How many liters of 0.85 M HCl solution would react completely with 3.5 moles Ca(OH)2?
you need 7 moles of HCl for a complete reaction
7 moles / .85 M/L =
To determine the volume of 0.85 M HCl solution required to react completely with 3.5 moles of Ca(OH)2, we can use the balanced chemical equation for the reaction between HCl and Ca(OH)2:
2HCl + Ca(OH)2 → CaCl2 + 2H2O
From the balanced equation, we can see that it takes 2 moles of HCl to react with 1 mole of Ca(OH)2. Therefore, the ratio of moles of HCl to Ca(OH)2 is 2:1.
In this case, we have 3.5 moles of Ca(OH)2. Since the ratio of HCl to Ca(OH)2 is 2:1, we can calculate the moles of HCl needed by dividing the moles of Ca(OH)2 by 2:
Moles of HCl = 3.5 moles Ca(OH)2 / 2 = 1.75 moles HCl
Now, we need to use the molarity of the HCl solution (0.85 M) to find the volume of the solution needed. The equation for finding the volume is:
Volume (Liters) = Moles / Molarity
Plugging in the values:
Volume of HCl solution = 1.75 moles / 0.85 M
Volume of HCl solution ≈ 2.059 liters or 2.06 liters (rounded to two decimal places)
Therefore, approximately 2.06 liters of 0.85 M HCl solution would react completely with 3.5 moles of Ca(OH)2.