Weight of the mustard package Sample: 3.02 (g)
Weight of the mustard package Solution: 33.3 (g)
Trial #1 Trial #2 Trial #3
Weight of Mustard Package Solution Delivered (g) : 1.09 .948 .909
Weight of NaOH Solution Delivered (g) : .354 .304 .269
Concentration of NaOH : 7.48e-3 (g of NaOH/g of solution)
Calculate the weight percent of Mustard in your originally prepared solution.
Forget it i got the answer
What are you titrating?
mustard solution, how would i calculate the mass of naOH used?
mols NaOH used is M x L = ?mols NaOH used.
g NaOH used = mols x molar mass NaOH.
After getting this, in order to convert the three masses into moles, what do I divide each mass by
The molar mass of what ever it is you are converting to mols. Which harks back to my original question of what are you titrating. The NaOH surely is titrating an acid; therefore, I expect you want grams of the acid. So mols of NaOH = M x L. Most of acid probably = mols NaOH (I assume a 1:1 reaction).
mol acid x molar mass acid = grams.
grams x the dilution factor converts g in the original sample to grams of the titrated sample.
%acid = (g acid/mass sample)*100 = ?
mols = grams/molar mass.
To calculate the weight percent of mustard in the originally prepared solution, you need to find the weight of mustard in the solution and divide it by the total weight of the solution.
First, find the weight of mustard in the solution by subtracting the weight of the mustard package from each trial's "Weight of Mustard Package Solution Delivered":
Trial #1: Weight of Mustard Solution = 1.09g - 3.02g = -1.93g (negative value indicates an error in measurement)
Trial #2: Weight of Mustard Solution = 0.948g - 3.02g = -2.072g (negative value indicates an error in measurement)
Trial #3: Weight of Mustard Solution = 0.909g - 3.02g = -2.111g (negative value indicates an error in measurement)
Since all the calculated weights of mustard in the solutions are negative, it suggests that there was an error in the measurements or calculations. Please check the data and calculations for accuracy and try again.