FINAL 11 EXAM FINALLY DONE WITH CHEM Flashcards
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Mole Ratio
ratio between the amount of moles of any two compounds involved in a chemical reaction
Excess reactant
the reactant is left after the reaction has stopped, not all reactants have been consumed in reactions
Limiting reactant
the reactant runs out first in a reaction, limits product formed
Mol Ratio equation steps
- write balanced equation
- write variable values under equation
- calculate number of known moles using n = m/M
- find the number of unknown moles using mole ratios
- Calculate mass of unknown using the formula m = n x M
Aliquot
small measured amount of homogenous liquid that is added to a solution of unknown concentration
Titre
total volume of solution delivered by burette to reach endpoint
Equivalence
the point in which the reaction occurs (neutralisation/titration occurs)
Endpoint
the point in which a change in colour is observed that indicates titration is complete
PH Curve
also called a titration curve, a group showing the pH change during titration, x-axis volume of titrant, y-axis pH of solution
Concordant
when the volume of two or more titres are similar in quantity
Meniscus
the curve seen at the top of a liquid in response to its container
Volumetric flask
used to prepare standard solution
Pipette
(used to accurately measure aliquot)
Burette
used to accurately measure known volumes of solution known as titre
Volumetric analysis steps
- write a balanced equation
- write variables
- calculate known moles using n = CV
- use mole ratio o find unknown moles
- calculate the unknown concentration using C = n/V
Strong acid
readily donates a proton
Weak acid
partially donates a proton
Acid
donates a proton
Base
accepts/retrieves a proton
Neutral
equal OH- and H+
pH
measure of acidity produced of H
Colorimetry colours absorbed vs colour of sample solution
(I don’t know if you need to learn this)
violet - green/yellow
violet/blue - yellow
blue - orange
Calibration curve x and y axis
x - Concentration
y - Absorbance
Oxidation reaction
a substance loses electrons
Reduction reaction
a substance gains electrons
Reducing agent
a substance that loses electrons and causes reduction
Oxidising agents
a substance that gains electrons and causes oxidation
Metal reactivity series
a list of metals ordered by their ability to react with acids
Standard electrode potential
measure of the tendency of a half-reaction to gain electrons (get reduced)
OIL RIG
oxidation is loss reduction is gain
Half equation electrons
reduction - electron on left side
oxidation - electron on right side
Potable
water that is safe enough to drink
Hydrogen bonding
when hydrogen bonds with either oxygen, nitrogen or fluorine (H-NOF)
Polar
significant differences in the electronegative between two or more atoms
Dispersion forces
the temporary force when shared electrons are unbalanced
Specific heat capacity
the quantity of energy needed to increase the temperature of a certain amount of substance by 1 degree Celsius
Specific heat capacity formula
Q=mcΔT
Q = heat energy (J)
m = mass(g)
c = specific heat capacity
ΔT = change in temperature (degrees C)
What is the specific heat capacity of water?
4.18
Density
how much space a substance takes up in volume compared to mass
Is ice or water more dense and why?
water is more dense as ice forms a hexagonal pattern that takes up more space
this allows ice to float in water
Latent heat of vaporisation
heat energy required to change 1 mole of substance from liquid to gas
Latent heat of fusion
heat energy required to change 1 mole of substance from solids to liquid
Latent heat formula
Q = mL
m - mass (kg)
L - specific latent heat value (kg/mol)
Amphiprotic substance
a substance that can act as both an acid and a base, for example water
Polyprotic
acid that can donate more than 1 proton
General neutralisation equation
equation
acid + base -> salt + water
General acid and metal hydroxide
acid + metal hydroxide -> salt + water
General acid and metal carbonate equation
acid + metal carbonate -> salt + water + carbon dioxide
Ionic product formula
Kw = [H3O+] x [OH-] = 1.0 x 10(-14) x M(2)
PH formula
pH = -log10[H3O+]
Concentration of acid formula
H3O+ = (10*(-14))/(OH-)
Concentration of base formula
OH- = (10*(-14))/(HO3+)
Concentration of neutral formula
OH- = H+ = 10*(-7) x M
Indicator
when a substance changes colour due to a pH change
Alkalinity
ability to neutralise an acid
Ppm to g/L formula
ppm = (g/L) x 10*(3)
Density formula
density = mass/volume
Salinity
dissolved salt content of a body of water
Celsius to Kelvin
273 Celsius = 0 Kelvin
Gas equation formula
PV=nRT
P = pressure (kPa)
V = volume (L)
n = number of mols (mol)
R = 8.31
T = temperature (K)
Pa to kPa to atm conversion
100 000 Pa = 100 kPa = 0.987 atm
3 Mole formulas
n = N/NA
n = m/M
c = n/v
Dilution formula
C1 x V1 = C2 x V2
Unsaturated
a solution that contains less solute than is needed to make the solution saturated
Saturated
a solution in which no more solute can be dissolved
Supersaturated
an unstable solution that contains more dissolved solute than a saturated solution
Anode
part in galvanic cell where oxidation occurs
Cathode
part in galvanic cell where reduction occurs
Displacement reaction
when an atom or atoms are displaced by one another (oxidation and reduction occurs), top is reduced and bottom is oxidised
