C 2 D 3 has a solubility product constant of 9.14×10 −9 . What is the molar solubility of C 2 D 3 ?

Hello. In this problem we are asked what are the liabilities of copper to oxalate in pure water? And in a 2.5 times 10 demise three molar sodium oxalate solution. We'll begin by considering just pure water. So write our equation then that describes the equilibrium between our solid proper to oxalate and its ions. And we'll set up a nice tables. We have initial change in equilibrium so we'll ignore our solid since it won't appear in our equilibrium constant expression. Initially we have no copper ions or oxalate and ions to changes in its plus X plus X. The equilibrium then is the initial and the change so we have X. And X. So our celebrity product constant then is equal to the concentration of our copper ions times the oxalate and this is equal to X times X. So we have X squared. Then it's equal to 4.43 Times 10 -10. So extend is equal to the square root of this. So x. works out then to two 10 times 10 to -5 smaller. So this is then the more solid ability of copper to oxalate in pure water. Next we'll consider then the miller sorry ability of property oxalate in a solution of sodium oxalate, sodium oxalate is a soluble salt. So it will associate completely then to form it's irons in a quick solution We're told that the concentration of the sodium oxalate is 2.5 Times to the -3 levels per leader. Given that in the reaction we have one mole of sodium oxalate produced one mole of oxalate irons. That means that the concentration of sodium oxalate will be equal to the concentration of our oxalate anons. We'll set up the ice table again, beginning with our equation for opportunity in equilibrium with the lions and we have initial change in equilibrium. So again, we'll ignore the solid initially have no copper ions, but now we do have oxalate antigens due to the presence of our sodium oxalate solution. And so this is what we refer to as the common iron effect. So the change then is plus X plus X, equilibrium, then is initial plus a change. This is X. And then 2.5 times 10 to the minus three plus X. Since we're dealing with a fairly insoluble salt, the scalability product constant is the order of 10 to the minus 10. X is going to be small relative to the 2.5 times 10 minus three. So we'll just approximate this. Then it's 2.5 times 10 to the minus three and drop our X. Our scalability product constant. Then we have the concentration of our copper lines times out of our oxalate and turns and this works out to X 10 times 2.5 times 10 to the minus three. This is equal to 4.43 times 10 to the minus russell Kerekes. That works out then to 1.8 Percent of -7 Moller. This is then the scalability of cop to oxalate In a solution of sodium oxalate. We found that the scalability decreased in the presence of a common iron. Thanks for watching. Hope this helped.

