Question
10.0 g of NH4NO3 is dissolved in enough water to make 450.0 mL of solution. What is the molarity of the solution?
Answers
Helper
a number of ways to do this
he must have put 1/10 of 10.8g in the sample, then diluted it to a volume of .050liters
Molarity=10.8/10 * 1/molmass*1/.050
where molmass is the molmass of ammonium nitrate.
he must have put 1/10 of 10.8g in the sample, then diluted it to a volume of .050liters
Molarity=10.8/10 * 1/molmass*1/.050
where molmass is the molmass of ammonium nitrate.
DrBob222
NOPE, that is not one of the ways to do this problem. The correct way to do this is as follows:
M = mols/L of solution. L is 0.45 from the problem. Find mols by
moles = grams/molar mass = 10.8/80 = xx
So M = mols/L = xx from above/0.45 = ?
M = mols/L of solution. L is 0.45 from the problem. Find mols by
moles = grams/molar mass = 10.8/80 = xx
So M = mols/L = xx from above/0.45 = ?