Ch.12 - SolutionsWorksheetSee all chapters
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Ch.1 - Intro to General Chemistry
Ch.2 - Atoms & Elements
Ch.3 - Chemical Reactions
BONUS: Lab Techniques and Procedures
BONUS: Mathematical Operations and Functions
Ch.4 - Chemical Quantities & Aqueous Reactions
Ch.5 - Gases
Ch.6 - Thermochemistry
Ch.7 - Quantum Mechanics
Ch.8 - Periodic Properties of the Elements
Ch.9 - Bonding & Molecular Structure
Ch.10 - Molecular Shapes & Valence Bond Theory
Ch.11 - Liquids, Solids & Intermolecular Forces
Ch.12 - Solutions
Ch.13 - Chemical Kinetics
Ch.14 - Chemical Equilibrium
Ch.15 - Acid and Base Equilibrium
Ch.16 - Aqueous Equilibrium
Ch. 17 - Chemical Thermodynamics
Ch.18 - Electrochemistry
Ch.19 - Nuclear Chemistry
Ch.20 - Organic Chemistry
Ch.22 - Chemistry of the Nonmetals
Ch.23 - Transition Metals and Coordination Compounds
Sections
Solutions, Molarity and Intermolecular Forces
Henry's Law
Calculate Molarity
Mass Percent
Molality
Mole Fraction
The Colligative Properties
Additional Practice
Making Solutions
ppm
Boiling Point Elevation
Freezing Point Depression
Colloid
Additional Guides
The Freezing Point Depression
LearnAdditional Practice
Next SectionMole Fraction

Molality (m) represents the amount of solute dissolved per kilogram of solvent. 

Understanding Molality

Example #1:

Molality is depicted as moles of solute per kilograms of solvent.

 

Concept #1: Ionic molality or osmolality represents the molality of dissolved ions in a solution. 

 

Example #2:

A solution is prepared by dissolving 43.0 g potassium chlorate, KClO3, in enough water to make 100.0 mL of solution. If the density of the solution is 1.760 g/mL, what is the molality of KClO3 in the solution? MW of KClO3 is 122.55 g/mol. 

Molality Calculations

Example #3:

If the molality of glucose, C6H12O6, in an aqueous solution is 2.56 what is the molarity? Density of the solution is 1.530 g/mL.

 

Example #4:

What is the ionic molality of nitrate ions in 0.305 m lead (IV) nitrate, Pb(NO3)4?.

 

Practice: What is the mass percent of NH3 of a 1.25 m aqueous solution of NH3?

