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Exambusters Study Cards 16 Acids and Bases
Acids and Bases Cards 300-330
43
Chemistry
10th Grade
10/17/2012

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Term
Ionization Constant
Definition
Kw = 1 X 10-14 at 25 °C
Term
pH
Definition
pH = -log[H+]
Term
For what pH values is a solution acidic?
Definition
< 7
Term
For what pH values is a solution neutral?
Definition
= 7
Term
For what pH values is a solution basic?
Definition
> 7
Term
pOH
Definition
pOH = -log[OH-]
Term
For what pOH values is a solution acidic?
Definition
> 7
Term
For what pOH values is a solution neutral?
Definition
= 7
Term
For what pOH values is a solution basic?
Definition
< 7
Term
How are pH and pOH of a solution related?
Definition

The sum of the two values = 14

pH + pOH = 14

Term
How are the concentrations of [H+] and [OH-] related in a solution?
Definition

The product of the concentrations = 1 x 10-14

[H+][OH-] = 1 x 10-14

Term

Match pH value to distilled water.

a.) pH=2

b.) pH=7

c.) pH=12

Definition
b.) pH = 7
Term

Match pH value to lye.

a.) pH=2

b.) pH=7

c.) pH=12

Definition
c.) pH= 12
Term

Match pH value to stomach juice.

a.) pH=2

b.) pH=7

c.) pH=12

Definition
a.) pH=2
Term
For a solution with a pH of 3, find pOH
Definition
pOH = 11
Term
For a solution with a pH of 3, find [H+]
Definition
[H+] = 1 x 10-3
Term
For a solution with a pH of 3, find [OH-]
Definition
[OH-] = 1 x 10-11
Term
Solubility Product Constant - Ksp
Definition
An equilibrium exists in a saturated solution between dissolved and undissolved solute. "Ksp" is the equilibrium constant for this reaction.
Term
Write the solubility product expression for AgCl double arrow Ag+ = Cl-
Definition
Ksp = [Ag+][Cl-]
Term

In a saturated solution of BaSO4, [Ba2+] = 2 x 10-5.

Find Ksp.

Definition

Each molecule of BaSO4 that ionizes produces equal concentrations of ions; therefore;

[Ba2+] = [SO42-]

Ksp = [Ba2+][SO42-]

Ksp=[2 x 10-5][2 x 10-5]

Ksp = 4 x 10-10

Term
Common Ion Effect
Definition
When an ionization reaction is at equilibrium, and additional ion is added, the reverse reaction rate increases to consume the added ion.
Term

NaCl ↔ Na+ = Cl-

What happens when Cl- is added to this system at equilibrium?

Definition
According to the common ion effect, the reverse reaction will speed up, consuming Na+ and Cl-, and more NaCl will be formed.
Term
Six common characteristics of ACIDS
Definition

form H2O solutions

conduct electricity

react with active metals

turn blue litmus red

neutralize bases

sour taste

Term
Seven common characteristics of BASES
Definition

form H2O solutions

conduct electricity

turn red litmus blue

feel slippery

caustic

neutralize acids

bases + fats form soap

Term
Strong Acids
Definition

nitric

hydrochloric

sulfuric

hydriodic

hydrobromic

perchloric

Term
Weak Acids
Definition

hydrofluoric

acetic

carbonic

and most others

Term
Moderately Strong Acids
Definition

oxalic

phosphoric

sulfurous

Term
Strong Bases
Definition

hydroxides of:

potassium

sodium

barium s

trontium

calcium

 

also:

KOH

NaOH

Term
Hydronium ion
Definition

H3O+ ion found in water solutions of acids.

Water molecule with a proton attached.

Term
Neutralization Reaction
Definition
acid + base → salt + water
Term
Write the equation for hydrochloric acid and sodium hydroxide.
Definition
HCl + NaOH → NaCl + H2O
Term
Arrhenius Theory
Definition
An acid yields protons in solution. (H+ ions) A base yields hydroxide ions in solution. (OH- ions)
Term
Bronsted-Lowry Theory
Definition

An acid is a proton donor.

A base is a proton acceptor.

Term
Lewis Theory
Definition

An acid is an electron pair acceptor.

A base is an electron pair donor.

Term
Conjugate Base: Write conjugate base of HCl.
Definition
When a Bronsted acid donates a proton, it becomes its conjugate base. Conjugate base of HCl is Cl-.
Term
Conjugate Acid: Write conjugate acid of I-
Definition
When a Bronsted base accepts a proton, it becomes its conjugate acid. Conjugate acid of I- is HI.
Term
Indicator
Definition

A substance which changes color along the pH scale.

e.g. litmus, phenolphthalein, methyl orange, bromthymol blue

Term
Titration
Definition
A process of finding the unknown concentration of a solution by allowing it to react with another solution of known volume and concentration.
Term
Endpoint
Definition
The point during a titration at which the acid reacts completely with the base. The indicator changes color.
Term
Write the equation to calculate concentrations and volumes in titration reactions.
Definition

MA X VA = MB x VB

 

molarity = M

volume = V

acid = A

base = B

Term
Calculate the volume of 10 M NaOH needed to titrate 5L of 2M HCl
Definition

MA X VA = MB X VB

2M X 5L = 10M X VB

1L = volume of base

Term
Buffer Solutions
Definition
Equilibrium systems which resist changes in pH upon the introduction of acids or bases (due to the common ion effect). e.g. a weak acid (acetic acid) and its salt (sodium acetate)
Term
Electrolysis
Definition
The passage of a direct electric current through an ionic solution, producing chemical changes at the electrodes.
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