##### chemistry question, titrations

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a 30.0mL sample of .220M sulfuric acid is titrated with potassium hydroxide. if it takes 26.4mL of base solution to reach the endpoint, what is the molarity of the base solution?

Apr 21st, 2015

Firstly, we can write down the chemical balanced equation as follow:

H2SO4(aq) + 2KOH(aq) → K2SO4(aq) + 2H2O(l)

Conversion of units:
30.0 mL = 0.03 L
26.4 mL = 0.0264 L

The moles of sulfuric acid used can be calculated by:

nacid = Macid x Vacid = (0.220 M) x (0.03 L) = 6.6 x 10-3 mol

According to the balanced equation, since 1 mol of H2SO4 is reacted with 2 mol of KOH, we have that the moles of potassium hydroxide is equal to

nbase = 2 x 6.6 x 10-3 mol = 1.32 x 10-2 mol

Finally, the molarity of the 26.4mL base solution is determined by:

Mbase = nbase/ Vbase = ( 1.32 x 10-2 mol) / (0.0264 L) = 0.500 M

Apr 21st, 2015

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Apr 21st, 2015
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Apr 21st, 2015
Oct 17th, 2017
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