Previous SectionMass Percent
Next SectionMole Fraction
Additional Problems
Ethylene glycol (C2H6O2) is a common automobile antifreeze, dissolving in water to make a nonelectrolytic solution. A certain ethylene glycol solution is 40.0% by mass. What is the concentration of the solution in units of molality (m)?      
What mass (in g) of NH 3 must be dissolved in 475 g of methanol to make a 0.25 m solution? A) 2.02 g B) 4.94 g C) 1.19 g D) 8.42 g E) 1.90 g
A solution of 6.5% per weight H 2SO4 is dissolved in water. What is this concentration in molality? (Molar weight = 98 g/mol)   A. 2.3 m B. 0.71 m C. 4 x 10–14 m D. 0.02 m
How many grams of potassium nitrate (KNO3) do I need to dissolve in 800. g of water to prepare a 0.425 m KNO3 solution?
What is the molality (m) of a 1.25 M aqueous solution of sugar (C 6H12O6, 342.3 g/mol) which has a density of 1.14 g/mL? a) 0.742 molal b) 1.25 molal c) 0.614 molal d) 0.966 molal e) 1.76 molal
A solution of sucrose (C12H22O11 of MW 342 grams/mole) in benzene is 0.40 molal. The solution’s density is 0.90 grams/mL. How many milliliters of the solution would contain 0.10 moles of sucrose? 1. 444 mL 2. 316 mL  3. 250 mL 4. 360 mL 5. 225 mL
The molecular formula of Vitamin E (tocopherol is C29H50O2 (MW = 420.71). If the mole fraction of vitamin E in a methyl alcohol (CH3OH) solution is 0.002, what is the molality of the Vitamin E solution? a. none of the other answers is even close (within 10% error) b. 0.00273 c. 0.00503 d. 0.0625 e. 0.1570
What is the molality of an ascorbic acid solution made by dissolving 100.0 g of ascorbic acid, C6H8O6 (MW = 176.126 g/mol) in 750.0 g of water ( answers given in molal units)? a) 1.14 b) 0.032 c) 0.0046 d) 4.3 e) 0.757
What is the molality is an ascorbic acid solution made by dissolving 100.0 g of ascorbic acid, C6H8O6 (MW = 176.126 g/mol) in 750.0g of water (answers given in mole units)? a. 1.14 b. 0.032 c. 0.0046 d. 4.3 e. 0.757
An aqueous solution is 2.67 M in HNO 3 and has a density of 1.1064 g cm –3. Compute the molality of the HNO3 in this solution in mol/kg. a. 2.41 b. 2.97 c. 3.72 d. 2.32 e. 2.84
What is the molality of 150.0 g of NH 3 dissolved in a solution that is 1.25 Liters? The density of the solution is 1.45 g/mL. A. 4.86 B. 5.30 C. 7.04 D. 8.28 E. 12.0
What is the molality of 150.0 g of NH 3 dissolved in a solution that is 1.25 Liters? The density of the solution is 1.45 g/mL. A. 4.86 B. 5.30 C. 7.04 D. 8.28 E. 12.0 
Determine the molality of an aqueous solution prepared by dissolving 0.112 moles of LiCl in 13.7 moles of H 2 O. A) 0.122 m B) 0.454 m C) 0.220 m D) 0.818 m E) 0.153 m
How many grams of glucose (C6H12O6) must be dissolved in 563 g of ethanol (C2H5OH) to prepare a 2.40 x 10 -2 m solution? A. 2.43 g C6H12O6 B. 4.32 g C6H12O6 C. 0.000075 g C6H12O6 D. 437 g C6H12O6 E. 7.69  C6H12O6
Calculate the molality of a solution formed by dissolving 27.8 g of LiI in 500.0 mL of water. A) 0.394 m      B) 0.556 m      C) 0.241 m      D) 0.254 m      E) 0.415 m
Stock hydrochloric acid solution is 21.0% by mass HCl and has a specific gravity of 1.75. What is the molarity and molality of the solution?
A solution of sodium methoxide, NaOCH 3, in water has a mole fraction of 0.1750. What is the molality?
3.52 g NH4Cl (MW = 53.45 g/mol) is added to 12.4 g of water. Calculate the molality of ammonium chloride in the solution.  a) 5. 31 m b) 0.0872 m c) 15.2 m d) 15.2 x 103 m
What mass (in g) of NH­ 3 must be dissolved in 475 g of methanol to make a 0.250  m solution? a) 2.02 g   b) 4.94 g   c) 1.19 g   d) 8.42 g   e) 1.90 g
What mass of water is needed to dissolve 292.5 g of NaCl to produce a 0.25  m aqueous solution? Formula Molar Mass of NaCl is 58.5 g•mol –1. a) 20 kg b) 5.0 kg c) 0.80 kg d) 0.050 kg
