will the molarity be larger or smaller than 1.0? explain?

Question

suppose a 1.0 m solution of solute is made using a solvent w/ a density of 1.15g/mL

lower case m stands for molality

Answer 1

1 m is 1 mole of solute/ Kg of solvent.
You say that for the solvent d=m/V=1.15=>
Vsolvent=m/d=1000/1.15 mL= 1/1.15 L

But the Molarity is M= mole/Vsolution

Assuming that Vsolution=Vsolvent

Molarity = mole/Vsolvent= 1/(1/1.15)= 1.15 M. So it is larger.

If there is a big change in th volume upon dissolving the solute, then an increase in volume would make the Molarity even larger while a decrease would bring Molarity closer to molality.

Answer 2

I don't think molarity is dependent on the density of the solute. In a 1.0 M solution, you'd still have 1 mole per liter regardless of the density of the solution. Density is simply mass/volumeratio of the solute itself and is independent of molarity, which is a ratio of how many moles of the solute are dissolved in the (already prepared) solvent.

Answer 3

assume 1 mol in 1Kg or 1000g solvent. Molarity is mol solute per liter of solution(solute + solvent). The answer will absolutely depend on the solute's mass - but commonly Molarity is larger: A small solute LiF (26g/mol) means: total mass solution = 1026g solution = 892mL =0.892L so M=(1/.892)=1.12; A larger solute - glucose (180g/mol) means: total mass =1180g solution = 1026mL = 1.026L so M=(1/1.026)=0.974M