Acids
Bases
K
equations
pH
100
This particle is an Arrhenius acid
What is H+
100
This is an Arrhenius base
What is OH-
100
This is the equilibrium constant for water
What is 1.0 x 10^-14
100
H2O --> H+ + OH-
What is dissociation equation for water
100
this is what the letters pH stand for
What is "power of Hydrogen"
200
This is the species that acttually exists in water as an acid
What is H3O+
200
This is the concentration of base in neutral water
What is 1.0 x 10^-7
200
Ka is this
What is the acid dissociation equilibrium constant
200
This is the equation for K
What is K = [reactants]/[products]
200
pH of 1.0 x 10-8
What is 8
300
a strong acid
What is HCl, H2SO4, others
300
a strong base
What is NaOH or any alkali metal bases
300
pH = 3.2 in a 0.02 M solution of an acid, what is Ka?
What is 2.0 x 10^-5
300
these states of matter have concentrations of 1 in equilibrium equations
What are solids and liquids
300
2.3 x 10 ^-4
What is 3.6
400
a weak acid
carbonic acid, acetic acid
400
a common household substance that is basic
What is soap, detergent, bleach
400
Kb of a base with a pH of 8.9 and a concentrating of [.001M]
What is 1.5 x 10^-15
400
formation of the acid salt NH4NO3
What is NH3 + HNO3-->
400
pH = 5.6, what is the [H+]
What is 2.5 x 10^-6
500
Amphiprotic substances
What is any substance that can behave as either an acid or a base
500
[2.5 x 10^-3]
What is 2.6
500
K= 1.8 x 10^-5 in a pH of 4.5 , what is the concentration of the original acidic solution?
What is .00006 M
500
(-x) can be eliminated from the denominator of an equilibrium equation when the % dissociation is?
What is less than 5%
500
why will adding NaOH with a concentration of 1.0x10^-9 not change the pH of water.
What is concentration is so small
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