Week 14-15

Flashcards about Solution Chemistry, Precipitation, and Gases

Name different ways of expressing concentrations.

Qualitative and quantitative.

What are the principles of dilution?

The process of reducing the concentration of a solute in a solution by adding more solvent.

Compare and contrast strong electrolytes, weak electrolytes, and nonelectrolytes.

Strong electrolytes dissociate completely into ions when dissolved in water, weak electrolytes dissociate partially, and nonelectrolytes do not dissociate into ions.

Name some common strong acids and strong bases.

Includes HCl (hydrochloric acid), HBr (hydrobromic acid), HI (hydroiodic acid), HNO3 (nitric acid), H2SO4 (sulfuric acid), and HClO4 (perchloric acid). Strong bases include Group 1 hydroxides (e.g., NaOH, KOH) and some Group 2 hydroxides [Ca(OH)2, Sr(OH)2, Ba(OH)2].

What are neutralization reactions?

Reactions where an acid and a base react to form a salt and water.

What are precipitation reactions?

Reactions where two soluble salts react to form an insoluble product (a precipitate).

What are solubility rules?

Rules that predict whether a compound will dissolve in water based on its ions.

What is oxidation half-reaction?

The loss of electrons or an increase in oxidation state.

What is reduction half-reaction?

The gain of electrons or a decrease in oxidation state.

What is an oxidizing agent?

The substance that causes oxidation by accepting electrons.

What is a reducing agent?

The substance that causes reduction by donating electrons.

How do you balance redox equations?

Using the half-reaction method.

What are organic compounds?

Molecules that contain carbon atoms bonded mainly to hydrogen, but often also to oxygen, nitrogen, sulfur, or other elements.

What is a precipitate?

The solid product formed from a reaction in solution.

What is Titration?

Progressive addition of a standard solution of known concentration to determine the concentration of a solute in a sample

What is the end point in titration?

The point in a titration where the indicator changes color.

Name the simple gas laws.

Boyle’s, Charles’s, Avogadro’s, and the combined gas law.

What is Dalton's Law of Partial Pressures?

The total pressure of a mixture of gases is the sum of the partial pressures of the components.

What are the assumptions of KMT (Kinetic Molecular Theory)?

Gas molecules have tiny volumes compared with the volume the gas occupies, gas particles do not interact with each other, gas molecule collisions are elastic, and the average kinetic energy of the molecules in a gas is proportional to the absolute temperature.

What is the Perfect gas equation?

PV = nRT

What does Graham’s Law state?

Rate of effusion is inversely proportional to molar mass.

How is Atmospheric pressure measured?

Atmospheric pressure is measured with a barometer.

What is the relationship between volume and pressure of a gas (at constant temperature)?

The volume of a gas at constant temperature is inversely proportional to its pressure.

What are the two assumptions for the behavior of an ideal gas?

Volumes of individual gases are insignificant compared to overall volume. Particles do not interact with one another.

What is enthalpy (H)?

A measure of the total heat content of a system, calculated as: H = U + PV.

What is enthalpy change (ΔH)?

The change in enthalpy during a reaction (ΔH). Negative ΔH is exothermic; positive ΔH is endothermic.

What is an exothermic reaction?

A reaction that releases heat, resulting in a negative ΔH.

What is an endothermic reaction?

A reaction that absorbs heat, resulting in a positive ΔH.

What is specific heat capacity (c)?

The heat needed to raise the temperature of one gram of a substance by 1°C.

What is molar heat capacity?

The heat required to raise the temperature of one mole of a substance by 1°C.

What is Hess's Law?

The enthalpy change for a reaction is the same whether it occurs in one or multiple steps.

What is the standard enthalpy of formation (ΔH_f^o)?

The enthalpy change when one mole of a compound is formed from its elements in their standard states (ΔH_f^o).

What is heat (q)?

Energy transferred due to a temperature difference.

What is a calorimeter?

A device measuring heat in chemical or physical processes, like coffee cup calorimeters (constant pressure) and bomb calorimeters (constant volume).