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Solutions
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Solutions Solute- the substance being put into the solution.
Solvent- the substance in which the solute is being put into. Solution- the substance that results from a solute being put into a solvent. Example: Salt is a solute, Water is the solvent, Salt Water is the solution.
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Types of Solutions Are all solutions liquids?! NO!
Write down some examples: Solute Solvent Example Solution Gas Air Liquid Soda Juice Solid Sweet Tea Steel
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Solutions Soluble versus Insoluble. Miscible versus Immiscible.
Soluble – dissolved in solution. Insoluble – will not dissolve in solution. Miscible versus Immiscible. Miscible – “Mixable” able to mix together. (Ex. Water and Bleach) Immiscible – Not able to mix together. (Ex. Water and Oil)
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Types of Mixtures Solution Colloid Suspension Particle Size smallest
middle largest Tyndall Effect (scattering of light; or cloudy) No Yes Settles out/Filtration Mixture Type Homogeneous Heterogeneous Example Salt water Fog/Milk Muddy water
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Water as the Universal Solvent
What are some properties of water that make it a good solvent? Polar molecule: dissolves other polar substances IMF’s: High boiling point so it remains a liquid at room temperature and higher Most abundant liquid on earth
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“likes dissolves likes”
Polar substances dissolve other polar substances Nonpolar substances dissolve other nonpolar substances Polar substances do NOT dissolve nonpolar substances
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Will they be soluble? CH4 and H2O NH3 and H2O
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Will they be soluble? CH4 and H2O – CH4 is nonpolar, H2O is polar. They will NOT be soluble. NH3 and H2O – Both are polar. They will be soluble!
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Solutions as Electrolytes
Electrolyte: substances that dissolve in water to give a solution that conducts electricity Good electrolytes: substances that form IONS ionic compounds, acids, bases Non-electrolytes: DON’T FORM IONS: most molecular compounds (COVALENT)
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Electrolyte Versus Nonelectrolyte
Electrolyte- Ionic compounds that dissociate (or break apart) into their charged ions. Conducts electricity Nonelectrolyte- do not dissociate therefore they don’t conduct electricity
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Play the Electrolytes video from the website
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Play this video as well
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Decide if each chemical is an electrolyte or a nonelectrolyte
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Electrolyte or Nonelectrolyte?
NaCl Electrolyte - Ionic
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Electrolyte or Nonelectrolyte?
H2SO4 Electrolyte - Acid
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Electrolyte or Nonelectrolyte?
CO2 Nonelectrolyte - covalent
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Electrolyte or Nonelectrolyte?
C6H12O6 Nonelectrolyte - covalent
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Electrolyte or Nonelectrolyte?
K3PO4 Electrolyte - Ionic
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Electrolyte or Nonelectrolyte?
CCl4 Nonelectrolyte - covalent
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Electrolyte or Nonelectrolyte?
Ca(OH)2 Electrolyte – ionic, base
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Electrolyte or Nonelectrolyte?
HCl Electrolyte - acid
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Electrolyte or Nonelectrolyte?
SO2 Nonelectrolyte - covalent
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Electrolyte or Nonelectrolyte?
KOH Electrolyte – ionic, base
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The Solution Process Solvation: process by which solvent particles surround solute particles Dissociation: separation of ionic compounds into ions Hydration: Solvation with water as a solvent; ions are surrounded by water molecules and kept separate (H on the water is attracted to the negative ion; O is attracted to the positive ion)
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Dissociation The separation of ions from one another.
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Hydration Water molecules attach to dissolving molecules and ions.
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Play this video:
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Factors that Affect Rate of Solution
Increasing surface area: the smaller the crystals, the faster it will dissolve because of the greater surface area, stirring also increases surface area and rate of solution Increasing temperature: Increases rate because particles move faster
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More Factors that Affect Rate of Solution
Increasing pressure: GASES ONLY, increasing pressure increases the increases the rate (Think about soda) Increasing concentration – more particles means more collisions, so rate increases Using a catalyst – speeds up the rate by lowering activation energy
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Solubility Solubility refers to HOW MUCH solute can be dissolved in an amount of solvent (Different than RATE which is the SPEED at which something dissolves)
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Factors that Affect Solubilty
Nature of solute/solvent: Polar dissolves polar, nonpolar dissolves nonpolar, polar does NOT dissolve nonpolar Temperature: For solid and liquid solutes: increasing temperature increases solubility For gas solutes: increasing temperature decreases solubility (think about soda Pressure: GASES ONLY! Increasing pressure means MORE can dissolve (increased solubility)
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Key Terms: Saturated – solution is holding the maximum amount of solute that it can hold Unsaturated – solution is holding less than the maximum amount of solute Supersaturated – solution is holding more than the maximum amount of solute
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Solubility Curves Shows the amount of a solute (in grams) that will dissolve in a specific amount of water (usually 100g) at various temperatures.
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Play Solubility Curves video
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Try It: 1. Which substance has the highest solubility at 10°C?
2. How much KCl can 100 g of water hold at 50°C? 3. How much KCl can 300g of water hold at 50°C? 4. If a solution contains 100 g of NaNO3 at 20°C, is the solution saturated, unsaturated, or supersaturated?
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Solution Concentration
Concentration is a measure of the amount of solute in the amount of solvent or solution. Qualitative measures of concentration Dilute: small amount of solute compared to the amount of solvent (could be a saturated solution) Concentrated: large amount of solute compared to the amount of solvent
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Play Molarity video
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Molarity and Concentration
Quantitative measures of concentration:
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Practice Problem 1 What is the molarity of a solution containing 5.85 grams of potassium iodide in 125 mL of solution?
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Practice Problem 2 How many moles of sulfuric acid are present in 500 mL of a M solution?
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Practice Problem 3 What is the mass of sodium chloride in 240 mL of a 3.00 M solution?
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Play dilutions video
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Diluting Solutions H2O 2M 12M M1V1=M2V2 Moles = Moles
M=mol/volume ; mol= (M)(V) M1V1=M2V2
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Diluting Solutions – Practice Problem
What volume of 2.00M CaCl2 would you use to make 0.5L of 0.300M CaCl2?
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Quiz Topics Solutions Vocab Molarity Calculations
Solubility (how is it affected) Solubility Curves Saturated, Unsaturated, Supersaturated
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Colligative Properties
Definition: Physical properties of a solution that are affected by the number of solute particles. Four you need to know: Vapor pressure lowers Boiling point rises Freezing point lowers Osmotic pressure increases
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Colligative Properites
Electrolytes: NaCl(s) Na+(aq) + Cl- (aq) Since electrolytes break apart in solution, there are more particles, and therefore a bigger effect on the colligative properties Nonelectrolytes: C12H22O11(s) C12H22O11(aq) They don’t break apart in solution, so there are fewer particles, and a smaller effect.
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Vapor Pressure Lowering
Vapor pressure lowers when a solute is present, because it is more difficult for a solvent to evaporate because of the strong IMF formed between the solute and solvent
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Boiling Point Elevation
Adding salt (or any solute) to water increases its boiling point Increases boiling point because more imfs between solute and solvent to break before the solution boils
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Freezing Point Depression
Decreases freezing point because more imfs to overcome before the solution freezes
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Osmotic Pressure The pressure needed to reverse or stop osmosis
Osmosis: the diffusion of solvent particles across a semipermeable membrane
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