Guidelines for Study

Reading Chemistry

Pre-Reading
* Prior to lecture quickly pre-read the chapter.  This gives you a preview of the information that the instructor will be lecturing on.
	— Pay attention to topic headings, bold words, example problems, and the chapter summary.  
	— Skim through the assigned problems at the end of the chapter.  This provides a clue about what the instructor thinks are the important sections of the chapter.

Reading The Text	
*  After you have pre-read the chapter, it is time to go back and do a thorough job.  Some people find it more effective to pre-read the chapter prior to lecture and then thoroughly read the chapter after lecture. 
	— Your goal is to understand the material.
	— Pay close attention to any definitions and equations.  
	— Make use of the graphs and tables provided by the author since they give you a visual representation of the concept being studied.  
	— Work through the practice problems.  This will test whether you understand the material or not.  
*  After you are done reading the chapter, tackle the assigned problems at the end of the chapter.  Don’t get frustrated if you cannot work through all of them the first time.  Chemistry problems are not easy and often take multiple attempts to solve.  Use the answer manual as a tool for helping you get out of the area that you are stuck.  The correct answer is not as important as understanding the steps taken to solve a problem.

Solving Chemistry Problems
	
	Working through the assigned problems is the only way to ensure that you understand the material being presented in the chapter.  Chemistry problems are often difficult, so do not be afraid to ask for help (from a friend, professor, or tutor) if you are having difficulties.

Approaching the Problem	
	*  Skim the problem — what are you being asked?
	*  Read the problem again paying close attention to what information they provide.    
    As you do this, try to remember what the question is.
	* Write down the information given to you.  Write down
	    the units (they will give you clues about how to solve the
	    problem.)
	*  Look at what you are given — what information do you
	    need to solve the problem.  What equations could you
	    use?  Try to make a flow chart on how you’re going to
	    find the answer.

	EX.  	All the silver in a 45.0ml portion of silver nitrate
	         solution is precipitated as silver iodide by 26.0ml of a
	         0.250M calcium iodide solution:
			2AgNO3  +  CaI2  ®2AgI  +  Ca(NO3)2
		Calculate the molarity of the silver nitrate solution.

	1)	Quickly read the problem.  What are you being asked?
			— To find the molarity of AgNO3

	2)  	Read the question again.  What type of information are
	         you given?  What are you trying to solve?
			— To find the molarity of AgNO3 you need the # of
	         moles of AgNO3 and the volume of AgNO3.  You are
	         given an equation (always check to make sure it’s
	         balanced), the volume and molarity of CaI2, and the
	         volume of AgNO3.  Remember we want to find the 
		molarity of AgNO3.  

	3) 	Write down the information that you are given.
		Equation:  2AgNO3  +  CaI2  ®  2AgI  +  Ca(NO3)2
		CaI2:  0.250 mol  ,  26.0ml                AgNO3:  45.0ml
			             L

4)  	What do you still need to solve the problem?
		— You want to find the molarity of AgNO3.  The
		units of molarity are moles.  Look at the information 				   		          			        L
		you wrote down.  They gave you the volume of AgNO3
		but not how many moles there are.  This is what you
		have to find.  Look at the information again.  Try to
		make a flow chart on how you are going to find moles
		of AgNO3.

volume CaI2®moles CaI2(using molarity)®moles AgNO3 (using balanced
										     equation)
					molarity of AgNO3 in problem	      ¿					   					(using given volume)

26.0 ml CaI2  x    L      x    0.250 mol CaI2    x    2 mol AgNO3 =    0.013 mol AgNO3
                                1000ml                   L                                1molCaI2

                               Molarity of AgNO3  =  0.013 mol AgNO3  =     0.289M AgNO3
                                                        0.045 L AgNO3

*Remember to pay attention to units.

Don’t forget to consider your resources; go see your instructor or consult with an understanding/experienced peer tutor in the Academic Assistance Center.  Do not be afraid to ask for help from a friend, professor or peer tutor if you are having difficulties.

Academic Assistance 
Library 124  x7518

This handout provided as a service of Academic Assistance. Library 124 Ext 7518.

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