Stoichiometry of Chemical Reactions

Molecular equation

________: shows complete chemical formulas of reactants and products.

Solubility

________: the maximum concentration of a solute that can dissolve in a solvent at a given temperature.

Coefficients

________: indicate the relative numbers of molecules of each kind.

Dissociation

________: when an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them.

Arrhenius

Based defined by ________: substances that increase the concentration of OH− when dissolved in water.

Titration

________: an analytical technique in which one can calculate the concentration of a solute in a solution.

Dissolution

________: the process where a solute dissolves in a solvent to form a solution.

Subscripts

________: indicate composition; changing the ________ changes the identity of the molecule.

Acids

________ defined by Arrhenius: substances that increase the concentration of H+ when dissolved in water.

Nonmetals

________ usually have negative oxidation numbers a) Oxygen is usually- 2 except in peroxides where it is- 1 b) Hydrogen is +1 when bonded to ________ and- 1 when bonded to metals c) Fluorine is- 1 in all compounds.

Analyte

________: solution being analyzed; solution in flask; solution of unknown concentration.

Chemical equations

________ represent chemical reactions.

Theoretical yield

________: the quantity of product calculated to form when all of the limiting reactant is consumed.

Oxidation numbers

________: bookkeeping device to track loss or gain of electrons in a redox reaction.

Ions

________ that cancel out are called spectator ________.

Titrant

________: solution in the buret; known in the concentration; can be either acid or base depending on the nature of the analyte.

dissolution

When ________ occurs, two or more substances disperse (or disappear) into each other to form a homogeneous solution.

oxidation numbers

The sum of the ________ in a neutral compound is zero; in a polyatomic ion the sum is equal to the charge on the ion.

Coefficients

indicate the relative numbers of molecules of each kind

Subscripts

indicate composition; changing the subscript changes the identity of the molecule

Dissolution

the process where a solute dissolves in a solvent to form a solution

Solubility

the maximum concentration of a solute that can dissolve in a solvent at a given temperature

Dissociation

when an ionic substance dissolves in water, the solvent pulls the individual ions from the crystal and solvates them

Molecular equation

shows complete chemical formulas of reactants and products

Net ionic equation

shows reactants and products actually participating in the reaction

Acids defined by Arrhenius

substances that increase the concentration of H+ when dissolved in water

Acids defined by J. N. Brønsted and T. M. Lowry

acids as proton donors

Based defined by Arrhenius

substances that increase the concentration of OH− when dissolved in water

Bases defined by Brønsted and Lowry

proton acceptors

Oxidation numbers

bookkeeping device to track loss or gain of electrons in a redox reaction

Theoretical yield

the quantity of product calculated to form when all of the limiting reactant is consumed

Actual yield

the quantity of product actually obtained (usually less than the theoretical yield)

Titration

an analytical technique in which one can calculate the concentration of a solute in a solution

Titrant

solution in the buret; known in the concentration; can be either acid or base depending on the nature of the analyte

Analyte

solution being analyzed; solution in flask; solution of unknown concentration

Equivalence point

volume of titrant where moles titrant and moles of analyte are exactly equal

End point

the physical indication of the equivalence point; comes after the actual equivalence point