A titration is carried out using a .25M solution of sulfuric acid and 35.2mL and

Question

A titration is carried out using a .25M solution of sulfuric acid and 35.2mL and .45M NaOH.

Select all the options that correctly reflect the quantities of the two substances at the equivalence point.

The balaned molecular equation is H2SO4(aq) + 2NaOH(aq) -> 2H2O(l)+Na2SO4(aq).

1 The volume of H2SO4 used is equal to 63.4mL.

2 There are 1.58*10^-2 moles of NaOH present in the original solution.

3. 3.16*10^-2mol of H2SO4 are required to neutralize the NaOH.

4 The volume of H2SO4 used is equal to 31.7mL

Explanation / Answer

1) let the volume be v.so,

2*v*0.25=35.2*0.45

or v=31.68 mL

2)moles of NaOH=35.2*10^-3*0.45

=1.58*10^-2

3)moles of H2SO4 required=0.5*1.58*10^-2

=7.9*10^-3 moles

so 2 and 4 are only correct

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