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Quantitative Analysis Test 2 Study Guide

by: Grace Ford

Quantitative Analysis Test 2 Study Guide CH 223-01

Marketplace > University of Alabama - Huntsville > Chemistry > CH 223-01 > Quantitative Analysis Test 2 Study Guide
Grace Ford
GPA 3.2

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About this Document

Covers Chapters 7-10
Quantitative Analysis
Dr. George
Study Guide
50 ?




Popular in Quantitative Analysis

Popular in Chemistry

This 2 page Study Guide was uploaded by Grace Ford on Saturday October 15, 2016. The Study Guide belongs to CH 223-01 at University of Alabama - Huntsville taught by Dr. George in Fall 2016. Since its upload, it has received 12 views. For similar materials see Quantitative Analysis in Chemistry at University of Alabama - Huntsville.


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Date Created: 10/15/16
Quantitative Analysis Test 2 Chapters 7-10 Chapter 7: Precipitation Titrations: - Pm=-log[M+] - Use the equation and given concentrations to determine points for the titration curve - Curve is graphed with concentrations on the x axis and the calculated pm on the y axis Chapter 8: Ionic Equilibria - When ions interact, the cations get surrounded by anions, forming a cloud (the ionic atmosphere) around the central ion - Ions continuously diffuse into and out of the atmosphere, so the net charge on the atmosphere is less than the charge on the cation/anion at the center - This lessens the attraction between cation and anion because they are shielded by their individual atmospheres - Ionic strength: o ???? = 1∑ ????????????????2 2 - Activity coeffecients o ???????? = [????]???? ???? - Systematic treatment of equilibrium: o Write pertinent reactions o Write charge balance reactins o Write mass balance reactions o Write equilibrium equations for each reaction o Count the number of equations and unknowns (they must be equal) o Solve for all unknowns Quantitative Analysis Test 2 Chapters 7-10 Chapter 9: Acids and Bases - pH=-log[H+] ????+ [????−] - ???? ???? [????????] - Fraction of dissociation: ???? = [????−] [????− [????????] [????????+] - Fraction of association: ???? = [????????+ [????] - Henderson-Hasselbalch: pH=pKa+log([A-]/[HA]) Chapter 10: Polyprotic Acids and Bases - Polyprotic acids and bases can give or receive multiple protons, making them amphoteric, so in calculating pH it is necessary to account for the extra protons - Results in three chemical equations: o The first is treated as a monoprotic substance ???? ???? ????+???? ???? o The second, the intermediate, requires the formula [????+] = √ 1 2 1 ???? ????1+[????????] o The third requires the formula Kb=Kw/Ka - Triprotic acids and bases are solved the same way, with an extra intermediate form


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