Chapters 15 & 16: Toxins in Solution and Acidic Toxins Flashcards

This flashcard set covers key vocabulary from chemistry lecture notes on solution types, solubility factors, molarity, dilutions, and acid-base theories and calculations.

Triple Point

The condition where the solid, liquid, and gas phases of a substance are all present at once.

Solute

The particles that are being dissolved in a solution.

Solvent

The dissolving medium in a solution.

Aqueous Solution

A homogeneous solution in which the solute is dissolved in water.

Solvation

A process by which individual solute ions break away from the crystal, become surrounded by solvent molecules, and the ionic crystal dissolves.

Electrolyte

A substance that dissolves in water to give a solution that conducts electric current, such as $NaCl$ in water.

Nonelectrolyte

A substance that dissolves in water to give a solution that does not conduct electric current, such as sucrose in water.

Suspension

A mixture where the particles in a solvent are so large that they settle out unless the mixture is constantly stirred or agitated.

Colloid

A mixture that has particles intermediate in size between those in solutions and suspensions, such as milk or mayonnaise.

Tyndall Effect

A property used to distinguish between a solution and a colloid where a beam of light is scattered by colloidal particles, making the beam visible.

Saturated solution

A solution that contains the maximum amount of solute for a given quantity of solvent at a given temperature and pressure.

Unsaturated solution

A solution that contains less solute than a saturated solution at a given temperature and pressure.

Supersaturated solution

A solution that contains more solute than it can theoretically hold at a given temperature.

Seed crystal

A very small crystal of the solute added to a supersaturated solution to initiate crystallization.

Solubility

The amount of solute that dissolves in a given quantity of a solvent at a specified temperature and pressure to produce a saturated solution.

Miscible

A description of two liquids that dissolve in each other in all proportions.

Immiscible

A description of two liquids that are insoluble in each other.

Henry's Law

The principle that the solubility of a gas is directly proportional to the partial pressure of that gas on the surface of the liquid.

Molarity ($M$)

A measure of concentration defined as the number of moles of solute dissolved in one liter of solution ($mol/L$).

Dilute solution

A solution that contains a small amount of solute.

Concentrated solution

A solution that contains a large amount of solute.

Alloy

A solid-solid solution, such as brass which is copper in zinc.

Arrhenius Acid

A substance that is an $H^+$ or $H_3O^+$ producer in solution.

Arrhenius Base

A substance that is an $OH^-$ producer in solution.

Br%f8nsted-Lowry Acid

A substance that acts as a proton ($H^+$) donor.

Br%f8nsted-Lowry Base

A substance that acts as a proton ($H^+$) acceptor.

Lewis Acid

A substance that acts as an electron pair acceptor.

Lewis Base

A substance that acts as an electron pair donor.

Indicator

A substance that turns one color in the presence of acids and another color in the presence of bases.

Conjugate Acid

The particle formed when a base gains a proton ($H^+$).

Conjugate Base

The particle that remains when an acid has donated a proton ($H^+$).

Amphoteric

Compounds that can act as either an acid or a base depending on the situation, such as water.

Ion product constant of water ($K_w$)

The equilibrium constant for the self-ionization of water, where the product of the molarity of hydronium and hydroxide ions is $1.0 \times 10^{-14}$ at $25\,^\circ C$.

pH scale

A logarithmic scale that describes the concentration of $H^+$ ions in solution, ranging from 0 to 14.

pOH scale

A logarithmic scale that describes the concentration of $OH^-$ ions in solution.

Titration

A laboratory procedure used to calculate the concentration of a solution by reacting it against a solution of known concentration.