SrCl2 => Sr^2+ + 2Cl^-
m = mols solute/kg solvent
If SrCl2 is 0.15 m then
Sr^2+ must be 0.15 m and Cl^- must be 0.30 m
*Consider a 0.15 m strontium chloride aqueous solution.
a. Determine the molality (in m) of all solutes in the solution. Assume that strontium chloride completely ionizes when dissolved in water. All solutes means all cations and anions. The molality that you determine here is the value for m solute. You must explain your answer.
2 answers
What is your formula for this?
1 answer