Final answer:
To neutralize the Ca(OH)2 solution, we can use the mole ratio from the balanced chemical equation to find the number of moles of HCl needed, and then calculate the volume of HCl required using its molarity. The volume of HCl needed is approximately 7.00 mL.
Step-by-step explanation:
To neutralize the Ca(OH)2 solution, we need to find the volume of HCl required. We can use the mole ratio from the balanced chemical equation to find the number of moles of HCl needed. Then, using the molarity of the HCl solution, we can calculate the volume of HCl needed:
Moles of HCl = Moles of Ca(OH)2 solution x Molarity of Ca(OH)2 solution
Volume of HCl = Moles of HCl / Molarity of HCl
By substituting the given values, we find that the volume of HCl needed is approximately 7.00 mL, so the answer is option c) 7.00 mL.
To calculate the volume of HCl needed to neutralize 10.5 mL of a saturated Ca(OH)2 solution, we must know the molarity of the Ca(OH)2. Without this, we cannot determine the correct volume of 1.20×10^(-3) M HCl required.
The volume of 1.20×10(-3) M HCl needed to neutralize 10.5 mL of a saturated Ca(OH)2 solution is dependent on the stoichiometry of the reaction between HCl and Ca(OH)2. The balanced chemical equation for this neutralization reaction is:
Ca(OH)2 + 2HCl → CaCl2 + 2H2O
Calcium hydroxide Ca(OH)2 dissociates into one Ca2+ and two OH- ions. Therefore, it requires two moles of HCl to neutralize one mole of Ca(OH)2. Thus, for every mole of Ca(OH)2 we need two moles of HCl. To calculate the volume of HCl needed, we first need to know the molarity of Ca(OH)2 solution, which is not provided in the question. If it was provided, we would calculate the number of moles of Ca(OH)2 in 10.5 mL, then double that to find the moles of HCl needed, and finally divide by the molarity of the HCl solution to find the volume.
As the molarity of Ca(OH)2 is not provided, a definitive answer cannot be given without more information.