- Joined
- Jul 15, 2015
- Messages
- 73
- Reaction score
- 16
(From AAMC FL1 C/P #58)
What volume of a 0.120 M CaI2 solution would contain 0.078 mol of SOLUTE?
Easy enough: 0.120 mol/L = 0.078 mol/xL
xL = 0.650 L
(Next-Step Science Diagnostic)
72g NH4Cl is dissolved in 1kg H2O. What is the molality of the resulting solution?
Molality = Moles of Solute / Mass of Solvent
72g NH4Cl = 1.35 mol >>> 1.35 mol NH4Cl / 1kg H2O = 1.35 m
BUT
NS is saying Moles of Solute = Moles of Ions:
1.35 Mol NH4CL >>> 1.35 mol NH4 + 1.35 mol Cl = 2.7 mol Solute
Molality = 2.7 mol/1 kg H2O = 2.7 m
When do we use Mol of Ions vs Mol of Solute? Both would ionize in solution so I'm confused...
What volume of a 0.120 M CaI2 solution would contain 0.078 mol of SOLUTE?
Easy enough: 0.120 mol/L = 0.078 mol/xL
xL = 0.650 L
(Next-Step Science Diagnostic)
72g NH4Cl is dissolved in 1kg H2O. What is the molality of the resulting solution?
Molality = Moles of Solute / Mass of Solvent
72g NH4Cl = 1.35 mol >>> 1.35 mol NH4Cl / 1kg H2O = 1.35 m
BUT
NS is saying Moles of Solute = Moles of Ions:
1.35 Mol NH4CL >>> 1.35 mol NH4 + 1.35 mol Cl = 2.7 mol Solute
Molality = 2.7 mol/1 kg H2O = 2.7 m
When do we use Mol of Ions vs Mol of Solute? Both would ionize in solution so I'm confused...