Chemistry 130-Final Study Guide

Chemistry 130 with Barnes at University of Tennessee - Knoxville

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By: Sophie @Studyblue
Created: 2011-04-22
Size: 93 flashcards
Views: 1824

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Addition of Solute to Solution _____ Vapor Pressure

Lowers

Addition of Solute to Solution _____ Freezing Point

Lowers

Addition of Solute to Solution _____ Boiling Point

Raises

Addition of Solute to Solution _____Osmotic Pressure

Raises

T or F: colligative properties are effected by the type of solute added to solution

False: colligative properties are quantitative

In the "Molar Mass of a Solid" lab what was used as a solvent?

Cyclohexane (unknown solute)

Solution A in Vitamin C clock experiment

Vitamin C, Iodine, Water

Solution B in Vitamin C clock experiment

H2O2 (peroxide), Starch, Water

Dynamic Equilibrium

rate that products become reactants and vice versa

Common-Ion Effect

the effect of adding an ion common to the system

Ligand

Lewis Base that donates a lone pair of e- to a metal ion

purpose of Conc NH3 in LeChateliers Buffers Lab

initiates color change (reaction)

H+ + OH- yields ______

salt and H2O

Spectator Ions

Cations or Anions that have no effect on pH

Anhydrous Salt

A salt having no hydrated water molecules in its solid structure

Slaking

Covering CaO with H2O

CaO + H2O yields Ca(2+) + 2OH-

Mg(OH)2

Milk of Magnesia

Anhydrous form of Washing Soda

Na2CO3

3 Bases of Portland Cement

CaO, K2O, Na2O

Test for presence of Ammonia

NH4Cl + Ca(OH)2 + heat yields NH3 + H2O + CaCl2

What three things will happen if excess solid material is added to a supernatant?

1) more acid needed to titrate

2) solubility product will increase

3) Molar Solubility will increase

Anions I

Insoluble Barium salts

(SO₄^2-)(PO₄^3-)(CO₃^2-)

Anions II

Insoluble Silver Salts in a dilute Nitric Acid soluton

(Cl-)(I-)(S^2-)

Anions III

Soluble anions

(NO₃^-)

Sulfate

all sulfates are soluble except strontium, barium, mercury, and lead

Phosphate

all phosphates are insoluble except group 1a cations and ammonium

Carbonate

all carbonates are insoluble except group 1a cations and ammonium

Sulfides

exists only in basic solutions

most are insoluble

if Cu(2+) is added, black precipitate forms

Halides

All salts of chloride, bromide, and iodide are soluble other than Ag+, Pb(2+), and Hg2(2+) halides

What method is used to identify nitrates?

Brown Ring test

(H2SO4)

Units of Specific Heat? (c)

Joules/(grams*degree celsius)

delta H_s=

-(heat change of H2O)+(heat change of salt)

If heat is lost to the Calorimeter...

reported delta Hn will be lower than the actual value

ClO2(-) yields ClO3(-)

oxidized

(+3 to +5)

Oxidation occurs at the ____

anode (-)

Reduction occurs at the ____

Cathode (+)

Cations flow toward the_____

Cathode [HNO3]

e- flow from _____ to _______

anode to cathode

Ecell =

E(reduction) - E(oxidation)

E(cathode) - E(anode)

metastable

releases gamma particles

(small margin of stability)

Coordination Compound is K₄[Fe(CN)₆]

a) number and type of ligands

6 CN-

Coordination Compound is K₄[Fe(CN)₆]

b) coordination sphere

Fe(CN)₆

Coordination Compound is K₄[Fe(CN)₆]

c) complex

[Fe(CN)₆]^4-

approx volume of a 75mm test tube

3 mL

small volumes of reagents added using

pipet

1 mL = ____ drops

How long should you centrifuge?

20-40 seconds

On a flow diagram what does || mean?

presence of a precipitate

On a flow diagram what does _______ mean?

separation of a precipitate from solution

On a flow diagram a box means

confirms presence of an ion

on a flow diagram = means

soluble ions in solution

What is the meaning of [ ] around a reagent?

reagent written in molecular form

The only two anions confirmed by the presence of a white precipitate

BaSO4 and CaCO3

Info about the test (per Dr. Green)

Probably about 5 pts from final lecture material
95 pts from old quizzes about 13-14 pts per quiz (probably 2-4 questions)

Per Dustin

Same format as quizzes
No True and False but know the concepts that were presented in T &F questions

Quiz 1 -Chapter 12

Molarity (M)= moles solute/ liters solution
Molality (m)= moles solute/ kg solvent
Colligative properties- physical properties that depend on the # of particles, not the type of particles
Calculate boiling point elevation and freezing point depression