A solution of ethanol, C2H6O, is prepared by dissolving 14.0 g C2H6O in 100.0 g water. (Molar mass ethanol = 46.07 g/mole) Find the molality of the solution.
Ethylene glycol (C2H6O2) is a common automobile antifreeze, dissolving in water to make a nonelectrolytic solution. A certain ethylene glycol solution is 30.0% by mass. What is the concentration of the solution in units of molality (m)?  
When 13.63 g (about one tablespoon) of table sugar (sucrose, C12H22O11) is dissolved in 241.5 mL of water (density 0.997 g/mL), the final volume is 250.0 mL (about one cup).What is the molality of the table sugar?
If you combine 25.1 g of a solute that has a molar mass of 25.1 g/mol with 100.0 g of a solvent, what is the molality of the resulting solution?
An aqueous NaCl solution is made using 126 g of NaCl diluted to a total solution volume of 1.15 L .Calculate the molality of the solution. (Assume a density of 1.08 g/mL for the solution.)
A solution is made containing 14.6 g of CH3 OH in 185 g H2 O.Calculate the molality of CH3 OH.
Calculate the molality of each of the following solutions.8.66 g benzene (C6 H6 ) dissolved in 23.5 g carbon tetrachloride (CCl4 )
Calculate the molality of each of the following solutions.4.80 g NaCl dissolved in 0.350 L of water
A sulfuric acid solution containing 571.5 g of H2 SO4 per liter of aqueous solution has a density of 1.329 g/cm3.Calculate the molality of H2 SO4 in this solution.
An aqueous solution contains 32% HCl by mass.Calculate the molality of the solution.
Brass is a substitutional alloy consisting of a solution of copper and zinc. A particular sample of red brass consisting of 81.0% Cu and 19.0% Zn by mass has a density of 8760 kg/m3 .What is the molality of Zn in the solid solution?
The figure shows two volumetric flasks containing the same solution at two temperatures.Does the molality of the solution change with the change in temperature?
Fluorocarbons (compounds that contain both carbon and fluorine) were, until recently, used as refrigerants. The compounds listed in the following table are all gases at 25 oC, and their solubilities in water at 25 oC and 1 atm fluorocarbon pressure are given as mass percentages. Fluorocarbon Solubility (mass %) CF4 0.0015 CClF3 0.009 CCl2F2 0.028 CHClF2 0.30 For CF4, calculate the molality of a saturated solution.
Fluorocarbons (compounds that contain both carbon and fluorine) were, until recently, used as refrigerants. The compounds listed in the following table are all gases at 25 oC, and their solubilities in water at 25 oC and 1 atm fluorocarbon pressure are given as mass percentages. Fluorocarbon Solubility (mass %) CF4 0.0015 CClF3 0.009 CCl2F2 0.028 CHClF2 0.30 For CClF3, calculate the molality of a saturated solution.
Fluorocarbons (compounds that contain both carbon and fluorine) were, until recently, used as refrigerants. The compounds listed in the following table are all gases at 25 oC, and their solubilities in water at 25 oC and 1 atm fluorocarbon pressure are given as mass percentages. Fluorocarbon Solubility (mass %) CF4 0.0015 CClF3 0.009 CCl2F2 0.028 CHClF2 0.30 For CCl2F2, calculate the molality of a saturated solution.
If an aqueous solution is very dilute, will its molality be greater than its molarity, nearly the same as its molarity, or smaller than its molarity?
Fluorocarbons (compounds that contain both carbon and fluorine) were, until recently, used as refrigerants. The compounds listed in the following table are all gases at 25 oC, and their solubilities in water at 25 oC and 1 atm fluorocarbon pressure are given as mass percentages. Fluorocarbon Solubility (mass %) CF4 0.0015 CClF3 0.009 CCl2F2 0.028 CHClF2 0.30 For CHClF2, calculate the molality of a saturated solution.
Acetonitrile (CH3 CN) is a polar organic solvent that dissolves a wide range of solutes, including many salts. The density of a 1.90 M LiBr solution in acetonitrile is 0.827 g/cm3 .Calculate the concentration of the solution in molality.
