Question

How many liters of 4.0 M NaOH solution will react with 1.2 mol H2SO4? (Remember to balance the equation.)

H2SO4 + NaOH → Na2SO4 + H2O

A. 1.6 L
B. 1.2 L
C. 0.90 L
D. 0.60 L

Answer 1

The answer to this is D

Answer 2

The answer is D. 0.60 L

Step-by-step explanation:

The balanced reaction equation including states of matter is;

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

More simple:

H2SO4 + 2NaOH → Na2SO4 + 2H2O

Now, we can see from this reaction equation that the mole ratio of NaOH to H2SO4 is 2:1

Number of moles of H2SO4 reacted = 1.2 moles

Hence;

2 moles of NaOH reacts with 1 mole of H2SO4

x moles of NaOH reacts with 1.2 moles of H2SO4

x = 2 * 1.2/1 = 2.4 moles of NaOH

Recall that;

Number of moles = Concentration * Volume

Volume = number of moles/concentration

Volume of NaOH is obtained from;

Volume = 2.4 moles/ 4.0 M

Volume = 0.60 L