Question

What volume of 1.75x10^-3 M HCl is needed to neutralize 13.5 mL of saturated Ca(OH)2 solution?

A) 15.43 mL
B) 12.77 mL
C) 18.22 mL
D) 14.88 mL

Answer 1

To find the volume of 1.75x10^-3 M HCl to neutralize 13.5 mL of Ca(OH)2, the moles of Ca(OH)2 need to be calculated, doubled (for the 2:1 reaction ratio), and then divided by the molarity of HCl. Exact volume calculation would require the molarity or mass of Ca(OH)2.

Step-by-step explanation:

To determine the volume of 1.75x10-3 M HCl needed to neutralize 13.5 mL of saturated Ca(OH)2 solution, we must first write the balanced chemical equation for the reaction between HCl and Ca(OH)2:

Ca(OH)2(aq) + 2 HCl(aq) → CaCl2(aq) + 2 H2O(l)
From the equation, we can see that it takes 2 moles of HCl to neutralize 1 mole of Ca(OH)2. Assuming the Ca(OH)2 is saturated, we can find the moles of Ca(OH)2 in 13.5 mL. Next, we double that number to find the moles of HCl needed since it is a 2:1 ratio. We then use the molarity of HCl to calculate the volume of HCl required to supply that number of moles. Without the molarity or mass of the Ca(OH)2, we cannot calculate the exact volume of HCl needed. Given more information, the calculation would follow this format:

• Calculate moles of Ca(OH)2 present in 13.5 mL of saturated solution.
• Multiply by 2 to find moles of HCl required.
• Use the moles of HCl and its molarity (1.75x10-3 M) to find the volume.