Write down as many correct, distinct, and relevant facts you can about the following prompt: 100 mL of 1.0 M solution H2SO4 is added to 7.0 grams of NaOH in the reaction below: H2SO4(aq) + 2NaOH(aq) --> Na2SO4(aq) + 2H2O (l)

Explanation:

From the equation:

H2SO4(aq) + 2NaOH(aq) --> Na2SO4(aq) + 2H2O (l)

1 mole of the acid (H2SO4) and 2 moles of the base (NaOH) are required for complete neutralization.

mole of acid (H2SO4) present = molarity x volume

                                  = 1 x 0.1 = 0.1 mole

Mole of base (NaOH)  present = mass/molar mass

                                                      = 7/40 = 0.175 mole

The ratio of acid and base should be 1:2, hence the acid is slightly excessive in this case and the base is the limiting reagent that will determine the extent of the reaction.

Amount of excess acid = 0.1 - 0.175/2

                                       = 0.0125 mole

volume of excess acid = mole/molarity

                                      = 0.0125 x 1 = 0.0125 L

                                       = 12.5 mL

Hence, the acid (H2SO4) was in excess by 12.5 mL.

the answer is 0.42 is that is an option. this question provides no info