Mix & Match
What do you call a uniform mixture made of two or more substances?
solution
What general rule explains why polar dissolves polar and nonpolar dissolves nonpolar?
"Like dissolves like"
What are dissolved ions in a solution called?
electrolytes
What unit represents moles of solute per liter of solution?
molarity
What happens to the freezing point of water when salt is added?
decreases
Which component is present in the greatest amount—solute or solvent?
Solvent
What happens to the solubility of a gas as temperature increases?
Decreases
What process occurs when an ionic compound breaks apart in water?
Dissociation
What’s the formula for molarity?
M = mol/L
What’s the name of properties that depend on concentration, not identity?
Colligative properties
What kind of solution has only a little solute compared to solvent?
Dilute solution
Name two factors that affect solubility.
temperature and pressure
NaCl → Na⁺ + Cl⁻ is an example of what?
Dissociation
What does M₁V₁ = M₂V₂ solve for?
dilution calculations
Why does salty water boil at a higher temperature than pure water?
boiling point elevation
Water is often called this because it dissolves so many things.
Universal solvent
Will oil dissolve in water? Why or why not?
No because oil is nonpolar and water is polar
What process creates ions from neutral molecules like HCl?
Ionization
What’s the difference between molarity and molality?
molarity uses liters of solution, molality uses kg of solvent
What’s the formula for calculating heat during phase change (e.g., vaporization)?
q = mΔHvap
If there are too many solute particles present, what type of solution is it?
supersaturated
A saturated solution of potassium nitrate (KNO₃) is cooled from 60°C to 20°C. Crystals form at the bottom of the container. What does this tell you about the solubility of KNO₃ with temperature?
the solubility of KNO₃ decreases as temperature decreases
HCl + H₂O → H₃O⁺ + Cl⁻ — what ion is newly formed here?
H3O+ and Cl-
How many moles of solute are in 2 L of a 3 M NaCl solution?
6 moles
Explain how colligative properties help on icy roads.
salt lowers the freezing point, melting the ice