Question 1c

Question 3a

Question 2a

A solution has a boiling point elevation of 0.768 °C. Kb water = 0.512 °C/m, i = 1.What is the molality? A.0.50 mB. 1.00 mC. 1.50 mD. 2.00 m ΔTb​=i⋅Kb​⋅m ​ ​

Question 2d

Question 4a

Question 1a

What is the van’t Hoff factor (i) for Al₂(SO₄)₃ assuming complete dissociation? A.3B. 4C. 5D. 6

A solution contains 15.0 g of KBr (119.0 g/mol) dissolved in 200.0 g of water. Calculate ΔTb. (Kb water = 0.512 °C/m, assume complete dissociation) A.0.323 °CB. 0.646 °CC. 0.161 °CD. 0.512 °C ​moles = mass (g) ÷ molar mass (g/mol) m = moles of solute ÷ kilograms of solvent   ΔTb​=i⋅Kb​⋅m

What mass of ethylene glycol (62.07 g/mol, i = 1) is needed to lower the freezing point of 500.0 g of water by 2.00 °C? Kf water = 1.86 °C/m A.16.7 gB. 33.4 gC. 62.1 gD. 124 g ΔTf​=i⋅Kf​⋅m m=i⋅Kf​ΔTf m = moles of solute ÷ kilograms of solvent Mass=moles⋅M ​​