Indice

Skip topic navigation

1. Intro to General Chemistry4h 5m

Classification of Matter
18m

Physical & Chemical Changes
19m

Chemical Properties
7m

Physical Properties
6m

Intensive vs. Extensive Properties
15m

Temperature
13m

Scientific Notation
13m

SI Units
8m

Metric Prefixes
26m

Significant Figures
9m

Significant Figures: Precision in Measurements
9m

Significant Figures: In Calculations
17m

Conversion Factors
16m

Dimensional Analysis
24m

Density
12m

Density of Geometric Objects
19m

Density of Non-Geometric Objects
6m

2. Atoms & Elements4h 40m

The Atom
10m

Subatomic Particles
17m

Isotopes
17m

Ions
27m

Atomic Mass
32m

Periodic Table: Classifications
15m

Periodic Table: Group Names
8m

Periodic Table: Representative Elements & Transition Metals
7m

Periodic Table: Element Symbols
6m

Periodic Table: Elemental Forms
6m

Periodic Table: Phases
9m

Periodic Table: Charges
20m

Calculating Molar Mass
10m

Mole Concept
31m

Law of Conservation of Mass
5m

Law of Definite Proportions
12m

Atomic Theory
9m

Law of Multiple Proportions
8m

Millikan Oil Drop Experiment
8m

Rutherford Gold Foil Experiment
14m

3. Chemical Reactions4h 34m

Empirical Formula
18m

Molecular Formula
21m

Combustion Analysis
39m

Combustion Apparatus
16m

Polyatomic Ions
25m

Naming Ionic Compounds
12m

Writing Ionic Compounds
8m

Naming Ionic Hydrates
8m

Naming Acids
23m

Naming Molecular Compounds
8m

Balancing Chemical Equations
14m

Stoichiometry
20m

Limiting Reagent
18m

Percent Yield
21m

Mass Percent
6m

Functional Groups in Chemistry
11m

4. BONUS: Lab Techniques and Procedures1h 30m

Laboratory Materials
21m

Experimental Error
16m

Distillation & Floatation
12m

Chromatography
4m

Filtration and Evaporation
5m

Extraction
14m

Test for Ions and Gases
14m

5. BONUS: Mathematical Operations and Functions52m

Multiplication and Division Operations
7m

Addition and Subtraction Operations
10m

Power and Root Functions
6m

Logarithmic Functions
20m

The Quadratic Formula
7m

6. Chemical Quantities & Aqueous Reactions4h 17m

Solutions
9m

Molarity
22m

Osmolarity
15m

Dilutions
15m

Solubility Rules
16m

Electrolytes
24m

Molecular Equations
21m

Gas Evolution Equations
13m

Solution Stoichiometry
14m

Complete Ionic Equations
18m

Calculate Oxidation Numbers
16m

Redox Reactions
20m

Balancing Redox Reactions: Acidic Solutions
17m

Balancing Redox Reactions: Basic Solutions
17m

Activity Series
11m

7. Gases4h 8m

Pressure Units
9m

The Ideal Gas Law
18m

The Ideal Gas Law Derivations
18m

The Ideal Gas Law Applications
6m

Chemistry Gas Laws
16m

Chemistry Gas Laws: Combined Gas Law
14m

Mole Fraction of Gases
6m

Partial Pressure
19m

The Ideal Gas Law: Molar Mass
13m

The Ideal Gas Law: Density
16m

Gas Stoichiometry
19m

Standard Temperature and Pressure
14m

Effusion
15m

Root Mean Square Speed
9m

Kinetic Energy of Gases
10m

Maxwell-Boltzmann Distribution
8m

Velocity Distributions
4m

Kinetic Molecular Theory
16m

Van der Waals Equation
9m

8. Thermochemistry3h 4m

Nature of Energy
6m

Kinetic & Potential Energy
11m

First Law of Thermodynamics
7m

Internal Energy
10m

Endothermic & Exothermic Reactions
10m

Heat Capacity
23m

Constant-Pressure Calorimetry
26m

Constant-Volume Calorimetry
11m

Thermal Equilibrium
8m

Thermochemical Equations
14m

Formation Equations
11m

Enthalpy of Formation
14m

Hess's Law
26m

9. Quantum Mechanics3h 7m

Wavelength and Frequency
6m

Speed of Light
9m

The Energy of Light
13m

Electromagnetic Spectrum
10m

Photoelectric Effect
20m

De Broglie Wavelength
10m

Heisenberg Uncertainty Principle
18m

Bohr Model
14m

Emission Spectrum
5m

Bohr Equation
13m

Introduction to Quantum Mechanics
5m

Quantum Numbers: Principal Quantum Number
6m

Quantum Numbers: Angular Momentum Quantum Number
10m

Quantum Numbers: Magnetic Quantum Number
11m

Quantum Numbers: Spin Quantum Number
10m

Quantum Numbers: Number of Electrons
11m

Quantum Numbers: Nodes
7m

10. Periodic Properties of the Elements3h 49m

The Electron Configuration
27m

The Electron Configuration: Condensed
