c1410 ob3 by 9O16ew7

VIEWS: 2 PAGES: 2

									CHEMISTRY 1410                                 BLINN COLLEGE
Joseph Kingcade                                FALL 2009

                     CHAPTER THREE

OBJECTIVE:   When you complete this unit you should be able to

    1. Balance simple chemical equations, and be able to list the
    three quantities that must be conserved in chemical reactions.
    Determine the chemical formula from elemental analysis.

    2. Express the relative amounts of reactants used and the
    quantities products produced in terms of molecules, mole and
    masses for chemical reactions.

    3. Distinguish between electrolytic and non-electrolytic and
    explain how their solutions differ. Predict the expected
    chemical species present in various simple solutions. Know the
    terms solution, concentration, solute and solvent.

    4. Relate the concentration of solute by both percent by mass
    and molarity. Be able to calculate changing concentrations upon
    dilution.

    5. Know the strong acids and bases [Table 3.2] and be able to
    write chemical equation for acid-base neutralization
    reactions.


PROBLEMS: (Q: = conceptual questions and PR: = problems)

    Objective 1 – 3.6-3.8, 3.10-3.12, 3.15-3.16, 3.27, 3.58-3.60,
    3.77-3.78, 3.96

    Objective 2 – 3.37-3.38, 3.41-3.43, 3.46-3.50, 3.53-3.55, 3.85

    Objective 3 – 3.21-3.25, 3.28-3.29, 3.36

    Objective 4 – 3.62-3.67

    Objective 5 – 3.32-3.36, 3.84
CHEMISTRY 1401                                 BLINN COLLEGE
Joseph Kingcade                                FALL 2009

            CHAPTER THREE – REVIEW PROBLEMS

1. What   are the formula weights for the following compounds?
     a)   Ammonium tetraborate: (NH4)2B4O7
     b)   magnesium phosphate: Mg3(PO4)2
     c)   Calcium cyclamate: Ca(C6H12NSO3)2

2. What is the relationship between formula weight and molar mass?

3. A sample of iron contains 12.04 x 1023 atoms:
     a) How many moles does the sample contain?
     b) What is the mass of the sample: in grams, in kilograms?

4. How many moles of sodium nitrate are in 1.80 g of sodium nitrate?

5. Calculate the percentage of nitrogen in urea, CO(NH4)2 .

6. Balance the following equations:
     a) Fe2O3 + H2 → Fe + H2O
     b) Na2CO3 + Mg(NO3)2 → MgCO3 + NaNO3

7. In what way is the concept of concentration different from that
of solubility?

8. Calculate the number of grams of each solute that has to be taken
to make each of the following solutions:
     a) 250 ml of 0.100M NaCl
     b) 500 ml of 0.500 M H2SO4
     c) 100 ml of 0.250 M Na2CO3

9. Concentrated ammonia contains 26.0 g soluute per 100 ml of
solution. What is its molarity?

10. Concentrated acetic acid is 17.4 M HC2H3O2. How many ml would one
need to prepare 1.00 L of 1.00M acetic acid?

11. If 150 ml of water is added to 100 ml of 0.15 M Na2CO3
, what is the final molar concentration of Na2CO3 ?

12. Write the dissolving equation for (NH4)2SO4 and for Na3PO4.

13. Write the net ionic equation for the release of hydrogen gas by
the reaction between Zn(s) and sulfuric acid
                  Zn(s) + H2SO4(aq) → H2(g) + ZnSO4(aq)

								
To top