48. when excess bacl2(aq) was added to a sample of fe(nh4)2(so4)2(aq) to determine the amount in moles of sulfate present, 5.02×10–3 mol of baso4 was obtained. how many moles of sulfate ions and iron ions were in the sample of fe(nh4)2(so4)2?
Answers
Given the moles of is
.
The Balanced chemical reaction is
Mole ratio of to
is 1:2
Calculating the moles of reacting with
=0.00251
Calculating the moles of Fe:
0.00251
=0.00251 mol
Calculating the moles of sulfate ion:
0.00251
=0.005023 mol
Answer:
Given the moles of BaSO_{4}BaSO
4
is 5.023*10^{-3}5.023∗10
−3
.
The Balanced chemical reaction is
2BaCl_{2} +Fe(NH_{4})_{2}(SO_{4})_{2} -- > 2BaSO_{4}+Fe(NH_{4})_{2}Cl_{4}2BaCl
2
+Fe(NH
4
)
2
(SO
4
)
2
−−>2BaSO
4
+Fe(NH
4
)
2
Cl
4
Mole ratio of Fe(NH_{4})_{2}(SO_{4})_{2}Fe(NH
4
)
2
(SO
4
)
2
to BaSO_{4}BaSO
4
is 1:2
Calculating the moles of Fe(NH_{4})_{2}(SO_{4})_{2}Fe(NH
4
)
2
(SO
4
)
2
reacting with 5.023*10^{-[tex] < /p > < p > [tex]5.023*10^{-3} mol BaSO_{4} *\frac{1 mol Fe(NH_{4})_{2}(SO_{4} )_{2} }{2mol BaSO_{4} }
=0.00251 Fe(NH_{4})_{2}(SO_{4})_{2}Fe(NH
4
)
2
(SO
4
)
2
Calculating the moles of Fe:
0.00251 Fe(NH_{4})_{2}(SO_{4})_{2}Fe(NH
4
)
2
(SO
4
)
2
*\frac{1mol Fe^{+2} }{1 mol Fe(NH_{4})(SO_{4})_{2} }∗
1molFe(NH
4
)(SO
4
)
2
1molFe
+2
=0.00251 molFe^{2+}Fe
2+
Calculating the moles of sulfate ion:
0.00251 Fe(NH_{4})_{2}(SO_{4})_{2}Fe(NH
4
)
2
(SO
4
)
2
*\frac{2mol SO_{4} ^{-2} }{1 mol Fe(NH_{4})(SO_{4})_{2} }∗
1molFe(NH
4
)(SO
4
)
2
2molSO
4
−2
=0.005023 molSO_{4} ^{-2}SO
4
−2