4m

The Electron Configurations: Exceptions
17m

The Electron Configuration: Ions
12m

Paramagnetism and Diamagnetism
13m

The Electron Configuration: Quantum Numbers
17m

Valence Electrons of Elements
12m

Periodic Trend: Metallic Character
6m

Periodic Trend: Atomic Radius
12m

Periodic Trend: Ionic Radius
14m

Periodic Trend: Ionization Energy
17m

Periodic Trend: Successive Ionization Energies
15m

Periodic Trend: Electron Affinity
10m

Periodic Trend: Electronegativity
7m

Periodic Trend: Effective Nuclear Charge
26m

Periodic Trend: Cumulative
13m

11. Bonding & Molecular Structure3h 54m

Lewis Dot Symbols
10m

Chemical Bonds
13m

Dipole Moment
15m

Octet Rule
10m

Formal Charge
12m

Lewis Dot Structures: Neutral Compounds
20m

Lewis Dot Structures: Sigma & Pi Bonds
15m

Lewis Dot Structures: Ions
18m

Lewis Dot Structures: Exceptions
14m

Lewis Dot Structures: Acids
17m

Resonance Structures
25m

Average Bond Order
4m

Bond Energy
17m

Coulomb's Law
7m

Lattice Energy
16m

Born Haber Cycle
15m

12. Molecular Shapes & Valence Bond Theory2h 11m

Valence Shell Electron Pair Repulsion Theory
5m

Equatorial and Axial Positions
12m

Electron Geometry
13m

Molecular Geometry
24m

Bond Angles
14m

Hybridization
12m

Molecular Orbital Theory
13m

MO Theory: Homonuclear Diatomic Molecules
11m

MO Theory: Heteronuclear Diatomic Molecules
7m

MO Theory: Bond Order
16m

13. Liquids, Solids & Intermolecular Forces2h 41m

Molecular Polarity
10m

Intermolecular Forces
22m

Intermolecular Forces and Physical Properties
12m

Clausius-Clapeyron Equation
22m

Phase Diagrams
13m

Heating and Cooling Curves
28m

Atomic, Ionic, and Molecular Solids
11m

Crystalline Solids
6m

Simple Cubic Unit Cell
7m

Body Centered Cubic Unit Cell
14m

Face Centered Cubic Unit Cell
10m

14. Solutions3h 17m

Solutions: Solubility and Intermolecular Forces
20m

Molality
18m

Parts per Million (ppm)
13m

Mole Fraction of Solutions
9m

Solutions: Mass Percent
12m

Types of Aqueous Solutions
8m

Intro to Henry's Law
4m

Henry's Law Calculations
12m

The Colligative Properties
17m

Boiling Point Elevation
18m

Freezing Point Depression
10m

Osmosis
21m

Osmotic Pressure
10m

Vapor Pressure Lowering (Raoult's Law)
19m

15. Chemical Kinetics3h 2m

Intro to Chemical Kinetics
4m

Energy Diagrams
9m

Catalyst
9m

Factors Influencing Rates
10m

Average Rate of Reaction
7m

Stoichiometric Rate Calculations
5m

Instantaneous Rate
7m

Collision Theory
7m

Arrhenius Equation
28m

Rate Law
25m

Reaction Mechanism
17m

Integrated Rate Law
25m

Half-Life
24m

16. Chemical Equilibrium2h 31m

Intro to Chemical Equilibrium
7m

Equilibrium Constant K
13m

Equilibrium Constant Calculations
9m

Kp and Kc
22m

Using Hess's Law To Determine K
9m

Calculating K For Overall Reaction
16m

Le Chatelier's Principle
21m

ICE Charts
34m

Reaction Quotient
15m

17. Acid and Base Equilibrium5h 5m

Acids Introduction
9m

Bases Introduction
7m

Binary Acids
15m

Oxyacids
10m

Bases
14m

Amphoteric Species
5m

Arrhenius Acids and Bases
5m

Bronsted-Lowry Acids and Bases
21m

Lewis Acids and Bases
13m

The pH Scale
17m

Auto-Ionization
9m

Ka and Kb
16m

pH of Strong Acids and Bases
9m

Ionic Salts
17m

pH of Weak Acids
31m

pH of Weak Bases
32m

Diprotic Acids and Bases
8m

Diprotic Acids and Bases Calculations
30m

Triprotic Acids and Bases
10m

Triprotic Acids and Bases Calculations
17m

18. Aqueous Equilibrium4h 47m

Intro to Buffers
21m

Henderson-Hasselbalch Equation
19m

Intro to Acid-Base Titration Curves
13m

Strong Titrate-Strong Titrant Curves
9m

Weak Titrate-Strong Titrant Curves
15m

Acid-Base Indicators
8m

Titrations: Weak Acid-Strong Base
38m

Titrations: Weak Base-Strong Acid
41m

Titrations: Strong Acid-Strong Base
11m

Titrations: Diprotic & Polyprotic Buffers
32m

Solubility Product Constant: Ksp
17m

Ksp: Common Ion Effect
18m

Precipitation: Ksp vs Q
12m

Selective Precipitation
9m

Complex Ions: Formation Constant
18m

19. Chemical Thermodynamics1h 51m

Spontaneous vs Nonspontaneous Reactions
7m

Entropy
23m

Entropy Calculations
13m

