Final answer:
To find the volume of K₂C₂O₄ required to react with Ba(OH)₂ and form BaC₂O₄, we need to use the stoichiometry of the reaction and relate it to the given mass of BaC₂O₄. By calculating the moles of K₂C₂O₄ and then using the molarity, we can find the volume in milliliters.
Step-by-step explanation:
To find how many ml of 1.248 M K₂C₂O₄ are required to react with excess Ba(OH)₂ and form 58.37 g BaC₂O₄, we need to use the balanced chemical equation and the stoichiometry of the reaction.
From the balanced equation:
1 mole of K₂C₂O₄ reacts with 1 mole of Ba(OH)₂ to form 1 mole of BaC₂O₄.
To find the amount in moles of K₂C₂O₄, we can use the equation:
Moles = Molarity x Volume (in liters).
Since we are looking for the volume in milliliters, we can rearrange the equation:
Volume (in mL) = Moles / Molarity.
Using the molar mass of K₂C₂O₄, we can find the moles of K₂C₂O₄ needed to react with 58.37 g of BaC₂O₄. Finally, we can substitute this value into the rearranged equation to find the volume in milliliters.