The question is incomplete, here is a complete question.
A sample of impure tin of mass 0.538 g is dissolved in strong acid to give a solution of . The solution is then titrated with a 0.0448 M solution of , which is reduced to NO(g). The equivalence point is reached upon the addition of of the solution.
Find the percent by mass of tin in the original sample, assuming that it contains no other reducing agents.
Answer : The percent mass of tin in the original sample is 61.3 %
Solution :
First we have to calculate the moles of .
Now we have to calculate the moles of
The balanced chemical reaction is,
From the reaction, we conclude that
As, 2 mole of react with 3 mole of
So, moles of react with moles of
Now we have to calculate the mass of
Molar mass of tin = 118.71 g/mol
Mass of reacted = 0.330 g
Original mass of = 0.538 g
Now we have to calculate the percent mass of tin in the original sample.
Therefore, the percent mass of tin in the original sample is 61.3 %