Chapters 6-8 Review & Molarity IntroductionWorksheet

Once completed, upload worksheet to the appropriate Assignmentsfolder.

Write the correct chemical formula forthe following combinations or compounds. You must have properformatting to receive credit!

1. sodium and oxygen

1. Al and O

1. aluminum sulfide

1. potassium phosphide

Name the following compounds. Spelling counts!

1. KOH

1. O₂

1. NH₄C₂H₃O₂

1. PbCl₂

Solve the following conversions using the dimensional analysisformat used in the previous worksheets.  Make sure toshow all your work with units (an example has been provided) andlabel your answer with correct units.

Example: What is the molar mass of sodiumchloride?  How many moles of sodium chloride are in 543grams of sodium chloride?

Na=22.99 g/mol

Cl=35.45 g/mol

22.99g/mol + 35.45g/mol = 58.44 g/mol NaCl

Make sure you have amount, units, and material in all your workand every answer for full credit.

1. What is the molar mass of calcium chloride?  How manymoles in 8.00 grams of calcium chloride?

1. What is the molar mass of water?  Convert 2.5 molesof water into grams.

Answer the following question.  You must have properformatting to receive credit!

1. Write and balance an equation including correct states ofmatter for each of the reactant(s) and product(s) that representsthe following reaction:  Although they were formerlycalled the inert gases, the heavier elements of Group 8 do formrelatively stable compounds.  For example, at hightemperatures in the presence of an appropriate catalyst, xenon gaswill combine directly with fluorine gas to produce solid xenontetrafluoride.

Molarity Introduction:  In future laboratoryexperiments, we will be measuring the amount of moles of solutefound in a solution using the solution’sconcentration.  The most common unit of concentrationused by chemists is molarity.  The symbol used is acapital “M” and the units of molarity are moles of solute per literof solution (moles/L).  Up until now, you have been given(or have measured) a mass of that substance and using the PeriodicTable, have calculated moles.  Using the same dimensionalanalysis method, you can calculate moles of a solute given theconcentration (molarity) of thesolution.  Example:  How many moles of HCl arein 25 mL of a 8.0 M (this is read as “eight point zero molar “)solution of hydrochloric acid?

1. Calculate the number of moles of HF in 42.0 mL of a 3.16 Msolution of HF.

1. How many moles of sodium hydroxide are in 80.0 mL of a 1.25 Msolution of sodium hydroxide?