Untitled Flashcards Set

1. Vocabulary Matching (20 pts)

Know these definitions and functions:

Term Meaning

Acid Produces H⁺ in water, pH < 7

Base Produces OH⁻ in water, pH > 7

Bronsted-Lowry Acid Donates H⁺

Bronsted-Lowry Base Accepts H⁺

Amphoteric Can act as both an acid and a base (e.g. H₂O)

Calorie Unit of energy; 1 Calorie = 1000 calories

Catalyst Speeds up a reaction, lowers activation energy

Activation Energy Minimum energy needed to start a reaction

Collision Theory Particles must collide with correct energy + orientation to react

Endothermic Absorbs heat; ΔH is positive

Exothermic Releases heat; ΔH is negative

Heat Thermal energy transfer

Specific Heat (c) Energy needed to raise 1g of a substance by 1°C

Surroundings Everything outside the system

System The part of the universe under study (e.g., the reaction)

Molarity (M) Moles of solute / Liters of solution

Monoprotic Acid Donates 1 H⁺ (e.g., HCl)

Diprotic Acid Donates 2 H⁺ (e.g., H₂SO₄)

Triprotic Acid Donates 3 H⁺ (e.g., H₃PO₄)

Neutralization Acid + base → water + salt

Le Châtelier’s Principle Equilibrium shifts to relieve stress

Equilibrium Constant (Keq) Ratio of products to reactants at equilibrium

Reaction Quotient (Q) Same formula as Keq but at any point in time

Rate Law Rate = k[A]^x[B]^y — shows how concentration affects rate

pH -log[H⁺]

pOH -log[OH⁻]

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2. Formulas to Memorize

Molarity

M = \frac{\text{moles of solute}}{\text{liters of solution}}

• Know how to solve for any of the three variables

• Convert grams ↔ moles using molar mass

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Thermochemistry

Basic:

q = m \times c \times \Delta T

• q = heat (J)

• m = mass (g)

• c = specific heat (J/g°C)

• \Delta T = change in temperature (°C)

Law of Conservation of Energy:

q_{\text{lost}} = q_{\text{gained}}

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Equilibrium and Rate Laws

Equilibrium Constant (Keq):

K_{eq} = \frac{[products]^{coeff}}{[reactants]^{coeff}}

Reaction Quotient (Q):

• Compare to Keq to predict direction:

• If Q < Keq → shift right (toward products)

• If Q > Keq → shift left (toward reactants)

• If Q = Keq → system is at equilibrium

Rate Law (for aA + bB → products):

\text{Rate} = k[A]^x[B]^y

• x and y = reaction order (usually determined from experiment)

• Overall order = x + y

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Acids and Bases

pH and pOH:

\text{pH} = -\log[H⁺], \quad \text{pOH} = -\log[OH⁻]

\text{pH} + \text{pOH} = 14

From pH to [H⁺]:

[H⁺] = 10^{-\text{pH}}, \quad [OH⁻] = 10^{-\text{pOH}}

Water constant:

[H⁺][OH⁻] = 1.0 \times 10^{-14}

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3. Problem Types to Practice (11 x 10 pts = 110 pts)

• Molarity problems: Given grams + volume, find M; or given M + volume, find grams/moles.

• Calorimetry: Use q = mc\Delta T; balance heat gained = heat lost.

• Reaction Rates: Determine rate law from data; describe how catalysts, temperature, surface area affect rates.

• Equilibrium Calculations: Use Keq or Q to predict shifts or find concentrations.

• Le Châtelier’s Principle: Predict shifts due to temperature, concentration, or pressure changes.

• Acid/Base Calculations: Calculate pH, [H⁺], or [OH⁻]; identify acid/base types (Arrhenius vs. Bronsted-Lowry).

• Neutralization: Use stoichiometry to find moles, volume, or concentration at neutralization.

• Endo vs. Exothermic: Interpret ΔH values or heating curves.

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4. Long Answer Essays (2 x 20 pts = 40 pts)

Be ready to:

• Explain equilibrium shifts using Le Châtelier’s Principle

• Describe how reaction rates change under different conditions

• Solve multi-step molarity or calorimetry problems

• Compare acids and bases using different definitions and calculations

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