Glucose makes up about 0.10% by mass of human blood.Calculate the molality.
How much dry solute would you take to prepare each of the following solutions from the dry solute and the solvent?126 g of 0.505 m KCl
How much dry solute would you take to prepare each of the following solutions from the dry solute and the solvent?126 g of 0.220 m NaNO3
Calculate the number of moles of solute present in each of the following aqueous solutions.86.4 g of 0.180 m KCl,
Describe how you would prepare each of the following aqueous solutions, starting with solid KBr.130 g of 0.180 m KBr
What is the molality of a solution made by dissolving 38 g of C 10H8 in 425 g of C7H8? a. 0.546 mb. 12.3 mc. 0.998 md. 4.65 me. 0.698 m 
What mass (in g) of NH3 must be dissolved in 475 g of methanol to make a 0.250 m solution?
How many moles of KF are contained in 244 mL of 0.135 m KF solution?  The density of the solution is 1.22 g/mL
What is the molality of a 4.0 M NaOH solution? The density of the solution is 1.04 g/mL. In 1 L solution. a) 0.15 m b) 4.5 m c) 0.18 m d) 4.0 m e) 3.8 m
Molality from weight percent: What is the molality of an 18.0% aqueous solution of KCl?
What mass (in g) of NH3 must be dissolved in 475g of methanol to make a 0.250 m solution?
30 grams of liquid ethanol, CH3CH2OH, are mixed with 70 g water. The density of pure ethanol is 0.789 g/mL. The density of water is 1 g/mL. What is the molality of the ethanol in this solution?
Calculate the molality of total ions in an aqueous solution prepared by dissolving 0.400 moles of magnesium chloride in 850.0 g of water. A. 0.47 x 10-4 m B. 1.41 x 10-4 m C. 1.41 m D. 0.47 m E. 0.941 m
A 9.2 M perchloric acid (HClO 4) solution has a density of 1.54 g cm -3 at 25°C. Calculate the molality of the perchloric acid.a) 5.97b) 14.2c) 10.6d) 14.9e) none of the given answers
An aqueous solution is 2.67 M in HNO 3 and has a  density of 1.1064 g cm -3 . Compute the molality of the HNO3 in this solution in mol/kg.a) 2.42b) 2.97c) 3.72d) 2.32e) 2.84 
What is the molality of a 32.0% by weight aqueous solution of acetone (C  3H6O)?A. 8.10B. 7.80C. 7.12D. 6.56E. 5.74
An aqueous  solution is 2.67 M in HNO3 and has a density of 1.1064 g cm -3. Compute the molality of the HNO3 in this solution in mol/kg.a) 2.76b) 2.97c) 2.84d) 3.72e) 2.32
Which of the following statements is FALSE?a) The minority component of a mixture is called the soluteb) The majority component of a mixture is called the solventc) A diluted solution contains a relatively small amount of solute relative to solventd) The molarity of a solution is the moles of solute divided by liters of solvente) The molality of a solution is the moles of solute divided by kg of solvent
A solution was prepared by dissolving 39.0 g of KCl in 225 mL of water.  Calculate the molality of KCl in the solution.
What is the total ionic molality in an aqueous solution prepared by dissolving 0.200 moles of aluminum perchlorate, Al(ClO4)3 in 900.0 g water? 
Calculate the molality of a 23.0% by mass acetic acid, HC 2H3O2, solution. (molar mass = 60.05 g/mole)
What is the molality of naphthalene (C10H8) when 10.5 g of the compound are dissolved in 325 g of benzene (C6H6)? A. 0.252 m  B. 0.0819 m  C. 13.4 m  D. 32.3 m 
The molecular formula of Vitamin E (tocopherol) is C29H50O2 (MW = 430.71). If the mole fraction of vitamin E in a methyl alcohol (CH3OH) solution is 0.002, what is the molality of the Vitamin E solution?a) none of the other answers is even close (within 10% error )b) 0.00273c) 0.00503d) 0.0625e) 0.1570
What is the molality of a 10.6 % by mass glucose (C6H12O6) solution? (The density of the solution is 1.04 g/mL).
