Chemistry: Molarity and Chemical Bonds

A measure of concentration, expressed as the number of moles of solute per liter of solution.

The total volume of the solution, measured in liters.

The amount of a substance contained in a given mass, expressed in moles.

The mass of one mole of a substance, typically measured in grams/mole.

The substance that is dissolved in a solution.

The substance that dissolves the solute to form a solution.

A measure of how much solute is present in a given amount of solvent or solution.

A table of the chemical elements, organized by atomic number.

The SI base unit for amount of substance.

A homogeneous mixture of two or more substances.

A measure of concentration, expressed as the number of moles of solute per liter of solution.

Another term for molarity, expressing a substance's concentration in moles per liter.

A unit of measurement representing 6.022 x 10^23 units of a substance (atoms, molecules, or ions).

The mass of one mole of a substance, usually measured in grams/mole.

The constant 6.022 x 10^23, representing the number of particles in one mole of a substance.

The substance being dissolved in a solution.

A homogeneous mixture of two or more substances

Calculating the number of moles from mass or vice-versa.

M (Molar) or mol/L (moles per liter).

Number of Moles = Mass (g) / Molar Mass (g/mol).

Molarity is a measure of substance concentration, calculated by dividing solute moles by solution liters.

An acid is a substance that donates a proton (H+).

A base is a substance that accepts a proton (H+).

pH measures the concentration of H+ ions in a solution.

The pH scale measures acidity and basicity ranges from 0-14.

A buffer solution resists changes in pH.

A functional group in chemistry containing an oxygen and a hydrogen atom.

A functional group in chemistry containing a carbon and an oxygen atom forming a double bond.

A functional group in chemistry containing a carbon, oxygen and hydroxyl functional group.

Specific arrangements of atoms within molecules that give characteristic chemical properties.

Ammonia (NH3) reacts with water to form ammonium ions (NH4+) and hydroxide ions (OH-), creating a buffer solution. The reaction shows that ammonia acts as a base.

A solution that resists changes in pH when small amounts of acid or base are added.

A measure of the extent to which a weak acid dissociates in water.Indicates how easily an acid releases a proton. Smaller Ka value equals weaker acid.

The negative logarithm of the acid dissociation constant (Ka). A measure of how strong or weak an acid is.

The lower the pKa value, the stronger the acid, and the larger the pKa value, the weaker the acid.

An acid that can donate only one proton (H+) per molecule in a reaction.

An acid that can donate more than one proton (H+) per molecule in a reaction.

The ability of a buffer to resist changes in pH.

pH is inversely proportional to the concentration of hydrogen ions ([H+]). A decrease in pH represents a 10-fold increase in [H+].

The pH range over which a buffer solution effectively resists changes in pH. pKa ± 1.