Acids/Bases
Potassium Hydroxide/Caustic Potash
Define Amphoteric
An amphoteric substance can act as both an acid or a base depending on its reaction partner.
What is an example of an amphoteric substance?
H2O, ZnO, HCO3-
Define Isomer
Compounds with the same molecular formula but different molecular structure.
What molecules are excluded from equilibrium constant calculations?
Liquids and Solids are noted as [1] in equilibrium constant equations.
Magnesium Hydroxide/Milk Of Magnesia
What is Arrhenius definition of acids and bases?
Acids produce H+ in aqueous solution.
Bases produce OH- in aqueous solution.
Example of conjugate acid-base pair
H2O + H+ = H3O+ + OH-
H+=Acid
H2O = Base
H3O+=Conjugate Acid
OH-=Conjugate Base
Define Acids and Bases according to Brønstead Lowry
Acids are proton (H+ Ion) donors
Bases are proton (H+ Ion) acceptors.
As temperature increases, equilibrium shifts towards the _____ side of the reaction.
Endothermic
Chemical and Salt Name for H2CO3
Carbonic Acid/Hydrogen Carbonate
Define an oxidation agent
An oxidation agent gains electrons, therefor causing oxidation.
Give an example of factors that affect yield in a chemical reaction.
Pressure, Heat, Concentration.
Define a reduction agent
A reduction agent loses electrons, therefor causes reduction.
NH3 + h2O --> NH4+ + OH-
NH4+
There is 5g of Ca(OH)2 in 2l of solution
Calculate Concentration
C = .03374M
Define Conjugate Acid-Base pairs according to Brønstead Lowry.
Two substances that differ by one proton (H+ Ion).
A conjugate acid has gained a proton during the reaction
A conjugate base has lost a proton during the reaction.
Acids are H+ donors
Bases are H+ acceptors.
Example of a 1-protic, 2-protic, and 3-protic acids
Multiple answers, i.e. HF, H2S, H3PO3
Define Catalyst
A catalyst is a substance that speeds up the rate of a chemical reaction without being consumed in the process.
What general information can be gathered by observing the magnitude of the equilibrium constant?
Kc>1: Reaction proceeds almost totally towards the products.
Kc<1: Reaction hardly proceeds at all towards the products.
A 0.10 M solution of acetic acid (CH₃COOH) has a dissociation constant
Ka=1.8×10^−5
Calculate pH of the Solution *Hint: Use ICE Table*
[H+]=1.34*10^-3 M
pH=2.87
What is Le Chatlier's Principle?
If a system at equilibrium is subjected to a change the position of the equilibrium will SHIFT to minimize the effect of the change.
Example of an Alkane, alkene, and alkyne
Alkane: Methane(CH4), Ethane(C2H6)
Alkene: Propene(C3H6), Ethene (C2H4)
Alkyne:Acetylene (C2H2), Propyne(C3H4)
Define dynamic equilibrium
Calculate concentration:
5.8g of (NaCl) is dissolved in water to make 500ml of solution.
Concentration = 0.200 mol/l