Derive a general equation that expresses the relationship between the molarity and the molality of a solution. Why are the numerical values of these two terms approximately equal for very dilute aqueous solutions?
The term proof is defined as twice the percent by volume of pure ethanol in solution. Thus, a solution that is 95% (by volume) ethanol is 190 proof. What is the molarity of ethanol in a 92 proof ethanol–water solution? Assume the density of ethanol, C2H5OH, is 0.79 g/cm3 and the density of water is 1.0 g/cm3.
A solution is prepared by dissolving 28.6 g of glucose (C6H12O6) in 360 g of water. The final volume of the solution is 380 mL. For this solution, calculate each of the following.Molality
Ascorbic acid (vitamin C, C6H8O6) is a water-soluble vitamin. A solution containing 81.5 g of ascorbic acid dissolved in 220 g of water has a density of 1.22 g/mL at 55oC.Calculate the molality of ascorbic acid in this solution.        
A solution is prepared by dissolving 20.2 mL of methanol (CH3OH) in 100.0 mL of water at 25 oC. The final volume of the solution is 118 mL. The densities of methanol and water at this temperature are 0.782 g/mL and 1.00 g/mL, respectively. For this solution, calculate each of the following.Molality
A solution is made containing 21.2 g phenol (C6H5OH) in 450 g ethanol (CH3 CH2OH).Calculate the molality of phenol.
What is the molality of a solution formed by dissolving 1.16 mol of KCl in 17.0 mol of water?
The density of toluene (C7H8) is 0.867 g/mL, and the density of thiophene (C4H4S) is 1.065 g/mL. A solution is made by dissolving 8.60 g of thiophene in 260 mL of toluene.Calculate the molality of thiophene in the solution.
Calculate the molality of the following: (a) A solution containing 85.4 g of glycine (NH2CH2COOH) dissolved in 1.270 kg of H2O
Calculate the molality of the following:(b) A solution containing 8.59 g of glycerol (C3H8O3) in 77.0 g of ethanol (C2H5OH)
Calculate the molality of the following: (a) A solution containing 174 g of HCl in 757 g of H2O
Calculate the molality of the following:(b) A solution containing 16.5 g of naphthalene (C10H8) in 53.3 g of benzene (C6H6)
Solutions of hydrogen in palladium may be formed by exposing Pd metal to H2 gas. The concentration of hydrogen in the palladium depends on the pressure of H2 gas applied, but in a more complex fashion than can be described by Henry’s law. Under certain conditions, 0.94 g of hydrogen gas is dissolved in 215 g of palladium metal (solution density = 10.8 g cm3).(b) Determine the molality of this solution.
The three aqueous ionic solutions represented below have total volumes of 25. mL for A, 50. mL for B, and 100. mL for C. If each sphere represents 0.010 mol of ions, calculate:(c) the lowest molality of solute (assuming the solution densities are equal);
What is the molality of a solution consisting of 44.0 mL of benzene (C6H6; d = 0.877 g/mL) in 167 mL of hexane (C6H14; d = 0.660 g/mL)?
What is the molality of a solution consisting of 2.66 mL of carbon tetrachloride (CCl4; d = 1.59 g/mL) in 76.5 mL of methylene chloride (CH2Cl2; d = 1.33 g/mL)?
How would you prepare the following aqueous solutions?(a) 3.10×102 g of 0.125 m ethylene glycol (C2H6O2) from ethylene glycol and water
A solution contains 22.4 g glucose (C6H12O6) dissolved in 0.500 L of water. What is the molality of the solution? (Assume a density of 1.00 g/mL for water.)
A solution contains 0.35 mol of isopropanol (C3H7OH) dissolved in 0.85 mol of water.(c) The molality?
What is the difference between a 1 M solution and a 1 m solution?
What is the molality of phosphoric acid, H3PO4, in a solution of 14.5 g of H3PO4 in 125 g of water?(a) Outline the steps necessary to answer the question.(b) Answer the question.
What is the molality of nitric acid in a concentrated solution of nitric acid (68.0% HNO3 by mass)?(a) Outline the steps necessary to answer the question.(b) Answer the question.
