Chemistry 2012 Student Edition (hard Cover) Grade 11
12th Edition
ISBN: 9780132525763
Author: Prentice Hall
Publisher: Prentice Hall
expand_more
expand_more
format_list_bulleted
Question
Chapter 16.1, Problem 5LC
Interpretation Introduction
Interpretation: The conditions that determine the solubility of solid, liquid, and gaseous solutes in a solvent need to be explained.
Concept introduction: A solution is a mixture of two or more components and the composition of the mixture is homogeneous. Solute in solvent makes the solution. Different conditions affect the rate of solubility of the solute in the solvent.
Expert Solution & Answer
Answer to Problem 5LC
The condition that determines the solubility of solid, liquid, and gaseous solutes are pressure and temperature.
Explanation of Solution
The solubility of solid, liquid, and gaseous solutes is affected by conditions and those following:
- Pressure: In the case of solid and liquid, the pressure does not affect the solubility that much but in the case of gas, the pressure affects the solubility to a great extent. The solubility of a gas increases when the partial pressure of a gas above the liquid increases. This solubility of gas can be explained by Henry law such as:
- S1 is the solubility of gas at pressure P1 .
- S2 is the solubility of gas at pressure P2 .
- P1 is the initial pressure.
- P2 is the final pressure.
- Temperature: In most of the solid substances, the temperature of the solvent increases then, solubility increases. This is because as the temperature increases, high energy can be provided to break the bonds in solids easily. In the case of gases, the temperature increases then the solubility of gas decreases. This is because high energy is provided to overcome the attraction between the gas molecules and the solvent.
Henry's law states that the solubility of a gas is proportional to its partial pressure. As, the partial pressure of the gas increases, its solubility also increases. This statement can be represented from the equation as:
Where:
From the above equation, it is clear that solubility and pressure are directly proportional to each other. When pressure increases, the solubility of the gas increases and vice versa.
Conclusion
The conditions that determine the solubility of
Chapter 16 Solutions
Chemistry 2012 Student Edition (hard Cover) Grade 11
Ch. 16.1 - Prob. 1SPCh. 16.1 - Prob. 2SPCh. 16.1 - Prob. 3LCCh. 16.1 - Prob. 4LCCh. 16.1 - Prob. 5LCCh. 16.1 - Prob. 6LCCh. 16.1 - Prob. 7LCCh. 16.1 - Prob. 8LCCh. 16.1 - Prob. 9LCCh. 16.2 - Prob. 10SP
Ch. 16.2 - Prob. 11SPCh. 16.2 - Prob. 12SPCh. 16.2 - Prob. 13SPCh. 16.2 - Prob. 14SPCh. 16.2 - Prob. 15SPCh. 16.2 - Prob. 16SPCh. 16.2 - Prob. 17SPCh. 16.2 - Prob. 18SPCh. 16.2 - Prob. 19LCCh. 16.2 - Prob. 20LCCh. 16.2 - Prob. 21LCCh. 16.2 - Prob. 22LCCh. 16.2 - Prob. 23LCCh. 16.2 - Prob. 24LCCh. 16.2 - Prob. 25LCCh. 16.2 - Prob. 26LCCh. 16.2 - Prob. 27LCCh. 16.3 - Prob. 28LCCh. 16.3 - Prob. 29LCCh. 16.3 - Prob. 30LCCh. 16.3 - Prob. 31LCCh. 16.3 - Prob. 32LCCh. 16.3 - Prob. 33LCCh. 16.4 - Prob. 34SPCh. 16.4 - Prob. 35SPCh. 16.4 - Prob. 36SPCh. 16.4 - Prob. 37SPCh. 16.4 - Prob. 38SPCh. 16.4 - Prob. 39SPCh. 16.4 - Prob. 40SPCh. 16.4 - Prob. 41SPCh. 16.4 - Prob. 42LCCh. 16.4 - Prob. 43LCCh. 16.4 - Prob. 44LCCh. 16.4 - Prob. 45LCCh. 16.4 - Prob. 46LCCh. 16.4 - Prob. 47LCCh. 16 - Prob. 48ACh. 16 - Prob. 49ACh. 16 - Prob. 50ACh. 16 - Prob. 51ACh. 16 - Prob. 52ACh. 16 - Prob. 53ACh. 16 - Prob. 54ACh. 16 - Prob. 55ACh. 16 - Prob. 