For a binary solution composed of components 1 and 2, we can represent the mass percent of component 2 as A2. The solution is composed of nTotal moles. Component 1 has a molar mass of M1 and component 2 has a molar mass of M2.       a) In terms of A2, what is the mass percent of component 1?       b) Derive an expression for the mole fraction of component 2, x2, in              terms of A2.       c) Derive an expression for the mole fraction of component 1, x1, in            terms of A2.        d) For an aqueous solution, we can define component 1 as water and             component 2 as our solute. The density of the solution, ρ, can be             thought of as a function that depends on A2. We denote this as             ρ(A2) – which is just a notation like f(x) and does not mean ρ*A2.             Show that the total volume of the solution is given by:              V = (n1M1 + n2M2) / (ρ*A2)

Colligative properties are those that depend on the number of solute particles. Because electrolytes dissociate into ions, the concentration of particles in the solution is greater than the formula-unit concentration of the solution. For example, if 1 mol of NazSO4 totally dissociates, 3 mol of ions are produced (2 mol of Nat ions and 1 mol of SO, ions). Thus, a colligative property such as osmotic pressure will be three times greater for a 1 M NazSO, solution than for a 1 M nonelectrolyte solution. Part A Assuming complete dissociation of the solute, how many grams of KNO3 must be added to 275 mL of water to produce a solution that freezes at - 14.5 °C? The freezing point for pure water is 0.0 °C and Kf is equal to 1.86 °C/m. Express your answer to three significant figures and include the appropriate units. • View Available Hint(s) However, complete dissociation of electrolytes does not always occur. The extent the van't Hoff factor, i: dissociation is expressed by HA moles of…

A mixture is prepared by mixing 29.27 mL of the blue dye solution with 35.00 mL of the red dye solution and 14.73 mL of the yellow dye solution. What is the molar concentration of the blue dye in the mixture? Dye stock solution   Concentration, M Blue   0.3523 Yellow   0.1542 Red   0.1017

A student dissolves 1.9 g of styrene (C,H,) in 150. mL of a solvent with a density of 1.02 g/mL. The student notices that the volume of the solvent does not change when the styrene dissolves in it. Calculate the molarity and molality of the student's solution. Be sure each of your answer entries has the correct number of significant digits. molarity = x10 molality 미□