solutions!. what is a solution? a homogeneous mixture! made up of a solute and solvent
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2 Parts of a Solution Solvent – Does the dissolving. Usually present in the larger amount.
Solute – Is dissolved. Usually present in the smaller amount.
Aqueous Solutions
Water is a good solvent because the molecules are polar.
The oxygen atoms have a partial negative charge.
The hydrogen atoms have a partial positive charge.
Hydration
The process of breaking the ions of salts apart.
Ions have charges and attract the opposite charges on the water molecules.
Soluble Vs. Insoluble Soluble: when attraction between ions and water molecules stronger than the attraction between ions
Insoluble: when attraction between the ions is stronger than the attraction between the ions and water molecules
Electrolytes
Conducts an electric current when placed in aqueous solution or in molten state. (Soluble)
Non-electrolytes do not conduct an electric current in either state. (Insoluble)
Properties of Solutions Solubility – how much dissovles
Determined by a few factors.- Nature of solvent and
solute.- Agitation.- Surface area of solute.- Temperature.
Nature of Solvent and Solute “Like dissolves like.”
Water is polar. It has small charges.
It dissolves ionic and polar compounds.
Non-polar will not dissolve.
Agitation Shaking increases the interaction between water and the solute.
What do you do when you make Kool-Aid?
Surface Area More exposed surface area means the water molecules can interact more with the solute.
A powder dissolves better than a solid.
Concentration A quantitative measure of the amount of solute dissolved in a given quantity of solution
Can use a few terms to define concentration. Solubility Molarity Molality
Solubility The amount of a substance that dissolves in a given quantity of a solvent at a given temperature. (g solute/100g solvent)
Saturated vs. Unsaturated vs. Supersaturated
Solubility Saturated
Solvent can’t dissolve more solute
Unsaturated Solvent can dissolve more solute
Supersaturated Solvent dissolved more than expected
Molarity M = moles solute/liters of solution
Uses the symbol M
Example: 2 moles of glucose are dissolved to make 2 liters of solution.
M = 2 moles/2L = 1M
Sample Problem #1 A saline solution contains 0.90g of NaCl in exactly 100mL of solution. What is the molarity of the solution?
Molality Another term used to describe the concentration.
Uses the symbol m.
m = moles solute/kg solvent
Colligative Properties Depend on the number of particles dissolved in a given mass of solvent.
Freezing point depression Boiling point elevation Vapor pressure lowering
Colligative Properties Freezing point depression and boiling point elevation both use a similar equation. ∆T = K(m)(i)
• K is a constant based on the solvent• m is the molality of the solution• i is the van’t Hoff factor, the number of particles a
solute creates in solution
Colligative Properties Which of the following will lower the freezing point of water the most?a. NaClb. Glucosec. CaI2
d. Al2(CO3)3
Types of Reactions
Precipitation reactions When aqueous solutions of ionic compounds are poured together a solid forms.
A solid that forms from mixed solutions is a precipitate
If you’re not a part of the solution, you’re part of the precipitate
Precipitation reactions
NaOH(aq) + FeCl3(aq) NaCl(aq) + Fe(OH)3(s)
is really Na+(aq)+OH-(aq) + Fe+3(aq) + Cl-(aq)
Na+ (aq) + Cl- (aq) +Fe(OH)3(s) So all that really happens is OH-(aq) + Fe+3 (aq) Fe(OH)3(s) Double replacement reaction
Precipitations Reactions
Only happen if one of the products is insoluble
Otherwise all the ions stay in solution- nothing has happened.
Need to memorize the rules for solubility
Solubility Rules
All nitrates are soluble Alkali metals ions and NH4+ ions are soluble
Halides are soluble except Ag+, Pb+2, and Hg2
+2
Most sulfates are soluble, except Pb+2, Ba+2, Hg+2,and Ca+2
Solubility Rules
Most hydroxides are insoluble except NaOH and KOH
Sulfides, carbonates, chromates, and phosphates are insoluble
Lower number rules supersede so Na2S is soluble
Precipitation reaction
We can predict the products Can only be certain by experimenting
AgNO3(aq) + KCl(aq)
Zn(NO3)2(aq) + BaCr2O7(aq)
Three Types of Equations
Molecular Equation- written as whole formulas, not the ions.
K2CrO4(aq) + Ba(NO3)2(aq) Complete Ionic equation show dissolved electrolytes as the ions.
2K+ + CrO4-2 + Ba+2 + 2 NO3
-
BaCrO4(s) + 2K+ + 2 NO3
-
Spectator ions are those that don’t react.