Lecture1 - Tuesday and Thursday, 11:00 12:15 Davidson Hall,...

Info iconThis preview shows pages 1–12. Sign up to view the full content.

View Full Document Right Arrow Icon
    Tuesday and Thursday, 11:00 – 12:15 Davidson Hall, Room 3
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Dr. Sungsool Wi ± Office: 3107 Hahn Hall ± Phone: 231-3329 ± Email: sungsool@vt.edu ± Office Hours: Tuesday 2:30 – 4:30 PM Thursday 2:00 – 4:00 PM by appointment ± See Blackboard for lecture stuff & assignments
Background image of page 2
Text Book ± Exploring Chemical Analysis ± 3 rd Edition ± Daniel C. Harris
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
What is Analytical Chemistry? ± It is a branch of chemical science to identify compositions, concentrations, and structures of unknown compounds or materials.
Background image of page 4
Quantification of Matters Coins, pebbles, balls, etc.: Fluids (water, gasoline, air): Grains, meats, etc.: => Weight => Volume => numbers
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Chapter 1 Chemical Measurements How do we quantify chemicals? H 2 SO 4 (l) => Volume
Background image of page 6
NaOH (s) => weight Chemical balance
Background image of page 7

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
H 2 SO 4 + 2NaOH -> Na 2 SO 4 + 2H 2 O How do you quantify chemical reactions ? Mole: Avogadro’s number (6.022 x 10 23 mol-1) of atoms, molecules or ions is defined as 1 mole Chemical Reactions => Count numbers: stoichiometry
Background image of page 8
Background image of page 9

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Carbon: 12 C 12 (exact) 98.93 13 C 13.00335 1.07 Mass number Abundance (atom %) Weight average = 12 x 0.9893 + 13.00335 x 0.0107 = 12.01
Background image of page 10
Examples: CuSO 4 •5H 2 O 126.54 g MW (FM) = Cu + S + 9O + 10H = 63.546 + 32.065 + 9 x 15.9994 + 10 x 1.00794 = 249.69 g/mol Mole of CuSO 4 •5H 2 O = = 0.50679 mol 126.54 g 249.69 gmol -1 Mole of Cu +2 = mole of SO 4 2- = mole of CuSO 4 •5H 2 O Mole of H 2 O = 5 x mole of CuSO 4 •5H 2 O
Background image of page 11

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Image of page 12
This is the end of the preview. Sign up to access the rest of the document.

Page1 / 23

Lecture1 - Tuesday and Thursday, 11:00 12:15 Davidson Hall,...

This preview shows document pages 1 - 12. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online