Molarity (M)

moles solute/ liters solution

Quiz 2- Chapter 13

Know 0 order and 1 st order rate laws (S is always to the -1 exponent!)
Rate = -1/a([A]/t) = -1/c([C]/t), for the reaction aA cC
Integrated rate law (same as what we did in ch 19 but k is )
AM quiz 2 #3, PM quiz 2 #3: Use the balanced equation and the data to answer the following questions

Molality (m)= moles solute/ kg solvent

To go between the two you must know: 1) the density of the solvent to get volume of solvent and 2) the volume of the solute and solvent to get total volume of the solution

Molality (m)

moles solute/ kg solvent

Calculate boiling point elevation and freezing point depression

T f = T f(solution)
T b = T b(solution) ? T b(solvent) = k b x m

T f = T f(solution)

T f(solvent) = -k f x m

Integrated rate law (same as what we did in ch 19 but k is )

Ln([N t ]/[N 0 ]) = -kt

What is the order of fluorine in the rate law equation of this reaction

0 order

What is the overall order of the equation

5 th order

Le Châtelier’s Principle

when any change in concentration, temp, pressure, or volume is imposed on a system at equilibrium, the system responds by attaining a new equilibrium condition that minimizes the impact of the change

Equilibrium

Equilibrium- condition where the forward reaction and the reverse reaction proceed at the same rate
Equilibrium constant expression- the ratio of equilibrium constants raised to the power equal to the stoichiometric...
Le Châtelier’s Principle: when any change in concentration, temp, pressure, or volume is imposed on a system at...

Review AM quiz 2 #8, PM quiz 2 #7

Use integrated rate law and half life equation (t 1/2 =0.693/k) to solve

pK w

pK a + pK b

pK a + log [conjugate base]/[weak acid] or pK b +log [conjugate acid]/[weak base]

Acid-Base chemistry

Acid –Base chemistry is mostly numerical mostly math problems
Only use ICE tables for weak acids and bases, not for strong acids and bases because they completely dissociate in solution
K w = 1 x 10
K w = K a x K b
pK w = pK a + pK b
pH = pK w – pOH or pK w =pH +pOH
Hydrolysis (could be on final)

Henderson

Henderson- Hasselbalch equation (from ch 15)
K sp expressions- the solubility constant expressions
Relationship of K sp to molar solubility (see AM and PM Quiz 5 #s 8 & 9)
Q ip

Hydrolysis (could be on final)

See AM and PM quiz 4 # 13

Henderson- Hasselbalch equation (from ch 15)

Only for buffer solutions
pH=pK a + log [conjugate base]/[weak acid] or pK b +log [conjugate acid]/[weak base]

K sp expressions- the solubility constant expressions

Only involves the products of the reaction
Will be mostly numerical problems

Relationship of K sp to molar solubility (see AM and PM Quiz 5 #s 8 & 9)

Molar solubility- the molarity of a solute in a saturated aqueous solution

Set up ICE table to find equilibrium values
Convert solubility (g/L) to M and plug M into equilibrium values as s, solve for K sp

Q ip

reaction quotient = the product of the initial concentrations of the products

Q ip > K sp precipitation should occur
Q ip < K sp precipitation cannot occur
Q ip = K sp solution is saturated

Relationships between

Gibbs equation: G = H- TS
Criterion for spontaneous change

Nonspon at all T

G = -RT lnK
Voltaic Cell Components
Balancing Redox Reactions
Quiz 7- Chapters 18-19
Integrated rate law again- use to find and substitute in � life equation
G = -nFE 0 cell
Nernst Equation
Electrolysis

G = -RT lnK

See AM and PM quiz 6 #6

Voltaic Cell Components

Anode- where oxidation occurs, decreases in size, where negative ions flow
Cathode- where reduction occurs, increases in size(plating), where positive ions flow
Salt bridge- completes the circuit
Electrodes- metals (either cathode or anode)

Balancing Redox Reactions

Separate into the � reactions
Balance everything except H and O
Balance oxygen with water
Balance water with H +
Balance charge with e -
Cancel out electrons by multiplication
Combine � reactions
Check that charges are balanced--- STOP HERE IF IN ACIDIC SOLUTION
If in basic solution, add OH - s to both sides and cancel waters

Example

CrBr 3 + HCl

H 2 O 2H 2 O 4e - + 4H + +O 2

Look at E 0 values for each possible equation, the one with the highest value will occur at the cathode and the one with the lowest value will occur at the anode

-nFE 0 cell

Cathode (reduction)

Cr 3+ Cr 3+ + 3 e - ? Cr

Anode (oxidation)

Br - 2 Br - ? Br 2 + 2e -

About this deck

By: Sophie @Studyblue
Created: 2011-04-22
Size: 93 flashcards
Views: 1824

About StudyBlue

“I have been getting MUCH better grades on all my tests for school. Flash cards, notes, and quizzes are great on here. Thanks!”
Kathy