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Chapter 22 Sect. 2: Solubility and Concentration

Chapter 22 Sect. 2: Solubility and Concentration. What has to take place in order for a solute to be dissolved? _______________molecules ________________the _________________particles and pull the solute particles into solution, and the complex spreads out evenly throughout the solution.

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Chapter 22 Sect. 2: Solubility and Concentration

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  1. Chapter 22 Sect. 2: Solubility and Concentration

  2. What has to take place in order for a solute to be dissolved? • _______________molecules ________________the _________________particles and pull the solute particles into solution, and the complex spreads out evenly throughout the solution Dissolving Review

  3. What determines the amount of solute that is able to dissolve in a solvent? • ____________: the ____________amount of ________________that can be ______________in a given amount of ___________at a given temperature • Solubility depends on the properties of the solute and solvent • Some solutes are more “soluble” in some solvents than others • This means that more of it can be dissolved in that particular solvent than in a different solvent, or more will dissolve in a solvent compared to another solute Solubility

  4. The concentration of a solution refers to the ___________of solute __________in a solution • Concentrated: Solutions with a ___________amount of solute particles • Diluted: Solutions with a ___________amount of solute particles Concentrated vs. Diluted

  5. To find the concentration of a solution: • Divide the _______of the __________by the ___________of _________________ • We will use units of grams of solute per 100 mL of solvent (_________________) • i.e. the concentration of a sample of salt water is 35.9 g/100 mL of water • You may need to set up a proportion to determine concentration Concentrations of Solutions =

  6. 1. What is the concentration of a solution in grams/100 mL when 40 grams of solute dissolve in 200 mL of solution? 2. A solution contains 15 grams of solute in 30 mL of solution. What is the concentration of the solution in g/100 mL? 3. A solution has a concentration of 2 g/ 100 mL. If you have 600 mL of the solution, how many grams of solute do you have? Calculating Concentrations

  7. There are three other terms that can be used to describe the concentration of a solution based on the ___________of _____________that is dissolved • ______________– a solution that contains __________ of the ____________solute that it can hold at a given temperature (no more solute can dissolve) • _______________– a solution that can dissolve ____________solute at a given temperature • _______________– a solution that contains __________ solute than a saturated solution at the same temperature • Usually in order to produce a supersaturated solution, the solution needs to be ____________ which increases the _____________of most substances • Gases on the other hand are more soluble in liquids when the temperature is ___________________ Types of Solutions

  8. Our classroom has 27 desks… • If there are < 27students: ______________classroom – more students can still fit in the class • If there are 27students: ______________classroom – can not fit anymore students • If there are > 27students, _____________classroom– adding more causes students to be displaced, or fall into aisles (__________________) • Increase _______________, students up and moving around the room, more energy, more students can fit in the classroom Saturation analogy

  9. A solubility curve is a ___________ showing the relationship between _____________and ____________ (or sometimes pressure) • We can use solubility curves to figure out how much __________will dissolve in a particular solvent at a certain temperature • We can also use them to determine if a solution is saturated, unsaturated, or supersaturated • If above the curve: ________________ • If on the line of the curve: ___________ • If below the curve: ______________ Solubility curves

  10. Use the solubility curve to the right to answer the following questions. What is the solubility of Ba(OH)2 in 100 mL of water at 80˚C? At about what temperature will 100g of water dissolve equal amounts of KNO3 and NaNO3? (Hint: 100g water = 100 mL water) How many grams of KNO3 are needed to produce a saturated solution at 40˚C? If 120g of NaNO3 are dissolved in 100g of water at 20˚C, is the solution saturated, unsaturated or super saturated? If 70g of KI are dissolved in 100g of water at 30˚C, is the solution saturated, unsaturated or super saturated? Solubility curves Practice

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