Calculate the molality of each of the following solutions:(a) 583 g of H2SO4 in 1.50 kg of water—the acid solution used in an automobile battery
Calculate the molality of each of the following solutions:(b) 0.86 g of NaCl in 1.00 × 102 g of water—a solution of sodium chloride for intravenous injection
Calculate the molality of each of the following solutions:(c) 46.85 g of codeine, C18H21NO3, in 125.5 g of ethanol, C2H5OH
Calculate the molality of each of the following solutions:(d) 25 g of I2 in 125 g of ethanol, C2H5OH
A solution contains 0.100 mol of NaCl dissolved in 8.60 mol of water.(c) The molality?
Calculate the molality of each of the following solutions:(a) 0.710 kg of sodium carbonate (washing soda), Na2CO3, in 10.0 kg of water—a saturated solution at 0°C
Calculate the molality of each of the following solutions:(b) 125 g of NH4NO3 in 275 g of water—a mixture used to make an instant ice pack
Suppose you take a solution and add more solvent, so that the original mass of solvent is doubled. You take this new solution and add more solute, so that the original mass of the solute is doubled. What happens to the molality of the final solution, compared to the original molality?
Calculate the molality of each of the following solutions:(c) 25 g of Cl2 in 125 g of dichloromethane, CH2Cl2
An automobile antifreeze mixture is made by mixing equal volumes of ethylene glycol (d = 1.114 g/mL; ℳ = 62.07 g/mol) and water (d = 1.00 g/mL) at 20°C. The density of the mixture is 1.070 g/mL. Express the concentration of ethylene glycol as:(d) Molality
An aqueous KNO3 solution is made using 77.6 g of KNO3 diluted to a total solution volume of 1.96 L. (Assume a density of 1.05 g/mL for the solution) Calculate the molality of the solution.
Calculate the molality of each of the following solutions:(d) 0.372 g of tetrahydropyridine, C5H9N, in 125 g of chloroform, CHCl3
The concentration of glucose, C6H12O6, in normal spinal fluid is 75 mg/100 g . What is the molality of the solution?
An aqueous solution contains 4.6 % NaCl by mass. Calculate the molality of the solution.
A 13.0% solution of K2CO3 by mass has a density of 1.09 g/cm3. Calculate the molality of the solution.
A solution is prepared by dissolving 50.5 g sucrose (C12H22O11) in 0.404 kg of water. The final volume of the solution is 355 mL. For this solution, calculate molality.
How would you prepare 250. g of 0.150 m aqueous NaHCO3?
How many grams of sulfur (S8) must be dissolved in 100.0 g naphthalene (C10H8) to make a 0.13 m solution?
Calculate the number of moles of solute present in 55.0 mg of an aqueous solution that is 1.55 m NaCl. Assume that for dilute aqueous solutions, the mass of the solvent is the mass of solution.
Describe how you would prepare each of the following aqueous solutions.Give the mass of the solute and mass of the solvent for 230 g of a solution that is 0.70 m in Na2 CO3, starting with the solid solute.
In lab you need to prepare at least 100 mL of each of the following solutions. Explain how you would proceed using thegiven information. a. 2.0 m KCl in water (density of H2O = 1.00 g/cm3)
Calculate the molality of each of the following solutions:a. 0.700 mol of glucose in 1.50 kg of waterb. 29.5 mmol of acetic acid in 65.0 g of waterc. 1.25 mol of baking soda (NaHCO3) in 290.0 g of water
A concentrated aqueous solution of sulfuric acid (H2SO4) has a density of 1.509 g/mL and contains 61% sulfuric acid by mass. Calculate the molality of sulfuric acid. a) 66 b) 9.4 c) 16 d) 0.62
Calculate the molality of each of the following aqueous solutions. (a) 1.85 M NaCl solution (density of solution = 1.08 g/mL): (b) 37.5 percent by mass KBr solution:
8.90 g of NH4Cl is added to 17.4 g of water. Calculate the molality of the solution. 
