5 gram of fuming h2 s o4 is neutralized by 26.7 ml of 0.4 n and the percent of h2 s o4 in the sample of oleum is
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0.5g of fuming H2SO4 is diluted with water. The solution requires 26.7ml of 0.4 N NAOH for complete neutralization. Can you find the percentage of free SO3?
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2 Answers
Renuka Varyani
Renuka Varyani, Maths Science Tutor and Executive Assistant at Sidra Medical and Research Center (2017-present)
Answered Jun 4 2018 · Author has 112 answers and 267.4k answer views
H2So4= 98/2 = 49
So3 = 80/2 = 40
26.7ml x 0.4N = 10.68ml - 0.01068L
x/49 + x/40 (0.5-X)
Eq. H2SO4 = Eq of NaOH
= (26.7 x 0.4)/1000
= 10.68 mEq.
H2SO4 + SO3 + H2O -----> 2(H2SO4)
==> SO3 + H2SO4 -----> H2SO4
∴Eq of SO3 = 1/2 of mEq. total H2SO4
==> Eq of H2SO4 + Eq of SO3 = Eq of total H2SO4
= 10.68/1000 (bec. 1 mEq. = 1/1000 Eq.)
Let x be mass of SO2 ==> mass of H2SO4
= (0.5-x)
= (0.5 - x)/49 + x/40 = 10.68/1000
Solving.... x = 0.1836g
Percentage of So3 = 0.1836/0.5 x 100
= 20.73%
Answer:
H2SO4 + SO3 + H2O -> 2(H2SO4) .
==> SO3 + H2SO4 -----> H2SO4
∴Eq of SO3 = 1/2 of H2SO4
==> Eq of H2SO4 + Eq of SO3
= Eq of total H2SO4
= 10.68/1000 (bec. 1 mEq. = 1/1000 Eq.)
Let x be mass of SO2 ==> mass of H2SO4 = (0.5-x)
= (0.5 - x)/49 + x/40 = 10.68/1000
Solving.... x = 0.1836g
Percentage = 0.1836/0.5 x 100 = 20.73%