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October 22, 2014

Posted by **Amanda** on Sunday, December 12, 2010 at 4:09am.

Could anyone please help me out with this problem? I've been finding ways to solve this for hours now but I still cannot find a solution to it. *sigh*

- Chemistry -
**Dr Russ**, Sunday, December 12, 2010 at 8:49amPerhaps if you post what you have done so far we can see where the problem is.

- Chemistry -
**Amanda**, Sunday, December 12, 2010 at 9:05amI have computed for the density of the water @ 10deg celcius first. (999.103g/1L = 999.103g/L)

Then I determined the density of the sulfuric acid by using the formula:

spec gravity = Densityh2so4 / Densityh2o

therefore,

Densityh2so4 = (1.839)(999.103g/L) = 1.837mg/L

Next, I multiplied the Densityh2so4 with 0.97 for the 97% Industrial Sulfuric Acid to get the concentration in terms of mg/L.

Concentration of industrial h2so4 = 1.782 mg/L

Afterwards, Ive computed for the Molarity..

Molarity = (10*%weight*Densityh2so4)/MolecularWeight

= (10*97*0.001782g/mL)/98.08

M = 0.035 M

Normality = 2*M

= 2*0.035

= 0.07 N

IS THIS CORRECT? If not, please tell me where i got lost. Hehe. Thanks!

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