What is the concentration of the unknown sulfuric acid solution?
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Posted on : 07-09-2010 | By : My Study Coach | In : Improve Your Concentration
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Loading ...A 15.00 mL sample of unknown concentration of sulfuric acid is precititated with excess lead(II) nitrate and a precipate of lead (II) sulfate is collected. The dried sample of PbSO4 has a mass of 5.354 grams. What is the concentration of the unknown sulfuric acid solution
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5.354g of PbSO4 are 0.01754 mol, so the concentration is 0.01754/0.015=1.17 mol/l
Begin off by writing a chemical equation:
H2SO4+ PbSO4 —> [ something ]
List your givens for PbS04
m = 5.354g
M = Pb + S + 4O
= 207.2g/mol + 32.06g/mol + 4(16.00g/mol)
= 303.26 g/mol
n = m/M
= 5.354g/303.26g/mol
= 0.0176mol
The mol of PbSO4 is about 0.0176mol, and you know that the mol ratio of HCl: PbSO4 is 1:1 , therefore, to find concentration of HCl, you have to use the equation, C= n/v
n = 0.0176mol
v = 15.00mL = 0.015L
C = ?
C = n/v
= 0.0176mol / 0.015L
= 1.17 mol/L
Therefore, the concentration of the unknown sulfuric acid is about 1.17 mol/L
Hope that helps =]