Determine how many milliliters of 0.448 M HClO4 will be required to neutralize 38.30 g Ca(OH)2 according to the reaction: 2HCl+Ca(ClO4)2+2H20

Answer 1

You need to start from a balanced equation

HClO4 + Ca(OH)2 -> Ca(ClO4)2 + H20

which you need to balance

2HClO4 + Ca(OH)2 -> Ca(ClO4)2 + 2H20

then work out how many moles 38.30 g Ca(OH)2 represents from

number of moles = 38.30 g/molar mass

from the equation 2 mole of HClO4 needed for each mole of Ca(OH)2

hence calcutae the number of moles of HClO4 needed.

ml of HClO4 needed is then

number of moles x 1000/(0.448 mole L^-1)