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Table T<br />
Important Formulas and Equations<br />
d = density<br />
m<br />
Density d = m = mass<br />
V<br />
V = volume<br />
Mole Calculations number of moles =<br />
given mass<br />
gram-formula mass<br />
measured value – accepted value<br />
Percent Error % error = × 100<br />
accepted value<br />
mass of part<br />
Percent Composition % composition by mass = × 100<br />
mass of whole<br />
mass of solute<br />
parts per million = × 1000000<br />
mass of solution<br />
Concentration<br />
molarity =<br />
moles of solute<br />
liter of solution<br />
Combined Gas Law<br />
P<br />
P = pressure<br />
1<br />
V 1<br />
P<br />
= 2<br />
V 2<br />
V = volume<br />
T 1<br />
T 2 T = temperature<br />
M A<br />
= molarity of H + M B<br />
= molarity of OH –<br />
Titration M A<br />
V A<br />
= M B<br />
V B<br />
V A<br />
= volume of acid V B<br />
= volume of base<br />
q = mCΔT q = heat H f<br />
= heat of fusion<br />
Heat q = mH f<br />
m = mass H v<br />
= heat of vaporization<br />
q = mH v<br />
C=specific heat capacity<br />
ΔT = change in temperature<br />
Temperature<br />
K = °C + 273<br />
K = kelvin<br />
°C = degree Celsius<br />
DET 609 ADU<br />
Reference Tables for Physical Setting/Chemistry – 2011 Edition 12