Final Study Guide for Test IV
CHEM 1203 – Fall, 2012
Chap. 7
Be familiar with Dalton's law of partial pressures and its applications to problems dealing with partial
pressures of gases. Understand the interchange of oxygen and carbon dioxide between blood and air in the
lungs, and between blood and the tissues. (Base your understanding on Dalton’s law of partial pressures and
on the fact that a gas flows from a region of higher partial pressure to a region of lower partial pressure. )
Chap. 8
1) Be thoroughly familiar with the two pages on “Chemistry of Solutions” in the Supplementary Notes (pages
31 and 32), except that you do not have to know the effect of temperature on solubility or the importance of
particle size. You do not have to know the definition of a “supersaturated solution”.
2) Be able to do calculations involving concentrations of solutions involving
1) Molarity calculations.
***2) Percent weight/volume (Know that percent of solute = grams of solute in 100 ml
of solution).
Kow the definitions of Molarity and Percent weight/volume (You need not know the other concentration
definitions.)
3) Know definitions of strong, weak, and nonelectrolytes; know that all ionic compounds are strong
electrolytes, and that sugars (including dextrose) are nonelectrolytes.
4) Colligative properties: Be thoroughly familiar with the contents of the page labeled “Colligative
Properties” in the Supplementary Notes (page 36), especially osmosis. Know the contents of the discussion
labeled “Osmolarity Terminology” on the class web site. (This information replaces the last two paragraphs
on page 36 of the Supplementary Notes.) Know that flow of water across an osmotic membrane is from the
hypo-osmotic solution to the hyperosmotic solution.
5) Know definition of an osmotic membrane (water can pass through but solute particles cannot).
6) Know interaction of red blood cells with hypotonic and hypertonic solutions (hemolysis and crenation).
7) Osmolarity and milliosmolarity problems for one solute. [Recall: for a one-solute solution, Osmolarity =
Molarity x (number of particles per formula unit) ]
8) Osmolarity and milliOsmolarity problems, including those based on IV solutions. This includes problems
similar to those done in class, problems similar to those in the Supplementary Notes, and problems similar to
those assigned as supplementary problems. These problems include calculations for more than one solute.
9) Calculations involving equivalents and milliequivalents, to the extent covered in class, in the
Supplementary Notes, and in the supplementary problems.
Page 2 of 2 pages
10) IV Dosage Calculation problems similar to those done in class and similar to those in the supplementary
problems. Also, know all material on the page labeled “IV Dosage Calculations” (Page 42, Supplementary
Notes).
Chap. 10 (Based primarily on the three pages in the Supplementary Notes labeled “Notes on Acids and
Bases”, pages 45-47.)
1) Know Arrhenius definitions of acids and bases. Know the strong bases and the strong acids as given in
class.
2) Know Bronsted-Lowry definitions of acids and bases.
3) Be familiar with the nature of the hydronium ion and how it is formed.
( Know that [H3O+] and [H+] are two ways of representing the same thing: the hydronium ion
concentration. )
4) Know what Bronsted-Lowry acid-base reactions are, and be able to write equations for such reactions.
5) Be able to write equilibrium expressions for weak acids (such as acetic acid) and weak bases (such as
ammonia).
6) Given an acid, be able to determine its conjugate base.
7) Given a base, be able to determine its conjugate acid.
8) Be familiar with the ionization of water, and be able to write the equation for the ionization.
Know that [H3O+] [OH-] = 1. 0 x 10-14 in all water solutions.
9) Given the [H3O+] know how to calculate the pH.
10) Given the [OH-] know how to calculate the pH.
11) Given the pH, be able to calculate the [H3O+] and the [OH-].
12) Given the [H3O+] know how to calculate the [OH-].
13) Given the [OH-] know how to calculate the [H3O+].
14) Know the characteristics of acidic, basic, and neutral solutions, in terms of pH, [H 3O+], [OH-], etc.
15) Know that the major blood buffer is (H 2CO3/HCO3-); be able to write the equilibrium expression for this
buffer.
Relevant Test Questions
Sample Test III: 1, 21, 22, 23, 25; Sample Test IV: 1-16, 20-22, 24-27