#11 Key
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The document contains a chemistry problem set with 10 questions: 1) It asks to calculate the molarity of three aqueous solutions. 2) It asks to calculate the percentage by mass of nitric acid in a 16 M commercial solution. 3) It asks to calculate the osmotic pressure of a solution formed by dissolving aspirin in water. 4) It asks to order solutions by increasing boiling point. 5) It defines hydrophobic and hydrophilic colloids and provides examples. 6) It asks to identify colloids as hydrophobic or hydrophilic.
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#10 Key
This document provides definitions and examples of key concepts in general chemistry including:
1. Solvation refers to the attractive interaction between solvent molecules and a solute. Hydration describes the interaction when water is the solvent.
2. The overall enthalpy change of a solution can be either positive (endothermic) or negative (exothermic).
3. A saturated solution is one in equilibrium with undissolved solute where dissolution and crystallization occur at equal rates. Unsaturated and supersaturated solutions contain less or more solute respectively.
4. Colligative properties include vapor pressure depression, freezing point depression, boiling point elevation, and osmotic pressure.
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Solubility and mixtures.pptx
This document provides an overview of solutions and related concepts in chemistry. It defines key terms like mixtures, solutions, solutes, solvents, concentration, solubility, and factors that affect solubility. It also discusses homogeneous and heterogeneous mixtures, concentration in terms of molarity and percent by mass, and how to perform calculations involving dilution of solutions and solution stoichiometry. The document uses examples and diagrams to illustrate these concepts.
#22 Key
1. An object can possess energy through kinetic energy from its motion or potential energy from its position. Kinetic energy depends on mass and velocity while potential energy depends on position.
2. A kilowatt-hour equals 3.6 million joules. An adult radiates heat at the same rate as a 100-watt bulb, so in 24 hours they radiate about 2.1 kilocalories of heat energy.
3. Chemical reactions that release heat are exothermic, while those that absorb heat are endothermic. Heat change equals internal energy change during constant pressure processes.
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Chemistry of solutions
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#19 key
1. 18.9 grams of K2Cr2O7 are present in 50.0 mL of 0.360 M K2Cr2O7 solution.
2. The molarity of the (NH4)2SO4 solution formed from dissolving 4.28 grams of (NH4)2SO4 in 300 mL of water is 0.108 M.
3. 58.7 mL of 0.240M CuSO4 solution contains 2.25 grams of CuSO4 solute.
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This experiment aims to determine the total hardness of drinking water using a complexometric titration with EDTA. The standardization of EDTA is performed using a calcium carbonate standard. Reactions involving the calcium-EDTA and magnesium-EDTA complexes are discussed. The addition of magnesium chloride is meant to create a sharper titration endpoint but the amount added was insignificant compared to the EDTA. Analysis of a water sample from Viva found it to have a total hardness of 192.49 ppm CaCO3, which is 25.8% lower than the value claimed.
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#10 Key
This document provides definitions and examples of key concepts in general chemistry including:
1. Solvation refers to the attractive interaction between solvent molecules and a solute. Hydration describes the interaction when water is the solvent.
2. The overall enthalpy change of a solution can be either positive (endothermic) or negative (exothermic).
3. A saturated solution is one in equilibrium with undissolved solute where dissolution and crystallization occur at equal rates. Unsaturated and supersaturated solutions contain less or more solute respectively.
4. Colligative properties include vapor pressure depression, freezing point depression, boiling point elevation, and osmotic pressure.
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The document outlines topics covered in General Chemistry II for week 4, including:
1) Expressing concentration of solutions using various units
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#22 Key
1. An object can possess energy through kinetic energy from its motion or potential energy from its position. Kinetic energy depends on mass and velocity while potential energy depends on position.
2. A kilowatt-hour equals 3.6 million joules. An adult radiates heat at the same rate as a 100-watt bulb, so in 24 hours they radiate about 2.1 kilocalories of heat energy.
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#19 key
1. 18.9 grams of K2Cr2O7 are present in 50.0 mL of 0.360 M K2Cr2O7 solution.
2. The molarity of the (NH4)2SO4 solution formed from dissolving 4.28 grams of (NH4)2SO4 in 300 mL of water is 0.108 M.
3. 58.7 mL of 0.240M CuSO4 solution contains 2.25 grams of CuSO4 solute.
