added to an aqueous solution causes many particles to come out of the solution, the original solution was ____.
- 3. Chapter 16 Review Colligative properties depend upon the ____. What happens to the solubility of a gas in a liquid, if the partial pressure of the gas above the liquid decreases? Which of the following substances is less soluble in hot water than in cold water: a) CO2(g), or b) KBr(s)?
- 4. Chapter 16 Review The solubility of a gas in a liquid is ____ proportional to ____. To what concentration variable is change in boiling point directly proportional? What usually occurs to solubility as temperature increases? What units are generally used to express solubility?
- 5. Chapter 16 Review What factors will usually make a substance dissolve faster in a solvent? In a concentrated solution, there is a ____ amount of solute. What are the three colligative properties of a solution we have studied?
- 6. Chapter 16 Review What are the solution concentration units used to express molarity? What is the maximum amount of KCl that can dissolve in 200 g of water at 20 oC? (the solubility of KCl is 34 g/100 g H2O at 20 oC) What does NOT change when a solution is diluted by the addition of more solvent?
- 7. Chapter 16 Review Ifthe percent by volume is 2.0 % and the volume of solution is 250 mL, what is the volume of solute in solution? What two factors affect the solubility of a particular substance? Which of the following equations yields the number of moles? a) M x L, or b) M x mass of solution
- 8. Chapter 16 Review The volume of alcohol present in 620 mL of a 40.0 % (v/v) solution of alcohol is ____. A solute depresses the freezing point because the solute ____. To increase the solubility of gas at constant temperature from 1.20 g/L at 1.4 atm, to 2.3 g/L, the pressure would have to be increased to ____.
- 9. Chapter 16 Review What is the boiling point of a solution that contains 3 moles of KBr in 2000 g of water? (Kb = 0.512 oC/m; molar mass of water = 18 g/mol) What mass of KCl (solubility 34 g/100 g H2O at 20 oC) can dissolve in 3.30 x 102 g of water?
- 10. Chapter 16 Review What is the freezing point of a solution that has 5.0 mol of NaI in 1250 g of water? (Kf = 1.86 oC/m; molar mass of water = 18.0 g/mol) How many kilograms of solvent are in a sample of 0.30 molal solution, if the sample contains 13 moles of solute?
- 11. Chapter 16 Review What is the molality of a solution containing 5.0 mol of solute in 3.2 kg of solvent? What is the molarity of a solution containing 1.2 g of solute in 450 mL of solution? (molar mass of solute = 24 g/mol) How many liters of a 0.30 M solution are needed to give 2.7 mol of solute?
- 12. Chapter 16 Review How many liters of a 1.5 M solution are required to yield 5.0 g of solute? (molar mass of solute = 30.0 g/mol) If the volume of solute is 6.0 mL and the volume of solution is 300.0 mL, what is the solute’s percent by volume?
- 13. Chapter 16 Review If the solubility of a gas is 7.5 g/L at 404 kPa pressure, what is the solubility of the gas when the pressure is 202 kPa? What is the number of moles of solute in 650 mL of a 0.40 M solution?
- 14. Chapter 16 Review What is the number of moles of solute in a 0.3 molal solution containing 0.10 kg of solvent? If 1.0 mL of 6.0 M HCl is added to 499 mL of water to give exactly a 500 mL solution, what is the molarity of the dilute solution?
- 15. Chapter 16 Review Calculate the molality of a solution prepared by dissolving 175 g KNO3 in 750 g of water.