How to Prepare a 0.530 M Ca(OH)2 Solution?
What is the total volume of the solution formed by dissolving 36.0 grams of Ca(OH)2 in enough water to get a 0.530 M solution?
a) 0.720 liters
b) 0.917 liters
c) 1.03 liters
d) 1.21 liters
Final Answer:
The total volume of the solution formed by dissolving 36.0 grams of Ca(OH)2 in enough water to get a 0.530 M solution is 0.917 liters.
Explanation: To prepare a 0.530 M Ca(OH)2 solution, we need to dissolve 36.0 grams of Ca(OH)2 in enough water. The total volume of the solution can be calculated using the formula for molarity.
First, we need to calculate the number of moles of Ca(OH)2 in 36.0 grams. The molar mass of Ca(OH)2 is approximately 74.1 g/mol. Therefore, the number of moles of Ca(OH)2 is 36.0 g ÷ 74.1 g/mol = 0.486 moles.
Given that the molarity of the solution is 0.530 M, we can use the formula for molarity (M = moles of solute / volume of solution in liters) to calculate the total volume of the solution. Rearranging the formula, we get volume of solution = moles of solute / molarity, which gives us 0.486 moles / 0.530 M = 0.917 liters.
Therefore, to prepare a 0.530 M Ca(OH)2 solution, you would need to dissolve 36.0 grams of Ca(OH)2 in enough water to make a total volume of 0.917 liters. Enjoy your chemistry experiment!