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4.10.a Aqueous Equilibria Worked Example

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高级化学

肯塔基大学

4.7（430 个评分） | 51K 名学生已注册

A chemistry course to cover selected topics covered in advanced high school chemistry courses, correlating to the standard topics as established by the American Chemical Society. Prerequisites: Students should have a background in basic chemistry including nomenclature, reactions, stoichiometry, molarity and thermochemistry.

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审阅

4.7（430 个评分）

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KO

Jul 17, 2017

Excellent content and delivery!\n\nThis course has many well-explained examples and practice questions to reinforce the understanding of the taught concepts. Thank you!

CW

Sep 17, 2015

I used this course as a significant portion of my preparation for the CLEP Chemistry exam, and passed today with an A! Thank you!

从本节课中

Aqueous Equilibria

This unit continues and expands on the theme of equlibria. You will examine buffers, acid/base titrations and the equilibria of insoluble salts.

4.01 Buffers and the Common Ion Effect10:01

4.02 pH of Buffer Solutions14:04

4.02a Aqueous Equilibria Worked Example 13:58

4.03 Buffer Action25:21

4.03a Aqueous Equilibria Worked Example 25:22

4.03b Aqueous Equilibria Worked Example 35:11

4.04 Buffer: Preparation and Capacity8:45

4.05 Strong Acid - Strong Base Titration17:20

4.06 Titrations Involving Either a Weak Acid or a Weak Base36:45

4.06 Part 1 Aqueous Equilibria Worked Example3:46

4.06 Part 1.a - Aqueous Equilibria Worked Example4:06

4.06 Part 1.b - Aqueous Equilibria Worked Example4:55

4.06 Part 1.c - Aqueous Equilibria Worked Example4:21

4.06 Part 1.f Aqueous Equilibria Worked Example8:01

4.06 Part 1.h Aqueous Equilibria Worked Example3:57

4.06 Part 2.a Aqueous Equilibria Worked Example8:25

4.06 Part 2.b Aqueous Equilibria Worked Example5:53

4.07 Polyprotic Acid Titrations5:53

4.08 Indicators10:19

4.09 Solubility Equilibria4:50

4.10 Molar Solubility and the Solubility Product10:37

4.10.a Aqueous Equilibria Worked Example2:20

4.11 Molar Solubility and the Common Ion Effect7:20

4.11 2.b - Aqueous Equilibria Worked Example4:42

4.11 2.c Aqueous Equilibria Worked Example3:45

4.12 The Effect of pH on Solubility7:07

4.12.b Aqueous Equilibria Worked Example3:42

4.12c Aqueous Equilibria Worked Example3:30

4.13 Precipitation Reaction and Selective Precipitation15:03

4.13a Aqueous Equilibria Worked Example9:05

教学方

Dr. Allison Soult
Lecturer
Dr. Kim Woodrum
Sr. Lecturer

脚本

We're going to work through this problem as three separate problems. The first one is to calculate the molar solubility of the silver chromate in pure water. So we will begin for each of these parts by writing the reaction of the dissolution of the solid. So there's a silver chromate. It will dissolve to produce 2 silver plus ions and a chromate ion. So we can set up an ICE table. We will place some of the solid, doesn't matter how much, some of the solid into the solution, into the water, and we will have no silver and no chromate present before the reaction happens. As it dissolves, we will subtract S, that is, the molar solubility. How much of the silver chromate would dissolve, and we would produce 2S here and s here. Giving me still some of the solid sitting in the bottom of the beaker. 2S and S. Write the KSP expression for the reaction you see above, so it's silver concentration squared, because it has a 2 coefficient, times a chromate concentration. And then we'll plug in the values that we know. 1.12 x 10 to the -12 is the KSP, and that's going to be equal for the silver concentration we have 2S, that's 2S, and that will be squared, plus the S for the chromate. This will give me 1.12 x 10 to the -12 = 4S cubed. So we squared the 2, we squared the S, now we can multiply that S squared with that other S and that's our values. Now, to obtain our value for S we have to divide both sides by 4. And then take the cube root of both sides, okay? So we're going to take the cube root. And that will leave us with S. And S = 6.54 x 10 to the minus 5, and since it's molar solubility that we're obtaining, we'll put an M for molarity.

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