Final answer:
To find the volume of sulfuric acid necessary, calculate the moles of sodium hydroxide, use the stoichiometry of the reaction to find moles of acid needed, and divide by the molarity of the sulfuric acid.
Step-by-step explanation:
To find the volume of sulfuric acid needed to react with 69.8 g of sodium hydroxide (NaOH), we can use stoichiometry and the molarity of the acid solution provided. The stoichiometric equation for the reaction between sulfuric acid (H2SO4) and sodium hydroxide is:
H2SO4 (aq) + 2NaOH(aq) → Na2SO4(aq) + 2H2O(l)
First, we need to calculate the moles of NaOH using its molar mass:
Moles of NaOH = mass (in g) / molar mass (in g/mol)
In this case:
Moles of NaOH = 69.8 g / (22.99 g/mol + 15.999 g/mol + 1.008 g/mol)
After finding the moles of NaOH, we multiply by the mole ratio from the balanced equation to find the moles of H2SO4 needed. Since 2 moles of NaOH react with 1 mole of H2SO4, we divide the moles of NaOH by 2 to get the moles of H2SO4.
Then, the volume of the sulfuric acid solution can be calculated using its molarity (M).
Volume of sulfuric acid (L) = moles of H2SO4 / molarity of H2SO4 (M)
Therefore, the exact volume can be found by plugging in the values from above into this final equation.