Name_________________________
Mr. Taylor-Waldman
Review Sheet for Chapter 3 Test: Acids, Bases and Solutions – Test is Monday, May 4
Chapter 2, Section 2 – Describing Chemical Reactions
Terms:
chemical equation
an easy way to show a chemical reaction using
_________________ instead of words
reactant
the substances that you have at the beginning of a chemical
reaction, on the left side
product
the substances produced in a chemical reaction, on the right
synthesis
a reaction where two reactants yield ______product. A + B  C
decomposition
a reaction where one reactant yields two products. __________
replacement
a reaction where two products split and reform two new
products. AB + CD  AC +BD
Concepts: 1. Chemical equations must be “balanced” and have same number and type of atoms
on both sides of the equation.
Chapter 3, Section 1 – Understanding Solutions
Terms
solution: a well-mixed, _________________ mixture, made up of a solute and ______________,
solute: the smaller part of a solution; it is what gets dissolved into a solvent (sugar in the soda)
solvent: is the larger part of a solution; it dissolves the solute (water in the soda).
suspension: a ________________ mixture in which the particles are large enough to be seen,
and can be removed by ________________________
colloid: a ________________ mixture that contains small, undissolved particles that do not
settle out; some colloids can also scatter light
Concepts
1. Solutes lower the freezing point and _____________________ the boiling point of solvents.
Chapter 3, Section 2 – Concentration and Solubility
Terms
concentration: a measurement comparing the amount of solute to the amount of solvent
dilute solution: a mixture that has a ______________ ratio of solute to solvent
concentrated solution: a mixture that has a ______________ ratio of solute to solvent
saturated solution: a solution that has so much solute that ____________________________
unsaturated solution: a solution that can still dissolve more solute
supersaturated solution: a solution with more dissolved solute than is predicted by its
________________________ at a given temperature
solubility: the measure of how much solute can dissolve in a solvent ______________________
Concepts
1. Know how the factors of pressure, solvent type, and temperature affect solubility.
3. Know how to read solubility graphs, and how to make a statement of solubility.
Chapter 3, Section 3 – Describing Acids and Bases
Terms
indicator: a compound (such as litmus paper of pH paper) that ____________________ when it
comes into contact with an acid or a base
corrosive: a property of acids; a substance’s ability to eat away metals
Concepts
1. Know the properties of acids and bases, the chemical formulas of common acids and bases,
their uses, and where they are found.
Chapter 3, Section 4 – Acids and Bases in Solution
Terms
hydrogen ion (H+): a hydrogen atom that lost its electron, giving it a
________________________
hydroxide ion (OH-): a polyatomic ion made up of oxygen and hydrogen, carrying a - charge
neutralization: a reaction between an acid and base yielding a solution that
________________________than the starting solutions
Concepts
1. Acids produce ___________ and bases produce ___________ ions.
2. Know how the pH scale works, what it measures, and what determines whether and acid or
base is strong or weak.
3. The pH scale measure the concentration of hydrogen ions
4. _______ paper is more accurate than _______ paper at describing acid/base strength.
**Additional Concepts to Know**
1. Observing Chemical Change Lab
2. pH paper and Litmus paper homework
Review Questions
1. Distinguish between reactants and products in a chemical reaction.
2. According to the principle of conservation of mass, what must be true in all chemical
reactions?
3. What are two different examples of evidence that a chemical reaction has occurred?
4. Describe the part of our “Observing Chemical Reactions” Lab that can be represented by the
following chemical equation: NaCl (aq) + AgNO3 (aq) → AgCl (s) + NaNO3 (aq)? What kind of
substance was formed by this reaction? What is the name of this compound? Classify this type
of reaction.
5. Using a balanced chemical equation, represent the chemical reaction of magnesium
combustion that we observed in our lab. What type of chemical equation is this?
6. Which experiment in our “Observing Chemical Reactions” Lab that can be represented by this
chemical equation: ___Al(s) + ___NaOH(aq) → ___H2(g) + ___Na3Al2O3(aq)? Which
substance in this experiment is a strong base?
7. Balance the following equations, and classify each reaction as either synthesis,
decomposition, single or double replacement.
____ Fe + ____ O2 → ____ Fe2O3
____ P4 + ____ O2 → ____ P2O5
____ NaCl + ____ F2 → ____ NaF + ____ Cl2
____ C3H8 + ____ O2 → ____ CO2 + ____ H2O
____ NaHCO3 → ____ Na2CO3 + ____ H2O + ____ CO2
____ Cu + ____ HNO3 → ____ Cu(NO3)2 + ____ NO + ____ H2O **extra challenging**
8. Give one example each of a solution, colloid and a suspension, and classify each as
homogeneous or heterogeneous mixture.
9. How could you make a solution of lemonade (made with powder mix) more diluted? More
concentrated? Increase its solubility?
10. What is an unsaturated solution? Saturated Solution? Supersaturated solution?
11. What property of solutions is calculated by comparing the amount of solute to the amount
of solvent?
12. What two indicators can be used to test a substance’s pH? Which indicator is more precise?
13. How much potassium nitrate can be
dissolved into 100 ml of water at 50°C?
14. Describe the solubility of hydrogen
chloride at 20°C.
15. Can you dissolve 50 grams of sodium
chloride into 100 ml of water at 30°C?
How could you increase its solubility?
16. At what temperature can you dissolve exactly 105 grams of sodium nitrate into 100 ml of
water?
17. Describe the difference between an acid and base in terms of the ions they form in water.
18. Describe the reaction of mixing a base with an acid. What is this called, and what products
are formed?
19. How do solutes affect the freezing and boiling points of solvents?
20. What is an example of an acid, including chemical formula? Base, including chemical
formula?
21. How would you describe a solution with a pH of 2? pH of 8? What pH is neutral?