Section 13.2 Review A Molecular View of the Solution Process 12.1 3.2.2 or a bod

Question

Section 13.2 Review A Molecular View of the Solution Process 12.1 3.2.2 or a body Which of the following compounds do you expect to be more sol water? (Select all that appl ) SO, CO. Na, SO, CH.. Brl n Which of the Following compounds dissolved in water would berween the solute and solve? H, CH,OH, CO, NH, NaC Worked Exam vy Worked 13.3 CONCENTRATION UNITS of solutions in units of The d Recall that molarity, M is defined as the number of moles of solute din of solution I section 9.5]. of moles of solute divided by the (a) molality, We learned in Chapter 9 that chemists often express concentration moles of solute molarity -Mliters of solution the molality to calculate the total nun Male fation a which i kefinod as he aunbr of msoles f solute divided by Setup Th Solution moles, is also an expression of concentration [tt Section 11.7 moles of A mole fraction of component A sum of moles of all components dmicribe the In this section, we will learn about molaliry and pencent by mass, two additional ways to expres lluse pescent by the concentration of a mixture component. How a chemist expresses concentrationpro type of problem being solved Molality Molality (m) is the number of moles of solute dissolved in I kg (1000 g) of solvent: moles of solute mass of solvent (in kg) molalitym nd molality For example, to prepare a I molal (I-m) aqueous sodium sulfate solution, we must dissolve I mole (1420 g) of Na,SO, in I kg of water Thin Pay kilo the mau of Percent by Mass The percent by mass (also called percent by weight) is the ratio of the mass of a solute to the mass of the solution, multiplied by 100 percent. Because the units of mass cancel on the top and botom of the fraction, any units of mass can be used provided they are used consistently: Pr Equation 13.2 percent by mass mass of solute mass of solute + mass of solvent ×100% For example, we can express the concentration of the 1-m aqueous sodium sulfate solution as percent by mass Na,SO mass of Na SO mass of Na SO, +mass of water 100% 142.0 g 11420g × 100% 12.4% The term percen liteally means "parts per bundred" If we were to use Equation 13.2 but molid's by 1000 instead of 100, we would get" parts per thousand; multiplying by 1,000 parts per millon" or ppm: and so on. Parts per million, parts per bilion, parts per tillio would give

Explanation / Answer

mass of Na2SO4 + mass of H2O:

mass of Na2SO4 = 142.0 g

mass of solvent that is water = 1 L = 1000 mL ( mass of solvent must be 1 kg for 1 m solution. 1 kg os water = 1 L of water as the density of water is 1.00. so the mass of solvent(H2O) = 1 L = 1000 mL)

Therefore, mass of Na2SO4 + mass of H2O = 142.0 + 1000 = 1142.0 g

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