Question

How many millilitres of 0.1 n h2so4 solution will be required with a solution containing 0.125 g of pure na2co3?

Answer 1

Answer:

23.58 mil

Explanation:

It's simple acid base neutralisation.

For complete reaction no. of equivalents must be equal.

No. of moles of Na2CO3 = mass/molar mass == 0.125/106 == 0.001179 mol

No. of equivalents of Na2CO3 == no. of moles X valence factor == 0.001179 X 2 == 0.002358

This is no. of equivalents H2SO4 must be present for complete reaction.

For H2SO4 no. of equivalents == Normality X vloume(in litres)

Therefore volume in L of H2SO4

== 0.002358/0.1

== 0.02358 Litre

== 0.02358*1000 mil.

== 23.58 Millilitres

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