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This experiment aims to determine the total hardness of drinking water using a complexometric titration with EDTA. The standardization of EDTA is performed using a calcium carbonate standard. Reactions involving the calcium-EDTA and magnesium-EDTA complexes are discussed. The addition of magnesium chloride is meant to create a sharper titration endpoint but the amount added was insignificant compared to the EDTA. Analysis of a water sample from Viva found it to have a total hardness of 192.49 ppm CaCO3, which is 25.8% lower than the value claimed.
CONCENTRATION OF SOLUTIONS
Here are the key steps to solve this problem:
1) Convert grams of NH3 to moles using molar mass (65.3 g / 17 g/mol = 3.83 mol NH3)
2) Use balanced equation to determine moles of other substances (3.83 mol NH3 x 4/1 = 15.32 mol NO)
3) Use heat of reaction and moles of limiting reactant to determine heat (ΔH = -904 kJ/mol NH3 x 3.83 mol NH3 = -3,459 kJ)
Physical Properties of solution
A solution is a homogeneous mixture composed of a solute dissolved in a solvent. The solute is the minority component that is dissolved, while the solvent makes up the majority of the solution. Solutions can be classified based on the physical states involved, such as liquid solutions which are the most common. The concentration of a solution describes how much solute is present and can be expressed in terms such as molarity. Properties like vapor pressure, boiling point, and freezing point are influenced by the presence of solute particles in colligative properties.
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#23 Key
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Here are the key steps to solve this problem:
1) Convert grams of NH3 to moles using molar mass (65.3 g / 17 g/mol = 3.83 mol NH3)
2) Use balanced equation to determine moles of other substances (3.83 mol NH3 x 4/1 = 15.32 mol NO)
3) Use heat of reaction and moles of limiting reactant to determine heat (ΔH = -904 kJ/mol NH3 x 3.83 mol NH3 = -3,459 kJ)
Physical Properties of solution
A solution is a homogeneous mixture composed of a solute dissolved in a solvent. The solute is the minority component that is dissolved, while the solvent makes up the majority of the solution. Solutions can be classified based on the physical states involved, such as liquid solutions which are the most common. The concentration of a solution describes how much solute is present and can be expressed in terms such as molarity. Properties like vapor pressure, boiling point, and freezing point are influenced by the presence of solute particles in colligative properties.
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This document discusses colligative properties of solutions, which are properties that depend only on the number of solute particles in solution. It defines four main colligative properties - vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure. The document provides formulas for calculating these properties and includes examples of their application. It also discusses how colligative properties are affected in electrolyte vs. nonelectrolyte solutions and introduces the concept of van't Hoff factor. Finally, it briefly touches on colloids and their differences from true solutions.
MOLARITY
Molarity is a measurement that expresses the concentration of a solute in a solution as moles of solute per liter of solution. It is calculated by taking the moles of solute and dividing by the total liters of solution. Several examples are provided to demonstrate how to calculate molarity from mass, moles, or volume information and how to determine moles or mass of a solute given the molarity and volume of a solution.
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This document provides sample problems and questions for a general chemistry exam. It includes sample balanced equations for neutralization reactions and definitions of key terms like oxidation, reduction, concentration, and indicators. It also asks students to determine oxidation states, identify redox reactions, calculate molarity and amounts of substances in solutions, and determine concentrations of ions after mixing solutions.
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Colligative properties depend on the concentration of solute particles but not their identity. The four main colligative properties are vapor pressure lowering, freezing point depression, boiling point elevation, and osmotic pressure. Freezing point depression and boiling point elevation are directly proportional to the molal concentration of the solution. Electrolytes enhance colligative properties because they dissociate into multiple ions in solution, effectively increasing the number of solute particles compared to nonelectrolytes of the same molar concentration.
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1. Calculate the enthalpy change for the reaction P4O6 (s) + 2 O2 (g) → P4O10 (s) using given enthalpy values for related reactions.
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This document contains 7 problems related to general chemistry. It provides chemical equations to balance, asks students to calculate formula weights and percent compositions of substances, defines key concepts like moles and molar mass, and has multi-step calculations involving moles, molar mass, and grams. The problems cover topics like stoichiometry, formula weights, percent composition, gas laws, and molar conversions.
