Chapter 4 Flashcards by Jacob Gillespie

When is there a negative pH

When molarity of the acid is above 1

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Larger equilibrium constant means what

Larger means the more the product as are favoured

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Kc =?

[products]
——————
[reactants]

If 2Al is the product its [Al] ^2

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Oxidation #

Elements

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Oxidation #

Elements

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Oxidation number oxygen

-2 usually

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Oxidation number H

With metal vs nonmetal

Metal= -1

Nonmetal = +1

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Element in group 1 oxidation number

Always +1

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Elements in group 2 oxidation number

Always +2

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Halogens. Period 7 oxidation numbers

Usually -1. Positive with oxygen

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F oxidation number

-1 always

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Sum of oxidation numbers for a neutral compound

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Sum of oxidation numbers for a polyatomic ion

Equal to the ion charge

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Sum of oxidation numbers for a polyatomic ion

Equal to the ion charge

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Which is the most conductive and why

1Molar Na2SO4

1 molar NaCl

Na2SO4 bc there’s more ions (3) than NaCl(2)

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Ppm formula

Parts per million

Mg/kg

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Ppb formula

Parts per billion

Micrograms/kg

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PH formula

-log(concentration)

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Reducing agent

Oxidizing agent

Gain electrons reduce

Al + F2= Al^3+ + F-

Al is reducing

F2 is oxidizing

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PH vs POH

How to convert

pH is for an acid

pOH is for a base

Example when u have 0.12M base

-log(.12)=POH= 0.92

To get ph

PH=14-POH=13.08

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Strong vs weak Electrolytes

Strong-
-almost 100% dissociation (-> in equation)
-good conductor

Weak
-slightly dissociate into ions
-(<->equilibrium arrows in equation)
-slightly conductive

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Nonelectrolites

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No ionization occurs
Don’t conduct current

Examples of nonelectrolytes

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Aqueous solutions of sugar, ethanol, ethylene glycol

Bronsted Lowry acid vs base

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Proton donor-acid
Vs

Proton acceptors - base

Neutralization

Acid and base reacts producing a salt in water

What do they mean by produce a salt in a base

Cation (+) of the base and the anion (-) of the acid

Nonmetal oxides do what Example

Form acids in hydrolysis SO3+ h2o= H2SO4

Strong acids and bases vs weak acids and bases

Strong: - dissociate completely (—>) Weak: -partially dissociate (<————>)

Examples of strong acids

-HCl -HBr -HI -HNO3 -H2SO4 -HCLO4

Amphiprotic

Acts as acid and a base Ex-Water

Standard solution in titration

Known concentration AKA titrant

Equivalence point

When the moles of the titrant are stoichiometrically equivalent to the solution being tested

End point

When the indicator changes color

Soluble cations

Group 1 ions (alkali metals) NH4

Soluble anions

Saturated solution

Contains maximum concentration of a solute possible at a given temperature

Supersaturated solution

Solution containing more than the maximum quantity of a solute predicted to be soluble

Ion exchange

1 ion displaced with another Important in purification Switch soft metal ions (Na) with “hard” metal ions (Ca2+)

Ion exchange

1 ion displaced with another Important in purification Switch soft metal ions (Na) with “hard” metal ions (Ca2+)

When is equilibrium achieved in dynamics

Forward rate= reverse rate

Law of mass action

Principle of relating the balanced chemical equation of a reversible constant to its (mass action expression) equilibrium constant expression

Mass action expression

Equivalent to equilibrium form expression but applied to reaction mixtures that may or may not be at equilibrium

Equilibrium constant expression

Ratio of conc. Or partial pressures of products to reactants at equilibrium. With each term raised to a power (equal to the coefficient)

Equilibrium constant

Numerical value of the equilibrium constant expression of a reversible chemical reaction at a particular temp

Equilibrium constant (K) Traits

-K is always positive -K>1 means rxn when everything mostly at equilibrium -K(1-0) associated with rxn when few products at equilibrium

Lies to the right in terms of equilibrium constant

K>1 products favored Nearly all reactants form products

Lies to the left in terms of equilibrium constant

K<1 favored reactants Few products are produced

Strong bases Kb value

Kb>1

Weak bases Kb value

Kb<1

Strong acids Ka value

Ka>1

Weak acids Ka value

Ka<1

Trends in conjugate acids and bases

The stronger the acid the weaker its conjugate base Vice versa

Levelling effect

Strong acids have the same strength in water and are completely converted to h3o ions Strong bases are levelled in water and are completely converted into (OH-) ions (The stronger Ka or Kb, the more dissociation increases)

Kw = pKw =

Kw=1x10^-14=[H3O][OH] pKw=14=pH + pOH

Chapter 4 Flashcards

(54 cards)