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Chapters 6-8 Review & Molarity Introduction Worksheet Once completed, upload worksheet to the appropriate Assignments folder....

Chapters 6-8 Review & Molarity Introduction Worksheet

Once completed, upload worksheet to the appropriate Assignments folder.

Write the correct chemical formula for the following combinations or compounds. You must have proper formatting to receive credit!

sodium and oxygen

Al and O

aluminum sulfide

potassium phosphide

Name the following compounds. Spelling counts!

KOH

O₂

NH₄C₂H₃O₂

PbCl₂

Solve the following conversions using the dimensional analysis format used in the previous worksheets. Make sure to show all your work with units (an example has been provided) and label your answer with correct units.

Example: What is the molar mass of sodium chloride? How many moles of sodium chloride are in 543 grams 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 work and every answer for full credit.

What is the molar mass of calcium chloride? How many moles in 8.00 grams of calcium chloride?

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

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

Write and balance an equation including correct states of matter for each of the reactant(s) and product(s) that represents the following reaction: Although they were formerly called the inert gases, the heavier elements of Group 8 do form relatively stable compounds. For example, at high temperatures in the presence of an appropriate catalyst, xenon gas will combine directly with fluorine gas to produce solid xenon tetrafluoride.

Molarity Introduction: In future laboratory experiments, we will be measuring the amount of moles of solute found in a solution using the solution’s concentration. The most common unit of concentration used by chemists is molarity. The symbol used is a capital “M” and the units of molarity are moles of solute per liter of solution (moles/L). Up until now, you have been given (or have measured) a mass of that substance and using the Periodic Table, have calculated moles. Using the same dimensional analysis method, you can calculate moles of a solute given the concentration (molarity) of the solution. Example: How many moles of HCl are in 25 mL of a 8.0 M (this is read as “eight point zero molar “) solution of hydrochloric acid?

Calculate the number of moles of HF in 42.0 mL of a 3.16 M solution of HF.

How many moles of sodium hydroxide are in 80.0 mL of a 1.25 M solution of sodium hydroxide?

Expert Solution

queen_honey_blossom answered 8 months ago

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