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MCAT General Chemistry Review 6
Lesson 6 - Acids and Bases
30
Chemistry
Not Applicable
06/29/2011

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Term

Arrhenius Acid

 

Arrhenius Base

Definition

Anything that produces hydrogen ions in an aqueous solution.

 

Anything that produces hydroxide ions in an aqueous solution.

Term

Bronsted and Lowry Acid

 

Bronsted and Lowry Base

Definition

Anything that donates a proton

 

Anything that accepts a proton

Term

Lewis Acid

 

Lewis Base

Definition

Anything that accepts a pair of electrons.

 

Anything that donates a pair of electrons.

Term
pH Measurement
Definition
pH = -log[H+]
Term
Conjugate Acid
Definition

The resultant product of a base in a reaction.

Term
Conjugate Base
Definition
The resultant product of a acid in a reaction.
Term
Amphoteric
Definition
Substance that act as an acid or base dependent on the environment.
Term
Strong Acids
Definition

Hydroidic acid,     HI

Hydrobromic acid,  HBr

Hydrochloric acid,  HCl

Nitric acid,               HNO3

Perchloric acid,         HClO4

Chloric acid,             HClO3

Sulfuric acid,             H2SO4

Term
Strong Base
Definition

Sodium Hydroxide,      NaOH

Potassium Hydroxide, KOH

Amide Ion,               NH2-

Hydride Ion,          H-

Calcium Hydroxide,         Ca(OH)2

Sodium Oxide,           Na2O

Calcum Oxide,          CaO

Term
Polyprotic
Definition
Can donate more than one proton
Term
How Molecular Structure Affects Acid Strength
Definition

1. Strength of the bond holding the hydrogen to the molecule

2. the polarity of the bond

3. the stability of the conjugate base

Term
Hydrides
Definition
Binary compounds that contain hydrogen
Term
Autoionization of Water
Definition

Pure water reacting with itself to form hydronium and hydroxide ions.

 

H20 + H20 --> H- + H30+

Term
Kw Equilibrium Constant
Definition

Kw = [H+][OH-]

 

Kw =10-14

 

KaKb=Kw

Term
pKw of Water
Definition

pKw=pH + pOH

pKa + pKb = pKw

Term
Acid Dissociation Constant, Ka
Definition
Ka = [H+][A-]/[HA]
Term
Base Dissociation Constant, Kb
Definition

Kb = [OH-][HA]/[A-]

Term
Ka = ?
Definition

Ka = [H+][A-]/[HA]

 

If we know Ka and molar concentration of the acid, and need to find the pH, we can solve for

x*x/.01-x = Ka which reduces to

x2/.01=Ka

Term
Salt
Definition

Ionic compounds that dissociate in water.

When salts dissociate they often create acidic and basic conditions.

Term
Titration
Definition

Drop by drop mixing of an acid and a base.

 

Performed to find the concentration of some unknown by comparing it with the concentration of the titrant.

Term
Equivalence Point (Stoichiometric point)
Definition
Point for a monoprotic acid in titration when there are equal equivalents of acid and base in a solution.
Term
Titration with a base stronger than the acid:
Definition
Equivalence point is above 7
Term
Titration with the acid stronger than the base.
Definition
Equivalence point below 7
Term
Half equivalence point
Definition

Point where one half of the acid has been neutralized by the base.

 

Concentrations of the acid equal to the concentration of the conjugate base.

 

This shows the point where the solution is the most well buffered.

 

pH of the solution = pKa of the acid.

Term
Buffered Solution
Definition
We can add the largest amount of base or acid with the least amount of change in pH.
Term
Henderson-Hasselbalch Equation
Definition

pH = pKa + log([A-]/[HA])

 

When [A-]=[HA], pH=pKa because log(1) = 0 

Term
Indicator
Definition
A weak acid whose conjugate base is a different color.
Term
Range
Definition
The pH values of the two points of color change. Can be predicted by the HH Equation
Term
Endpoint
Definition
The point where an indicator changes color.
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