Final answer:
The molarity of KMnO₄ in a solution made by dissolving 0.0946 g of KMnO₄ in 0.475 l of solution is 1.26 x 10⁻³ M, calculated by dividing the number of moles of KMnO₄ by the volume of the solution.
Step-by-step explanation:
To calculate the molarity of a KMnO₄ solution, we first need to determine the molar mass of KMnO₄. The molar mass is the sum of the atomic masses of potassium (K), manganese (Mn), and four oxygen (O) atoms, which is approximately 39.10 (K) + 54.94 (Mn) + 4 × 16.00 (O) = 158.04 g/mol. With this information, we can calculate the number of moles of KMnO₄ in the solution:
Number of moles (mol) = mass (g) / molar mass (g/mol)
Number of moles = 0.0946 g / 158.04 g/mol
Number of moles = 5.987 × 10⁻´ moles
Now, to find the molarity, we divide the number of moles by the volume of the solution in liters:
Molarity (M) = moles of solute / volume of solution (L)
Molarity = 5.987 × 10⁻´ moles / 0.475 L
Molarity = 1.26 × 10⁻³ M
Therefore, the molarity of the KMnO₄ solution is 1.26 x 10⁻³ M.