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UGA / Engineering / CHEM 1212 / is agoh soluble

is agoh soluble

is agoh soluble


School: University of Georgia
Department: Engineering
Course: Freshman Chemistry II
Professor: Suzanne ellenberger
Term: Spring 2017
Tags: General Chemistry
Cost: 50
Name: CHEM 1212 exam 4 study guide
Description: This study guide has problems from lecture that should be covered on the exam.
Uploaded: 04/14/2017
4 Pages 129 Views 0 Unlocks

what is the Δ G ° for the dissolution of OH ¿2 ?

7KJ /mol∗K , what is the Δ G value at 25 °C?

What is the molar solubility of CuCl in pure water?

Exam 4 Study Guide Chapters 18,19, and 20 These are problems from lecture: Which of these compounds is more soluble,  OH ¿2 Mg ¿or  AgOH ? OH ¿2:Ksp=1.5e−11 Mg¿ AgOH :Ksp=2.0e−8 (substitute elements with X) OH ¿2 Mg ¿:  2 X ¿2=4 X3=1.5e−11 X ¿ OH ¿2 ¿ X=  OH ¿2 1mol Mg(¿) 58.31968 gMg¿ ¿ 1.55 e−4mol/ L ¿ = 0.00906We also discuss several other topics like conjugadion
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 g/L AgOH : X2=2.0e−8mol/ L X=1.414 e−4 mol/L(124.8756 g AgOH 1mol AgOH)=0.0177 g /L AgOH is more soluble What is the molar solubility of CuCl in pure water? Ksp :1.9e−7 Molar solubility =  √❑ =  √❑ M What is the pH of a concentrated  OH ¿2 Ca ¿solution?  Ksp=5.5e−52 X ¿2=5.5e−5 OH ¿2: X ¿ Ca¿ X=0.023996 [OH ]=2 X=0.04792 M pOH =  −log(0.04792)=1.319 pH=14−pOH=12.68 A solution contains  1.06 e−2 M lead(II) acetate and  1.35 e−2 M silver nitrate.  Solid sodium sulfate is added slowly. Which compound will precipitate first?  (the compound with the lowest amount of sulfate will precipitate first) KspPbSO4=1.8e−8 Ksp Ag2 SO4=1.7e−5 2+¿ 2−¿ S O4¿ P b¿¿ PbS O4:Ksp=¿ 2−¿ SO4¿ 1.8e−8=(1.06 e−2)¿ 2−¿ S O4¿=1.698 e−6 ¿+¿ 2−¿ SO4¿ A g¿¿ Ag2S O4:Ksp=¿ 2−¿ SO4¿ 1.7e−5=(1.35 e−2)¿ 2−¿ S O4¿=1.259 e−3 ¿ PbS O4 will precipitate first.If  Δ H f=−74.86KJ /mol and  Δ Srxn=−80.7KJ /mol∗K , what is the  Δ G value at 25 °C? Δ G=Δ H−T Δ S −80.7 KJ /mol∗¿=−50.8 KJ /mol ΔG=−74.86 KJ /mol−(298 K)¿ The reaction is not spontaneous. CO+12O2→C O2 Calculate  Δ G at 25 °C Δ H and  Δ S of the reaction. CO: Δ H f=−11.5 KJ /mol ,Δ S=197.7 J /mol∗K O2:Δ H f=0KJ /mol , ΔS=205.1 J / mol∗K C O2: Δ H f=−393.5 KJ /mol ,Δ S=213.7 J /mol∗K Δ Hrxn=[−393.5]−[12(0)+(−11.5)]=−283KJ /mol Δ Srxn=[213.7]−[12(205.1)+197.7]=86.55 J /mol=0.08655KJ /mol Δ G=Δ H−T Δ S Δ G=−283 KJ /mol−(298 K)(0.08655KJ /mol)=−257.2KJ /mol Ksp for  OH ¿2=5.0e−6 Ca ¿.  what is the  Δ G ° for the dissolution of  OH ¿2 ? Ca ¿ Δ G °=−RTlnKsp R=8.31 J /mol∗K Δ G °=−(0.00831KJ /mol∗K)(298K)(ln 5.0 e−6)=30.24 KJ /mol The pH of a 0.1000 M monoprotic weak acid is 3.276 at 25 °C.  Determine Gibbs free  energy change in KJ/mol. +¿ H3O¿=10−pH=1 0−3.276=0.0005297 M ¿(set up and ice table) +¿ −¿ A¿ ¿ 0.0005297 M ¿2 ¿¿ H3O¿¿ ¿ Ka=¿ Δ G=−RTln Ka Δ G=−(0.00831KJ /mol∗K)(298K)(ln 2.805 e−6)=31.7KJ /mol Steps to balancing Redox reactions in acidic solutions: 1. Balance all atoms except O and H 2. Balance O by adding  H2O 3. Balance H by adding +¿H¿ 4. Balance charges by adding electrons 5. Make sure electrons gained = electrons lost Steps to balancing Redox reactions in basic solutions: 1. Balance all atoms except O and H 2. Balance O by adding H2O 3. Balance H by adding  +¿H¿ 4. Balance  +¿H¿ by adding  −¿ O H¿ to both sides 5. Balance charges by adding electrons 6. Make sure electrons gained = electrons lost

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