titration problem: how many moles of base are used with a sample mass of .1118grams and 15.83 mL of base?

Answer 1

Depends on what base was used. Was it NaOH?

One mole of anything is 6.02 x 1023 (Avogadro's number) of that thing. One mole of an element is 6.02 x 1023 atoms of that element and is a mass of that element equal to its atomic weight in grams. One mole of a compound is 6.02 x 1023 molecules of that compound and equals its formula weight (the sum of the atomic weights of all the atoms in the formula) in grams. For example, 1 mole of C = 12 g C = 6.02 x 1023 atoms; 1 mole CO2 = 44 g CO2 = 6.02 x 1023 molecules of CO2. And (grams of compound) × (formula weight) = number of moles of compound (number of moles of compound) × (formula weight) = grams of compound.


Na = 23
O = 16
H = 1
1 mole of NaOH = 40 grams

Answer 2

There isn't enough information in your question. You would need to know the identity or (molar mass) of your sample. You also would need to know the balanced chemical equation for the acid/base neutralization reaction...or at least if the base and acid react in a 1:1 mole ratio or some other ratio.