3SnF2 + 2La(NO3)3 ==> 2LaF3 + 3Sn(NO3)2
1.mols SnF2 = grams/molar mass
2.Using the coefficients in the balanced equation, convert mols SnF2 to mols LaF3.
3. Convert mols of LaF3 to grams. g = mols x molar mass. This is the theoretical yield (TY) of LaF3 from the reaction. The actual yield (AY) is 0.105 g.
4. %yield = (AY/TY)*100 = ?
The tin (II) fluoride in a 10.000 g sample of toothpaste is extracted into solution and them a precipitate of lanthanum (II) fluoride (LaF3) is formed by the addition of a lanthanum (III) nitrate solution. If the mass of the lanthanum (III) fluoride precipitate is 0.105g, what is the percentage of tin (II) fluoride in the toothpaste?
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