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Chapter 3 notes
The document defines atomic mass, molar mass, molecular mass, and formula mass. It explains that atomic mass is the mass of an atom measured in atomic mass units (amu) and is based on carbon-12. Molar mass is the mass of one mole of a substance in grams. One mole contains 6.022x1023 elementary units. Molecular mass is the sum of atomic masses in a molecule. Formula mass is the sum of atomic masses in a formula unit of an ionic compound. The document provides examples of calculating molar mass, molecular mass, and formula mass from atomic masses on the periodic table.
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The document describes an experiment to determine how different concentrations of hydrochloric acid affect the rate of reaction with copper (II) powder. A colorimeter will be used to measure the absorbance of light by solutions containing copper (II) and hydrochloric acid over three minutes. Five concentrations of hydrochloric acid will react with 20g of copper (II) powder in separate trials. Variables like temperature, volume, and light intensity will be controlled. Absorbance readings will be taken and used to calculate the order of reaction and compare how concentration impacts the rate. The experiment will be repeated three times for each concentration to collect sufficient data.
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This document discusses concentration of solutions and different ways to measure concentration. It defines dilute and concentrated solutions, and introduces molarity and molality as units of concentration. Molarity is defined as moles of solute per liter of solution. The document provides examples of how to calculate the molarity of a solution given the mass of solute and volume of solution. It also gives practice problems calculating molarity and molality.
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Chapter 12 6-8 Colligative Properties presntation.pptx
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Chapter 4 Problems1. Which of these compounds is a strong elec.docx
Chapter 4 Problems
1.
Which of these compounds is a strong electrolyte?
A.
H2O
B.
O2
C.
H2SO4
D.
C6H12O6 (glucose)
E.
CH3COOH (acetic acid)
2. Which of these compounds is a nonelectrolyte?
A.
NaF
B.
HNO3
C.
CH3COOH (acetic acid)
D.
NaOH
E.
C6H12O6 (glucose)
3. Based on the solubility rules, which one of these compounds should be insoluble in water?
A.
NaCl
B.
MgBr2
C.
FeCl2
D.
AgBr
E.
ZnCl2
4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?
A.
KNO3 will precipitate; Pb2+ and I- are spectator ions.
B.
No precipitate will form.
C.
Pb(NO3)2 will precipitate; K+ and I- are spectator ions.
D.
PbI2 will precipitate; K+ and NO3- are spectator ions.
E.
Pb2+ and I- are spectator ions, and PbI2 will precipitate.
5. Give the oxidation # for the following atoms:
a. N in NaNO3 _________
b. Mn in KMnO4 _________
c. Cl in ClO3- _________
6. Which of these equations does not represent an oxidation-reduction reaction?
A.
3Al + 6HCl ( 3H2 + AlCl3
B.
2H2O ( 2H2 + O2
C.
2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3
D.
2NaI + Br2 ( 2NaBr + I2
E.
Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu
7. What element is oxidized in the chemical reaction
NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?
A.
Ni
B.
Cd
C.
O
D.
H
E.
This is not a redox reaction.
8. Which of these chemical equations describes a precipitation reaction?
A.
2H2(g) + O2(g) ( 2H2O(l)
B.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
C.
2KNO3(s) ( 2KNO2(s) + O2(g)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
9.
The common constituent in all acid solutions is
A.
H2.
B.
H+.
C.
OH-.
D.
H2SO4.
E.
Cl-.
10. Which of these chemical equations describes an acid-base neutralization reaction?
A.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
B.
SO2(g) + H2O(l) ( H2SO3(g)
C.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
11. Which of these chemical equations describes a combustion reaction?
A.
2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)
B.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
C.
N2(g) + 3H2(g) ( 2NH3(g)
D.
2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
12.
What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?
13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?
14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?
15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?
16. 34.62 mL of ...
Chapter 4 Problems1. Which of these compounds is a strong elec.docx
Chapter 4 Problems
1.
Which of these compounds is a strong electrolyte?
A.
H2O
B.
O2
C.
H2SO4
D.
C6H12O6 (glucose)
E.