Be sure to answer all parts.Calculate the molality of each of the following solutions:(a) 25.7 g of sucrose (C12H22O11) in 717 g of water, (b) 6.57 moles of ethylene glycol (C2H6O2) in 3483 g of water.
Concentrated aqueous sodium hydroxide, NaOH(aq), is sold commercially as a 14.30 M solution with a density of 1.430 g/mL. What is the concentration of this solution in molality? (A) 20.25 m (B) 16.67 m(C) 12.92 m (D) 14.77 m (E) 18.35 m
What is the mole fraction, X, of solute and the molality, m (or b), for an aqueous solution that is 100% NaOH by mass? 
Calculate the molality of a solution formed by dissolving 27.8 g of Lil in 500 0 mL of water.(i) 0.254 m (ii) 0.241 m (iii) 0.556 m (iv) 0.394 m (v) 0.415 m
What is the molality of the solution when 49.0 g H 2SO4 is dissolved in 150 g of water?
Be sure to answer all parts.Calculate the molality of each of the following aqueous solutions. (a) 2.30 M NaCl solution (density of solution = 1.08 g/mL): (b) 36.7 percent by mass KBr solution: 
Enter your answer in the provided box.Determine the molality of an aqueous solution that is 12.0 percent urea by mass.
An aqueous solution of barium nitrate has a concentration of 5.84 x 10-2 molal. The percent by mass of barium nitrate in the solution is ____________ %.
What is the mole fraction, X, of solute and the molality, m (or b), for an aqueous solution that is 11.0% NaOH by mass?
Calculate the osmolarity of a solution prepared by dissolving 6.53 grams of NiCl2 (M.W. = 129.6 g/mole) in water to give 250.0 mL of solution. 
What is the molality of a solution that has been prepared by mixing 50.0 g of sodium chloride with 500 g of water? a. 1.14 m b. 1.21m c. 1.48 m d. 1.59 m e. 1.71m
Lauryl alcohol, C12H25OH, is prepared from coconut oil. It is used to make sodium lauryl sulfate, a synthetic detergent. What is the molality of lauryl alcohol in a solution of 12.4 g lauryl alcohol dissolved in 165 g ethanol, C2H5OH? Molality = m
The density of a 20.3 M CH 3OH (methanol) solution is 0.858 g/mL. What the molality of this solution? H2O is the solvent. 20.8 m 978 m 174 m 23.7 m 700 m
Question 3 What is the molality of 3.04 g of sodium nitrate in 12.19 g water? The molar mass of sodium nitrate is 84.99 g/mol. (Enter only the numerical answer.) Question 4 Calculate the percent water in a 1.28 molal solution of ammonium perchlorate (molar mass 117.49 g/mol).
Be sure to answer all parts. Calculate the molality of each of the following solutions: (a) 19.1 g of sucrose (C12H22O11) in 745 g of water, (b) 8.05 moles of ethylene glycol (C2H6O2) in 3175 g of water.
Be sure to answer all parts.Calculate the molality of each of the following aqueous solutions. (a) 2.95 M NaCl solution (density of solution = 1.08 g/mL) (b) 52.5 percent by mass KBr solution 
A solution is 0.0433 m LiF. What is the molarity of the solution if the density is 1.10 g/mL? (i) 0.0390 M (ii) 0.0476 M (iii) 0.0519 M (iv) 0.0417M (v) 0.0441 M
520 g of CaCO3 is dissolved in 5 kg of water. What is the molality of the solution?• 26 m• 1.04 m• 104 m
The density of a 4.500% by mass aqueous solution of potassium sulfate, K2SO4, is 1.0370 g/mL. The molar mass of potassium sulfate is 174.3 g/mol. A. What is the molarity of the solution? B. What is the molality of the solution? C. What is the mole fraction of potassium sulfate?
At 20°C, a 0.376 M aqueous solution of ammonium chloride (NH 4Cl) has a density of 1.0045 g/mL. What is the molality of NH4Cl in the solution?A. 0.774B. 2.68C. 0.385D. 0.00710E. 2.00
Your lab partner combined Xchloroform (CHCl3) and acetone (C3H6O) to create a solution where the mole fraction of chloroform, Xchloroform is 0.187. The densities of chloroform and acetone are 1.48 g/mL and 0.791 g/mL, respectively Calculate the molarity of the solution.  Calculate the molality of the solution.