Question

URGENT. Find the volume of 0.150 M sulfuric acid necessary to react completely with 70.4 g sodium hydroxide.

Answer 1

we have the Balanced chemical equation as:

2 NaOH + H2SO4 ---> Na2SO4 + 2 H2O

Molar mass of NaOH = 1*MM(Na) + 1*MM(O) + 1*MM(H)

= 1*22.99 + 1*16.0 + 1*1.008

= 39.998 g/mol

mass of NaOH = 70.4 g

we have below equation to be used:

number of mol of NaOH,

n = mass of NaOH/molar mass of NaOH

=(70.4 g)/(39.998 g/mol)

= 1.76 mol

From balanced chemical reaction, we see that

when 2 mol of NaOH reacts, 1 mol of H2SO4 is formed

mol of H2SO4 reacted = (1/2)* moles of NaOH

= (1/2)*1.7601

= 0.88 mol

This is number of moles of H2SO4

we have below equation to be used:

M = number of mol / volume in L

0.150 = 0.88/ volume in L

volume = 5.87 L

Answer: 5.87 L