CH3COOH (acetic acid)
2. Which of these compounds is a nonelectrolyte?
A.
NaF
B.
HNO3
C.
CH3COOH (acetic acid)
D.
NaOH
E.
C6H12O6 (glucose)
3. Based on the solubility rules, which one of these compounds should be insoluble in water?
A.
NaCl
B.
MgBr2
C.
FeCl2
D.
AgBr
E.
ZnCl2
4. Based on the solubility rules, which of these processes will occur when a solution containing about 0.1 g of Pb(NO3)2(aq) is mixed with a solution containing 0.1 g of KI(aq)/100 mL?
A.
KNO3 will precipitate; Pb2+ and I- are spectator ions.
B.
No precipitate will form.
C.
Pb(NO3)2 will precipitate; K+ and I- are spectator ions.
D.
PbI2 will precipitate; K+ and NO3- are spectator ions.
E.
Pb2+ and I- are spectator ions, and PbI2 will precipitate.
5. Give the oxidation # for the following atoms:
a. N in NaNO3 _________
b. Mn in KMnO4 _________
c. Cl in ClO3- _________
6. Which of these equations does not represent an oxidation-reduction reaction?
A.
3Al + 6HCl ( 3H2 + AlCl3
B.
2H2O ( 2H2 + O2
C.
2NaCl + Pb(NO3)2 ( PbCl2 + 3NaNO3
D.
2NaI + Br2 ( 2NaBr + I2
E.
Cu(NO3)2 + Zn ( Zn(NO3)2 + Cu
7. What element is oxidized in the chemical reaction
NiO2 + Cd + 2H2O ( Ni(OH)2 + Cd(OH)2?
A.
Ni
B.
Cd
C.
O
D.
H
E.
This is not a redox reaction.
8. Which of these chemical equations describes a precipitation reaction?
A.
2H2(g) + O2(g) ( 2H2O(l)
B.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
C.
2KNO3(s) ( 2KNO2(s) + O2(g)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
9.
The common constituent in all acid solutions is
A.
H2.
B.
H+.
C.
OH-.
D.
H2SO4.
E.
Cl-.
10. Which of these chemical equations describes an acid-base neutralization reaction?
A.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
B.
SO2(g) + H2O(l) ( H2SO3(g)
C.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
D.
2KBr(aq) + Cl2(g) ( 2KCl(aq) + Br2(l)
E.
CaBr2(aq) + H2SO4(aq) ( CaSO4(s) + 2HBr(g)
11. Which of these chemical equations describes a combustion reaction?
A.
2C2H6(g) + 7O2(g) ( 4CO2(g) + 6H2O(l)
B.
LiOH(aq) + HNO3(aq) ( LiNO3(aq) + H2O(l)
C.
N2(g) + 3H2(g) ( 2NH3(g)
D.
2Na(s) + 2H2O(l) ( 2NaOH(aq) + H2(g)
E.
2Al(s) + 3H2SO4(aq) ( Al2(SO4)3(aq) + 3H2(g)
12.
What is the molarity of a solution that contains 5.0 moles of solute in 2.00 liters of solution?
13. What mass of K2CO3 is needed to prepare 200. mL of a solution having a concentration of 0.150 M?
14. A 50.0 mL sample of 0.436 M NH4NO3 is diluted with water to a total volume of 250.0 mL. What is the ammonium nitrate concentration in the resulting solution?
15. During a titration the following data were collected. A 10. mL portion of an unknown monoprotic acid solution was titrated with 1.0 M NaOH; 40. mL of the base were required to neutralize the sample. What is the molarity of the acid solution?
16. 34.62 mL of.
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2014 Class12th chemistry set 1
This document contains solutions to chemistry problems from the 12th CBSE exam. It covers several topics including chemisorption, redox reactions involving displacement, acid-base properties, isomers, carbohydrate reactions, organic naming conventions, kinetics, electrolytic refining, phosphorus chemistry, crystal lattices, conductivity, reaction orders, colloids and emulsions, coordination compounds, organic reactions, proteins, amino acids, and more. The problems involve calculations, identifying principles, explaining observations, and balancing and describing chemical equations.