56ACh. 16 - Prob. 57ACh. 16 - Prob. 58ACh. 16 - Prob. 59ACh. 16 - Prob. 60ACh. 16 - Prob. 61ACh. 16 - Prob. 62ACh. 16 - Prob. 63ACh. 16 - Prob. 64ACh. 16 - Prob. 65ACh. 16 - Prob. 66ACh. 16 - Prob. 67ACh. 16 - Prob. 68ACh. 16 - Prob. 69ACh. 16 - Prob. 70ACh. 16 - Prob. 71ACh. 16 - Prob. 72ACh. 16 - Prob. 73ACh. 16 - Prob. 74ACh. 16 - Prob. 75ACh. 16 - Prob. 76ACh. 16 - Prob. 77ACh. 16 - Prob. 78ACh. 16 - Prob. 79ACh. 16 - Prob. 80ACh. 16 - Prob. 81ACh. 16 - Prob. 82ACh. 16 - Prob. 83ACh. 16 - Prob. 84ACh. 16 - Prob. 85ACh. 16 - Prob. 86ACh. 16 - Prob. 87ACh. 16 - Prob. 88ACh. 16 - Prob. 89ACh. 16 - Prob. 90ACh. 16 - Prob. 91ACh. 16 - Prob. 92ACh. 16 - Prob. 93ACh. 16 - Prob. 94ACh. 16 - Prob. 95ACh. 16 - Prob. 96ACh. 16 - Prob. 97ACh. 16 - Prob. 98ACh. 16 - Prob. 99ACh. 16 - Prob. 100ACh. 16 - Prob. 101ACh. 16 - Prob. 103ACh. 16 - Prob. 104ACh. 16 - Prob. 105ACh. 16 - Prob. 106ACh. 16 - Prob. 107ACh. 16 - Prob. 108ACh. 16 - Prob. 109ACh. 16 - Prob. 110ACh. 16 - Prob. 111ACh. 16 - Prob. 112ACh. 16 - Prob. 113ACh. 16 - Prob. 114ACh. 16 - Prob. 115ACh. 16 - Prob. 116ACh. 16 - Prob. 117ACh. 16 - Prob. 118ACh. 16 - Prob. 119ACh. 16 - Prob. 120ACh. 16 - Prob. 121ACh. 16 - Prob. 122ACh. 16 - Prob. 123ACh. 16 - Prob. 124ACh. 16 - Prob. 1STPCh. 16 - Prob. 2STPCh. 16 - Prob. 3STPCh. 16 - Prob. 4STPCh. 16 - Prob. 5STPCh. 16 - Prob. 6STPCh. 16 - Prob. 7STPCh. 16 - Prob. 8STPCh. 16 - Prob. 9STPCh. 16 - Prob. 10STPCh. 16 - Prob. 11STPCh. 16 - Prob. 12STPCh. 16 - Prob. 13STPCh. 16 - Prob. 14STP
Knowledge Booster
Similar questions
- When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 12.80 mL of 3.00 M HCl, both initially at room temperature (22.00 C), the temperature increased to 29.30 C. The resultant salt solution had a mass of 27.80 g and a specific heat capacity of 3.74 J/Kg. What is heat capacity of the calorimeter (in J/C)? Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ/mol.arrow_forwardWhen 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 12.80 mL of 3.00 M HCl, both initially at room temperature (22.00 C), the temperature increased to 29.30 C. The resultant salt solution had a mass of 27.80 g and a specific heat capacity of 3.74 J/Kg. What is heat capacity of the calorimeter (in J/C)? Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ/mol. Which experimental number must be initialled by the Lab TA for the first run of Part 1 of the experiment? a) the heat capacity of the calorimeter b) Mass of sample c) Ti d) The molarity of the HCl e) Tfarrow_forwardPredict products for the Following organic rxn/s by writing the structurels of the correct products. Write above the line provided" your answer D2 ①CH3(CH2) 5 CH3 + D₂ (adequate)" + 2 mited) 19 Spark Spark por every item. 4 CH 3 11 3 CH 3 (CH2) 4 C-H + CH3OH CH2 CH3 + CH3 CH2OH 0 CH3 fou + KMnDy→ C43 + 2 KMn Dy→→ C-OH ") 0 C-OH 1110 (4.) 9+3 =C CH3 + HNO 3 0 + Heat> + CH3 C-OH + Heat CH2CH3 - 3 2 + D Heat H 3 CH 3 CH₂ CH₂ C = CH + 2 H₂ → 2 2arrow_forward
- When 15.00 mL of 3.00 M NaOH was mixed in a calorimeter with 12.80 mL of 3.00 M HCl, both initially at room temperature (22.00 C), the temperature increased to 29.30 C. The resultant salt solution had a mass of 27.80 g and a specific heat capacity of 3.74 J/Kg. What is heat capacity of the calorimeter (in J/C)? Note: The molar enthalpy of neutralization per mole of HCl is -55.84 kJ/mol.arrow_forwardQ6: Using acetic acid as the acid, write the balanced chemical equation for the protonation of the two bases shown (on the -NH2). Include curved arrows to show the mechanism. O₂N- O₂N. -NH2 -NH2 a) Which of the two Bronsted bases above is the stronger base? Why? b) Identify the conjugate acids and conjugate bases for the reactants. c) Identify the Lewis acids and bases in the reactions.arrow_forwardQ5: For the two reactions below: a) Use curved electron-pushing arrows to show the mechanism for the reaction in the forward direction. Redraw the compounds to explicitly illustrate all bonds that are broken and all bonds that are formed. b) Label Bronsted acids and bases in the left side of the reactions. c) For reaction A, which anionic species is the weakest base? Which neutral compound is the stronger acid? Is the forward or reverse reaction favored? d) Label Lewis acids and bases, nucleophiles and electrophiles in the left side of the reactions. A. 용 CH3OH я хон CH3O OH B. HBr CH3ONa NaBr CH3OHarrow_forward
- potential energy Br b) Translate the Newman projection below to its wedge-and-dash drawing. F H. OH CH3 CI c) Isopentane (2-methylbutane) is a compound containing a branched carbon chain. Draw a Newman projection of six conformations about the C2-C3 bond of isopentane. On the curve of potential energy versus angle of internal rotation for isopentane, label each energy maximum and minimum with one of the conformations. 0° 。 F A B D C angle of internal rotation E F 360° (=0°) JDownlarrow_forwardQ7: Identify the functional groups in these molecules a) CH 3 b) Aspirin: HO 'N' Capsaicin HO O CH3 CH 3arrow_forwardQ2: Name the following alkanesarrow_forward
- 1. Complete the following table in your laboratory notebook. Substance Formula Methanol CH3OH Ethanol C2H5OH 1-Propanol C3H7OH 1-Butanol C4H9OH Pentane C5H12 Hexane C6H14 Water H₂O Acetone C3H60 Structural Formula Molecular Weight (g/mol) Hydrogen Bond (Yes or No)arrow_forwardQ1: Compare the relative acidity in each pair of compounds. Briefly explain. (a) CH3OH vs NH 3 (b) HF vs CH3COOH (c) NH3 vs CH4 (d) HCI vs HI (e) CH3COOH vs CH3SH (f) H₂C=CH2 vs CH3 CH3 (g) compare the acidity of the two bolded hydrogens O. H N- (h) compare the acidity of the two bolded hydrogens, draw resonance structures to explain H H Harrow_forwardQ3: Rank the following molecules in order of decreasing boiling point: (a) 3-methylheptane; (b) octane; (c) 2,4-dimethylhexane; (d) 2,2,4-trimethylpentane.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
ChemistryChemistryISBN:9781259911156Author:Raymond Chang Dr., Jason Overby ProfessorPublisher:McGraw-Hill Education
Principles of Instrumental AnalysisChemistryISBN:9781305577213Author:Douglas A. Skoog, F. James Holler, Stanley R. CrouchPublisher:Cengage Learning
Organic ChemistryChemistryISBN:9780078021558Author:Janice Gorzynski Smith Dr.Publisher:McGraw-Hill Education
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...ChemistryISBN:9781118431221Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. BullardPublisher:WILEY
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781259911156
Author:Raymond Chang Dr., Jason Overby Professor
Publisher:McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:9781305577213
Author:Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:Cengage Learning
Organic Chemistry
Chemistry
ISBN:9780078021558
Author:Janice Gorzynski Smith Dr.
Publisher:McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
Elementary Principles of Chemical Processes, Bind...
Chemistry
ISBN:9781118431221
Author:Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:WILEY