Vocab 4/1

Amphoteric

a substance such as a metal hydroxide that can behave as either an acid or a base.

Aqueous

a solution of substances dissolved in water.

Concentration

the amount of solute dissolved in a given amount of solution.

Corrosion

the deterioration of metals by oxidation-reduction reactions.

Electrolyte

a substance whose aqueous solution conducts electricity.

Equivalence point

the point in a titration when one reactant has been completely consumed by another reactant or when the amount of H+ exactly equals OH-

Formal charge

the charge on an atom in a molecule or ion calculated by \n assuming equal sharing of the bonding electrons.

Indicator

a substance used to signal the equivalence point in a titration by \n changing color.

Lewis acid

a substance that can accept a pair of electrons to form a new bond.

Lewis base

a substance that can donate a pair of electrons to form a new bond.

Mantissa

the part of a logarithm to the right of the decimal point.

Molarity

the number of moles of solute per liter of solution.

Monoprotic acid

an acid that can donate one proton.

Net ionic equation

an equation that shows only the substances undergoing \n chemical changes in a reaction and omitting the spectator ions.

Neutral solution

a solution in which the concentrations of hydrogen ion andhydroxide ion are equal.

Neutralization

an acid-base reaction that produces a neutral solution of

salt and water.

Nonelectrolyte

substances whose aqueous solutions do not conduct electricity.

Oxidation

the loss of electrons by an atom, ion or molecule causing the charge to increase

Oxidation number

a number assigned to each element in a compound to keep track of the electrons.

Oxidizing agent

a substance that accepts electrons and is reduced

Peroxides

compounds containing oxygen to oxygen single bonds or the O 2 - ion

pH

the negative logarithm of the hydrogen ion concentration.

pOH

the negative logarithm of the hydroxide ion concentration.

Polyprotic acid

an acid that can donate more than one proton.

Precipitate

an insoluble solid that forms from two reactants in aqueous solution.

Primary standard

a pure solid acid or base that can be weighed for preparing the known quantity in a titration

Qualitative analysis

information or analysis which is not based on numbers and measurements but on observations and descriptions

Quantitative analysis

information or analysis based on numbers or measurements.

Reducing agent

a substance that donates electrons and is oxidized.

Reduction

the gain of electrons by an atom, molecule or ion causing the charge to decrease.

Salt

an ionic compound whose cation is not H + and whose anion is not OH - .

Saturated solution

a stable solution in which the maximum amount of solute has been dissolved.

Solute

a substance present in the lesser quantity that gets dissolved by the solvent \n in a solution.

Solvent

the medium in which the solute is dissolved to form a solution.

Solution

a homogeneous mixture.

Solubility

the maximum amount of solute that will dissolve in a given amount of solvent at a given temperature to form a stable solution

Strong acid

an acid that completely ionizes in aqueous solution and greatly increases the concentration of H + 

Strong base

a base that completely ionizes in aqueous solution and greatly increases the concentration of OH - .

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Strong electrolyte

substances whose aqueous solutions are very good conductors of electricity.

Titration

procedure for analysis of a substance by an essentially complete reaction in solution with a measured quantity of a reagent of known concentration.

Weak acid

an acid that only partially ionizes in aqueous solution and therefore slightly increase the concentration of H + .

Weak base

a base that only partially ionizes in aqueous solution and therefore slightly increase the concentration of OH - .

Weak electrolyte

a substance that dissolves in water and is a weak conductor of electricity.