CHEM 1314 – Exam 3 Flashcards: Solutions & Concentration

Vocabulary flashcards from CHEM 1314 Exam 3 covering solutions, thermochemistry, gas laws, and related concepts.

What is a solute?

The substance dissolved in a solvent.

What is a solvent?

The component present in the greatest amount.

What does concentration measure?

Ratio of solute to solvent.

Formula for molarity?

M = moles / volume (L).

Relationship between moles, concentration, and volume?

n = C × V.

What happens when ionic compounds dissolve?

They dissociate into ions.

NaCl in water produces what ions?

Na⁺ and Cl⁻.

If NaCl is 0.034 M, what is [Na⁺]?

0.034 M.

What happens during dilution?

Solvent added → concentration decreases.

Dilution formula?

C₁V₁ = C₂V₂.

What is a titration used for?

Finding unknown concentration.

What is the endpoint?

When color changes.

What is equivalence point?

Reaction is complete (perfect mole ratio).

What is energy?

Capacity to do work or transfer heat.

Kinetic energy formula?

KE = ½mv².

SI unit of energy?

Joule (J).

1 cal equals?

4.184 J.

Open system?

Exchanges heat and matter.

Closed system?

Exchanges heat only.

Isolated system?

Exchanges neither.

Internal energy equation?

∆U = q + w.

When heat enters system?

q is positive.

When system does work?

w is negative.

Enthalpy formula?

H = U + PV.

∆H positive means?

Heat absorbed.

∆H negative means?

Heat released.

Heat equation?

q = mc∆T.

Boyle’s Law?

P₁V₁ = P₂V₂.

Charles’s Law?

V₁/T₁ = V₂/T₂.

Ideal Gas Law?

PV = nRT.

Total pressure?

Sum of partial pressures.

Vapor pressure?

Increases with temperature.