HOW CAN WE DELIVER KNOWN WEIGHTS OF REACTANTS WITHOUT WEIGHING THEM FIRST?

CONSIDER: HNO3 + NaOH = NaNO3 + H2O

NEITHER NITRIC ACID, NOR SODIUM HYDROXIDE CAN BE WEIGHED EASILY. WHY?

HOWEVER, SOLUTIONS OF KNOWN AMOUNT OF SOLUTE PER UNIT VOLUME CAN BE DELIVERED IN KNOWN VOLUME TO GIVE PRECISELY-KNOWN AMOUNTS OF REACTANTS. WHY?

BECAUSE: (MOLES/LITER) X LITERS = MOLES

IF YOU KNOW THE NUMBER OF MOLES CONTAINED IN ONE LITER, YOU CAN CALCULATE THE MOLES CONTAINED IN ANY MEASURED VOLUME OF THAT SOLUTION.

TYPICALLY, A FLASK CALLED A VOLUMETRIC FLASK IS USED TO PREPARE A SOLUTION OF KNOWN CONCENTRATION,

(MOLES SOLUTE/LITERS SOLUTION). SOLUTE IS WEIGHED AND ADDED TO THE FLASK. THEN THE SOLVENT IS ADDED TO MAKE UP A KNOWN FIXED VOLUME OF SOLUTION.

THE AMOUNT OF SOLUTE PER UNIT VOLUME SOLUTION(TYPICALLY MOLES/LITER) IS CALLED THE CONCENTRATION OF THE SOLUTION. IT HAS TO BE DEFINED QUANTITATIVELY. THIS CAN BE DONE IN SEVERAL WAYS. WE WILL USE THE DEFINITION MOST COMMONLY USED IN ANALYSIS, MOLARIT

42.093u/molecule or = 42.093 g./mole

4 Al + 3 O2 = 2 Al2O3 BALANCED.

Note M x VL = moles = 0.0867 = 0.215 x VL

3x12.011 + 3x1.00794 + 15.9994 = 55.056 u

Some common words found in the essay are:
CARBON DIOXIDE, FORMULA MASS, MOLAR MASS, SAMPLE MOLES, Al2O3 BALANCED, CALCULATION Molecular, MDIL VDIL, CO2 Note, C3H2Cl2 C6H4Cl2, MOLES MOLECULES/MOLE, carbon dioxide, molar mass, moles =, moles carbon, moles carbon dioxide, empirical formula, mass =, molecular mass, = moles, formula mass, dioxide =, carbon dioxide =, empirical formula mass, moles solute/liters solution, grams carbon dioxide,
Approximate Word count = 1926
Approximate Pages = 8 (250 words per page double spaced)