4.5-4.9 Quiz Flashcards
Excess reagent
The reactant that is not fully consumed
Analyte
The unknown solution in the flask during a titration
If a pH meter is used in a titration where is the equivalence point on the graph?
Right at the pH of 7
On a pH meter graph where would the other compound be an excess reactant?
All the space under the equivalence point
Equivalence point in a titration
- Definition
- Indicator that it has been reached
When the analyte is totally consumed by the reacting species in the titrant
- Color change
End point
When the indicator changes color in a titration
Percent yield formula
Actual(experimental) yield/ Theoretical(calculated) yield times 100
Titrant
What is coming out of the burette(typically KMnO4)
Limiting reagent
The reactant that runs out first
Review 4.5 quiz
What should you always start with in a stoichiometry problem?
Start with a balanced equation
How to find limiting reagent in stoichiometry?
Turn both reactants into moles or grams or something and see whichever one has less and that is the limiting reagent but if they are the same look at the coefficients to help you determine as well
How do you read a pH meter graph of a titration?
Drop a vertical line down to discover the volume
Practice stoichiometry problems
4.5 questions
acid- base reaction
Transfer of one or more hydrogen ions between compounds
Oxidation-reduction reactions
Transfer of one or more electrons; every single reaction except for double replacement and acid base
Combustion
A reaction with oxygen as a reactant and if its a hydrocarbon then the products are co2 and water
What is always soluble?
SNAP
sodium
nitrate salts
ammonium
potassium
Acid
Proton donors
Bases
Proton acceptors
Conjugate acid
A base that gained one proton
Conjugate Base
An acid that lost one proton
Amphoteric
Substances that can act as an acid or base
Strong acid or base
Will completely separate
Weak acid or base
Will only partially separate
Oxidation
OIL
Loss of electrons
Reduction
RIG
Gain of electrons
Oxidation number rules
- An atom in its elemental form has an oxidation number of 0.
- Any monatomic ion has an oxidation number equal to the charge on the ion. ex: Fe3+ = +3
- In binary compounds, the more electronegative atom is given the oxidation state of its species (ie.
the common ion of its group). Fluorine is always -1. - Atoms in groups 1 and 2 are +1 and +2, respectively.
- The sum of the oxidation state must be equal to the overall charge of the element or compound.
