Question

What is the volume of 0.1M NaOH needed to reach the end point of 10 mL of 3.5M H2SO4?

Thanks

Answer 1

Sol:-

data provided in the question is :-

concentrat​​​​​​​ion of  NaOH = 0.1 M

• concentration of  H₂SO₄ = 3.5 M
• volume of H₂SO₄ = 10 mL = 0.010 L​​​​​​​

Formula used :-

moles of compound = (Molarity)* (Volume of solution)

reaction:-

H₂SO₄ (aq) + 2NaOH(aq) Na₂SO₄(s) + 2H₂O(l)

Calculation :-

let the volume of NaOH require to reach end point is "x" L.

mole of H₂SO₄ = (3.5 M) * (0.010 L)

= 0.035 mole

mole of NaOH = ( 0.1 M) * ( x L)

= 0.1x mole.

end point means complete reaction of H₂SO₄ .

so,

1 mole of H₂SO₄ complete reacts with 2 mole of NaOH.

0.035 mole of H₂SO₄ complete reacts with 2*0.035 mole of NaOH.

then,

2*0.035 = 0.1x

x = 0.070/0.1

= 0.70 L

then

Volume require to reach end point of H₂SO₄​​​​​​​ is 0.70 L = 700 mL.