1. Chapter 1 Chemical Measurements

2. Overview 1-1 SI Units 1-2 Chemical Concentrations
1-3 Preparing Solutions
1-4 Stoichiometry Calculations for Gravimetric Analysis

3. SI Units SI base units include the following: meter (m) kilogram (kg)
second (s)
ampere (A)
kelvin (K)
mole (mol)

4. Derived SI Units
Other quantities can be derived in terms of base SI units. See Table 1-2.
force (newton, N), Kg∙m / s2
pressure (pascal, Pa), N / m2
energy (joule, J), N∙m

5. Prefixes
Table 1.3
Memorize these prefixes with their abbreviations and powers of ten.

6. Using Prefixes in Calculations
In calculations, units should be carried along with the numbers.
Prefixes such as kilo- and milli- are used to denote multiples of units.
Prefixes can be used to simplify conversions between units.
Example:
Express 19.3 mPa in terms of atm
19.3 mPa can be written as 19.3  10-3 Pa

7. Unit Conversions
The calorie content of a candy bar is 230 calories per serving (1 bar).
Calculate the specific energy (kJ/g) of the candy bar.
(1 candy bar = 52.7 g, 1 calorie = J)

8. Concentrations Molarity (moles of solute per liter of solution), M
Molality (moles of solute per kilogram of solvent), m
Formal concentration (formula units per liter), F
Percent composition (w/w, v/v or w/v), %
Parts per million, ppm
Parts per billion, ppb

9. % Composition (w/w or v/v)
95% (w/w) ethanol contains 95 g of ethanol for every 100 g of solution.

10. ppm, Parts per Million
Shortcut: ppm is also mg/L or µg/mL if the density of the solution is 1.0 g/mL.
An aqueous solution that is 1000 ppm in Cu contains mg Cu per liter of solution.
It also contains 1000 µg per mL of solution.

11. Chemical Concentratons
The maximum contaminant level for arsenic is ppm for drinking water per EPA regulation. The arsenic concentration for the drinking water of a municipality was measured to be 4.92  10−6 M arsenic. What is the arsenic concentration of the water sample in ppm? Does the water sample meet EPA guidelines? Assume the drinking water sample has a density of g/mL.

12. Making Solutions
How many moles of CuCl2∙5H2O are needed to make 500 mL of a solution that is 1,000.0 ppm in Cu?
grams of CuCl2∙5H2O?
milliliters of 10,000 ppm CuCl2∙5H2O solution?
Figure 1-4

13. Making Solutions
To calculate quantities of reagents needed to prepare solutions, use the relation
(Mconc)(Vconc) = (Mdil)(Vdil)
Equates moles of reagent removed from a stock solution to moles delivered into a new solution.

14. Preparing Solutions
Calculate the mass of Na2CO3 needed to prepare a mM solution with a volume of mL. (Na2CO3 = g/mol)

15. Preparing Solutions
What volume of 12.1 M HCl must be diluted to prepare a M HCl solution with a volume of L?

16. Preparing Solutions
What volume of a 50.0% by mass NaOH solution must be diluted to prepare a M NaOH solution with a volume of 500 mL? The density of 50% NaOH solution is g/mL at 25°C. (NaOH = g/mol)

17. Stoichiometry
Use stoichiometry relationships to calculate required masses or volumes of reagents for chemical reactions.
From the mass of product of a reaction, you should be able to compute how much reactant was consumed.

18. Stoichiometry
The recommended daily allowance of calcium for men between the ages of 19 to 50 is 1000 mg Ca. Three multivitamin tablets are analyzed for calcium gravimetrically with the precipitation of calcium cation by oxalate anion. If the mass of dry calcium oxalate obtained is g, how many tablets must a man take in a given day to meet the recommended daily allowance? Ca2+ (aq) + C2O42− (aq)  CaC2O4 (s)

19. Stoichiometry
The sulfur content of an ore is determined gravimetrically by reacting the ore with concentrated nitric acid and potassium chlorate, converting all sulfur to sulfate. The excess nitrate and chlorate is removed by reaction with concentrated hydrochloric acid and the sulfate is precipitated using barium cation. Ba2+ (aq) + SO42- (aq)  BaSO4 (s) Analysis of grams of a sulfur containing ore yielded grams of BaSO4. What is the percent by mass sulfur in the ore? (BaSO4 = g/mol)

20. Limiting Reagent
The limiting reagent in a chemical reaction is the one that is consumed first.
Once the limiting reagent is gone, the reaction ceases.
Example: For the reaction: A + 2B  P
0.751 moles of A are mixed with 1.43 moles of B.
What is the limiting reagent and how much excess reagent remains unreacted?

21. Limiting Reactant
Aqueous lead precipitates when mixed with aqueous carbonate. Pb2+ (aq) + CO32− (aq)  PbCO3 (s) If g Pb(NO3)2 and g Na2CO3 are mixed in water, which ion is the limiting reactant? What mass PbCO3 is precipitated? (PbCO3 = g/mol, Pb(NO3)2 = g/mol, Na2CO3 = g/mol)

22. END