Step-by-step explanation:
To calculate the molarity of the proposed solution, we need to know the mass of potassium permanganate (KMnO4) and the volume of the solution in liters.
First, we need to convert the volume of the solution from milliliters (mL) to liters (L):
500 mL = 500/1000 = 0.5 L
Next, we need to calculate the molarity (M) using the equation:
Molarity (M) = moles of solute / volume of solution (in L)
Given that there are 0.35 moles of KMnO4, we can substitute the values into the equation:
M = 0.35 moles / 0.5 L
M = 0.7 M
Therefore, the molarity of the proposed solution is 0.7 M.
To determine if the proposed solution can actually be prepared, we need to consider the solubility of potassium permanganate (KMnO4) in water. If the solubility of KMnO4 is less than 0.7 M, it will not be possible to dissolve 0.35 moles of KMnO4 in 500 mL of solution.
The solubility of KMnO4 in water at room temperature is about 6.4 g/100 mL of water. To calculate the maximum molarity, we need to convert grams to moles and volume to liters:
6.4 g/100 mL * (1 mole KMnO4 / molar mass KMnO4) * (10 mL/ 1 L) = approximately 0.096 M
The maximum molarity of KMnO4 in water is approximately 0.096 M, which is lower than the proposed molarity of 0.7 M. Therefore, it is not possible to dissolve 0.35 moles of KMnO4 into 500 mL of solution.