A stock solution of potassium permanganate (KMnO4) was prepared by dissolving 11.3 g KMnO4 with DI H2O in a 100.00-mL volumetric flask and diluting to the calibration mark. Determine the molarity of the solution.

[KMnO₄] = 0.71 M

Explanation:

Solute: Potassium permanganate, molar mass 158.04 g/mol

Solvent: Water, volume of 100 mL

We convert the mass of solute to moles:

11.3 g . 1mol / 158.04g = 0.071 moles

We asume the solvent's volume as the solution's volume

We convert the volume from mL to L → 100 mL . 1L / 1000 mL = 0.1L

Molarity (mol/L) → moles of solute in 1L of solution

Molarity → 0.071 moles / 0.1 L = 0.71M

for points guys

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.