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This document summarizes key concepts about aqueous solutions and types of reactions from Chapter 4. It defines terms like solvent, solute, solubility, electrolytes, and molarity. It describes how water is a polar solvent that can dissolve ionic compounds by hydrating ions. It explains types of solutions like strong/weak electrolytes and acids/bases. Precipitation, acid-base, and other reactions in solutions are discussed along with molecular, complete ionic, and net ionic equations. Solubility rules and stoichiometry of precipitation reactions are also covered.
Structure of Matter seminar problems
1. The document discusses moles, molar mass, molarity, and provides example calculations involving these concepts. Molarity is defined as the number of moles of solute per liter of solution.
2. The document then provides 21 practice problems calculating things like the number of moles or grams of various substances, the molarity of different solutions, and multi-step dilution problems.
3. Students are asked to use the concepts of moles, molar mass, and molarity to solve quantitative chemistry problems involving substances in solutions.
IB Exam Question on Titration, Uncertainty calculation, Ideal Gas and Open En...
The document describes several titration experiments:
1) Titration of ethanoic acid in vinegar with sodium hydroxide to determine its molarity. The vinegar was diluted before titration.
2) Titration of hydrated sodium carbonate with hydrochloric acid to determine its molarity and empirical formula.
3) Iodometric titration of vitamin C with potassium iodate to determine the amount of vitamin C.
4) Titration of iron in an iron tablet with potassium manganate to determine the percentage of iron.
5) Titration of chlorine in bleach with sodium thiosulfate after reaction with potassium iodide to determine its molarity.
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This document discusses various properties of mixtures, including solutions and colloids. It defines key terms like solvent, solute, and aqueous solutions. It describes factors that affect solubility such as temperature, nature of solute and solvent, and pressure. It also covers gas solubility based on Henry's Law. Finally, it discusses quantitative expressions of concentration including molarity and molality, as well as colligative properties of solutions like boiling point elevation.
Similar to #11 Key (20)
Chapter 4 Problems1. Which of these compounds is a strong elec.docx
Chapter 4 Problems1. Which of these compounds is a strong elec.docx
Chapter 4 Problems1. Which of these compounds is a strong elec.docx
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#26 Key
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#25 Key
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#11 Key
- 1. KEY GENERAL CHEMISTRY-II (1412) S.I. # 11 1. Calculate the molarity of the following aqueous solutions. a. 0.540 g Mg(NO3)2 in 250.00 mL of solution b. 22.4 g LiClO4 x 3H2O in 175 mL of solution c. 25.0 mL 3.50 M HNO3 diluted to 0.250 L. a. M = mol soute; 0.540 g Mg(NO3)2 x 1 mol Mg(NO3)2 = 1.46x10-2M Mg(NO3)2 L soln 0.2500L soln. 148.3 g Mg(NO3)2 b. 22.4g LiClO4x3H2O x 1mol LiClO4x3H2O = 1.12 M LiClO4x3H2O 0.175 L soln. 160.4 g LiClO4x3H2O c. Mc x Lc = Md x Ld; 3.50M HNO3 x 0.0250 L = ? M HNO3 x 0.250 L 250 mL of 0.350 M HNO3 2. Commercial aqueous nitric acid has a density of 1.42 g/mL and is 16 M. Calculate the percent HNO3 by mass in the solution. Assume volume = 1L (1.00L)(1000 mL)(1.42 g HNO3) = 1.42x103 g soln. (1 L) (1 mL) 16 M = (16 mol HNO3)(63.02 g HNO3) = 1008 = 1.0x103 g HNO3 (1 L soln) (1 mol HNO3) mass % = 1008 g HNO3 x 100% = 71% HNO3 1.42x103 g soln. 3. What is the osmotic pressure of solution formed by dissolving 44.2 mg of aspirin (C9H8O4) in 0.358 L of water 25°C. π = MRT M = (44.2 mg C9H8O4)(1g)(1 mol) = 6.85x10-4M T = 25°C +273 = 298 K (0.358 L) (1000 mg)(180.2 g C9H8O4) M = mol C9H8O4 / L soln. π = (6.851x10-4mol)(0.08206 Lxatm) x 298K = 0.01657 = 0.0168 atm (L) (Kxmol) 4. List the following aqueous solutions in order of increasing boiling point:
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