Last modified: Wed 08/27/2014 07:57:57 pm ACA

Oklahoma State University

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1. When working with aqueous solutions a method of knowing the relative amounts of each component is needed. Suppose we add 5.85 grams of NaCl (the solute) to some water (the solvent) and allow all the NaCl to dissolve. After the NaCl dissolves the volume of the solution is measured and found to be 100.0 mLs.

a) How many moles of NaCl dissolved in the water? mol

b) What is volume of the solution in liters? L

2. One way of expressing the amount of solute (NaCl) contained in the solution is using a concentration expression called molarity. Molarity is defined as,

Molarity of solution = moles solute/Liters of solution

a) Calculate the molarity of the NaCl solution discussed in Q1 above. M

3. Calculate the molarity of each of the following solutions,

a) 35.0 grams of MgCl2 dissolved in enough water to prepare 250. mLs of solution. M

b) 35.0 grams of C6H12O6 dissolved in enough water to prepare 3.00 L of solution. M

4) How many moles of NaCl are in 1 liter of 1 M NaCl? mol

5) How many moles of NaCl are in 5 liters of 1 M NaCl? mol

6) How many moles of NaCl are in 0.200 L of 0.345 M NaCl? mol

7. Consider the following reaction

NaCl(aq) + AgNO3(aq) ----> AgCl(s) + NaNO3(aq)

a) How many moles of AgNO3 are required to react with 2.50 mol of NaCl? mol

b) How many moles of AgNO3 are required to react with 50.0 mLs of 0.400 M NaCl? mol

c) How many mLs of 0.250 M AgNO3 are required to react with 50.0 mLs of 0.400 M NaCl? mLs

 

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