How many milliliters of 0.005 M Ca(OH)2 solution are required to neutralize 10.0 mL of the HCl?
The balanced reaction will be
Ca(OH)2 + 2HCl --------- CaCl2 + 2H2O
The data is incomplete, molarity of HCl is missing in the problem
Let the molarity of HCl be P
number of moles of HCl = Volume of HCl (in L) *Molarity = 0.01P
number of moles of Ca(OH)2 required = 1/2 * number of moles of HCl = 0.005P
0.005M * Volume of Ca(OH)2 (in L) =0.005P
Volume of Ca(OH)2 in L = P, where P is the molarity of HCl solution missing in problem
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