Unit 6: Reaction Stoichiometry

You will be able to:

balance a chemical reaction.
write a chemical equation from the description of a chemical reaction.
use the solubility rules to predict the solubility of an ionic compound and to predict whether a reaction occurs between two ionic compounds.
calculate molarity from mass and volume.
use molarity as a conversion factor.
use molarity to make calculations about the dilution of a solution.
relate the coefficients in a balanced chemical equation to the moles of reactants and products and products.
relate the number of moles of two substances in a balanced chemical equation.
classify and perform the three basic types of stoichiometry problems: mass-mass, mass-mole, and mole-mole calculations.
explain the concept of a limiting reactant.
identify the limiting reactant in a chemical reaction given the number of moles of each reactant.
calculate the percent yield for a reaction given the actual yield.

Readings:

Solubility Rules (You need to know how to use these, not memorize them.)

Activity Series (You need to know how to use these, not memorize them.)

What to know for the test

Take an equation written in words and write it in symbols.
Balance a chemical equation.
Write the net ionic equation for a reaction.
Given a set of solubility rules, predict the precipitate for a reaction.
Given the metal activity series, predict the reaction or if no reaction occurs.
Use the factor-label method to complete a stoichiometric calculation involving a chemical reaction. (mole-mole, mass-mass, mass-mole)
Use a molar solution concentration in a stoichiometric calculation.
Solve a limiting reactant problem including deciding what the limiting reactant is and what amount of excess reactant remains.
Comparing actual and theoretical yield to give the percent yield for the reaction.

These may be combined with individual questions. There is not necessarily a separate question for each of the above.

T.2024.05.07.Stoichiometry - Practice

Sildes

Unit 6.1: Writing and Balancing Reactions

Unit 6.2 Solubility Rules

Unit 6.3 Simple Stoichiometry

Unit 6.4 Molarity

Unit 6.5 Limiting Reactant

Laboratory

Precipitation Reaction and General Solubility Rules

Materials: BaCl2, Na2CO3, K2CrO4, NaOH, MgCl2, Na2SO4, AgNO3, Pb(NO3)2, KNO3, 96-well plate, micro-tip pipettes

Using a 96-well plate mix all of the possible solution combinations.

Place 2 drops of each solution in the well. In the upper right, write R if a precipitate forms or NR if no precipitate forms.

Write the formula for the precipitate in the box.
Write the balanced net ionic equation for each precipitation reaction.
Develop some general rules for solubility based on your results. (ex. All chlorides are soluble except...)
Using your rules, what could you add to separate the following pairs of ions? (That is, what could you add to precipitate only one of the ions.)
- a. Mg2+ and Ba2+
- b. Ag+ and Pb2+
- c. K+ and Mg2+