1. CHE 1316 Laboratory Measurements & Techniques
Dr. Kevin Chambliss
Dr. David Young
LECTURE (BSB D109)
Monday 12:00-12:50 (sections 1-6)
Wednesday 12:00-12:50 (sections 7-12)
PRE-LAB LECTURE (BSB C105)
M,W 2:00-5:00 (sections 1-3)
T,R 2:00-5:00 (sections 4-6)
T,R 8:00-11:00 (sections 7-9)
T,R 11:00-2:00 (sections 9-12)

2. Required Items Lab Manual Lab Notebook Safety Goggles
Scientific Calculator
Comet or other Cleanser
Marking Pen
Textbook:
USE YOUR CHE 1301/1302 TEXT!!!

3. Objectives
Develop laboratory techniques and skills necessary for making accurate measurements.
Learn basic theory behind. procedures and calculation of results.
Learn to organize laboratory time.
Learn record keeping skills.
Observe chemistry discussed in CHE1301 and CHE1302.

4. Getting Help Classmates Laboratory Assistants Office Hours (BSB E114)
TBA

5. What is Analytical Chemistry?
the art of recognizing different substances and determining their constituents. – Friedrich Wilhelm Ostwald, winner of the Nobel Prize in chemistry (1894)
a measurement science consisting of a set of powerful ideas and methods that are useful in all fields of science and medicine.
Analytical Chemistry
Qualitative Analysis
Quantitative Analysis
IDENTITY
AMOUNT

6. Types of Quantitative Analyses
Two measurements required to calculate the result of a quantitative analysis.
Determination of the mass or volume of the sample to be analyzed.
Determination of property “X” that is proportional to the amount of analyte in the sample.
Volumetric – volume of solution containing sufficient reagent to react completely with analyte.
Gravimetric – mass of analyte or some chemically related compound.
Spectroscopic – based on the interaction of electromagnetic radiation with analyte.
Electroanalytical – voltage, current, resistance, or charge.
Miscellaneous – mass-to-charge ratio, radioactive decay, heat of reaction, rate, thermal conductivity, optical activity, or refractive index.

7. Eliminate Interferences
Select Method
Steps in a Quantitative
Analysis
Acquire Sample
Process Sample
Soluble? No
Chemical Dissolution
Yes
Measurable
property?
Change Chemical
Form No
Estimate
Reliability
Yes
Eliminate Interferences
Measure
Property X
Calculate
Results

8. Reaction Requirements
Must go to completion
NaOH + HCl  NaCl + H2O
AgNO3 + NaCl → AgCl(s) + NaNO3
Must have known stoichiometry
Na2CO3 + HCl  NaHCO3 + NaCl
Na2CO HCl → 2 NaCl + CO2 + H2O

9. Units of Measurement Mass (weight): Volume: gram = g liter = L (dm3)
“milli” = one thousandth
mg = mass in g x 1000
g = mg
1000 mg = g
Volume:
liter = L (dm3)
milliliter = mL (cm3)

10. Units of Measurement Amount of Substance: Concentration:
Mole = amount of substance which contains as many elementary particles as there are atoms in kg of 12C.
6.02 × 1023 atoms, molecules, ions
molar mass = g/mol = mg/mmol
Concentration:
Amount (weight, moles, equivalents, etc.) of SOLUTE in a given amount (volume or weight) of SOLUTION.

11. Units of Measurement Molar Concentrations: mol solute L soln.
mmol solute
mL soln. =
Percent Concentrations: (applies to both solutions AND SOLIDS!!!)
Wt% (w/w) =
weight solute
weight soln.
x 100% (e.g., 70% HNO3, conc.)
Vol% (v/v) =
volume solute
volume soln.
x 100% (e.g., 5% methanol)
%Wt/Vol (w/v) =
weight solute, g
volume soln., mL
x 100% (e.g., 5% AgNO3)
Molarity = M =
mM =

12. Units of Measurement Very Low Concentrations p-Function
Negative base 10 logarithm of molar concentration. pX = −log [X]
pH = log [H3O+]
pAg = log [Ag+]
Wt component
Sample Wt
mg solute
L solution
parts per million =
x 106 ppm 
mg solute
L solution
Wt component
Sample Wt
parts per billion =
x 109 ppb 
(approximation assumes density of soln. = 1.0 g/mL)

13. Solution Stoichiometry
Na2CO3(aq) AgNO3(aq)
Ag2CO3(s) NaNO3(aq)
What mass of AgNO3 is needed to convert 2.33 g Na2CO3 to Ag2CO3?
mass
Na2CO3
mol
Na2CO3
mol
AgNO3
mass
AgNO3
Divide by
molar mass
of Na2CO3
Multiply by
stoichiometric
factor
Multiply by
molar mass
of AgNO3
1 mol Na2CO3
106.0 g Na2CO3
2 mol AgNO3
1 mol Na2CO3
169.9 g AgNO3
1 mol AgNO3
2.33 g Na2CO3 × × ×
= g AgNO3 → g (3 significant figures)

14. Chemistry. The Central Science
REVIEW ASSIGNMENT!!!
General Chemistry OR
Chemistry. The Central Science
Chapter 1: Sections
(Sections in Brown, Lemay,…)
Chapter 2: Sections
Chapter 3: ALL
Chapter 4: ALL