Entropy Calculations: Phase Changes
6m

Third Law of Thermodynamics
7m

Gibbs Free Energy
14m

Gibbs Free Energy Calculations
22m

Gibbs Free Energy And Equilibrium
14m

20. Electrochemistry2h 42m

Standard Reduction Potentials
9m

Intro to Electrochemical Cells
6m

Galvanic Cell
25m

Electrolytic Cell
10m

Cell Potential: Standard
13m

Cell Potential: The Nernst Equation
20m

Cell Potential and Gibbs Free Energy
16m

Cell Potential and Equilibrium
8m

Cell Potential: G and K
16m

Cell Notation
20m

Electroplating
16m

21. Nuclear Chemistry2h 37m

Intro to Radioactivity
10m

Alpha Decay
9m

Beta Decay
7m

Gamma Emission
7m

Electron Capture & Positron Emission
9m

Neutron to Proton Ratio
7m

Band of Stability: Alpha Decay & Nuclear Fission
10m

Band of Stability: Beta Decay
3m

Band of Stability: Electron Capture & Positron Emission
4m

Band of Stability: Overview
14m

Measuring Radioactivity
7m

Rate of Radioactive Decay
12m

Radioactive Half-Life
16m

Mass Defect
19m

Nuclear Binding Energy
14m

22. Organic Chemistry5h 4m

Introduction to Organic Chemistry
8m

Structural Formula
8m

Condensed Formula
10m

Skeletal Formula
6m

Spatial Orientation of Bonds
3m

Intro to Hydrocarbons
16m

Isomers
11m

Chirality
12m

Functional Groups in Chemistry
11m

Naming Alkanes
4m

The Alkyl Groups
9m

Naming Alkanes with Substituents
13m

Naming Cyclic Alkanes
6m

Naming Other Substituents
8m

Naming Alcohols
11m

Naming Alkenes
11m

Naming Alkynes
9m

Naming Ketones
5m

Naming Aldehydes
5m

Naming Carboxylic Acids
4m

Naming Esters
8m

Naming Ethers
5m

Naming Amines
5m

Naming Benzene
7m

Alkane Reactions
7m

Intro to Addition Reactions
4m

Halogenation Reactions
4m

Hydrogenation Reactions
3m

Hydrohalogenation Reactions
7m

Alcohol Reactions: Substitution Reactions
4m

Alcohol Reactions: Dehydration Reactions
9m

Intro to Redox Reactions
8m

Alcohol Reactions: Oxidation Reactions
7m

Aldehydes and Ketones Reactions
6m

Ester Reactions: Esterification
4m

Ester Reactions: Saponification
3m

Carboxylic Acid Reactions
4m

Amine Reactions
3m

Amide Formation
4m

Benzene Reactions
10m

23. Chemistry of the Nonmetals2h 39m

Main Group Elements: Bonding Types
4m

Main Group Elements: Boiling & Melting Points
7m

Main Group Elements: Density
11m

Main Group Elements: Periodic Trends
7m

The Electron Configuration Review
16m

Periodic Table Charges Review
20m

Hydrogen Isotopes
4m

Hydrogen Compounds
11m

Production of Hydrogen
8m

Group 1A and 2A Reactions
7m

Boron Family Reactions
7m

Boron Family: Borane
7m

Borane Reactions
7m

Nitrogen Family Reactions
12m

Oxides, Peroxides, and Superoxides
12m

Oxide Reactions
4m

Peroxide and Superoxide Reactions
6m

Noble Gas Compounds
3m

24. Transition Metals and Coordination Compounds3h 19m

Atomic Radius & Density of Transition Metals
11m

Electron Configurations of Transition Metals
7m

Electron Configurations of Transition Metals: Exceptions
11m

Paramagnetism and Diamagnetism
10m

Ligands
10m

Complex Ions
5m

Coordination Complexes
7m

Classification of Ligands
11m

Coordination Numbers & Geometry
9m

Naming Coordination Compounds
22m

Writing Formulas of Coordination Compounds
8m

Isomerism in Coordination Complexes
17m

Orientations of D Orbitals
4m

Intro to Crystal Field Theory
10m

Crystal Field Theory: Octahedral Complexes
5m

Crystal Field Theory: Tetrahedral Complexes
4m

Crystal Field Theory: Square Planar Complexes
4m

Crystal Field Theory Summary
8m

Magnetic Properties of Complex Ions
9m

Strong-Field vs Weak-Field Ligands
6m

Magnetic Properties of Complex Ions: Octahedral Complexes
11m

18. Aqueous Equilibrium

Ksp: Common Ion Effect

General Chemistry

18. Aqueous Equilibrium

Ksp: Common Ion Effect

Problema precedenteProssimo problema

Difficoltà con General Chemistry?

Unisciti a migliaia di studenti che si affidano a noi per superare al meglio i loro esami!

4:17 minuti

Domanda aperta

C₂D₃ has a solubility product constant of 9.14×10⁻⁹ . What is the molar solubility of C₂D₃?

Risposta video verificata per un problema simile:

Questa soluzione video è stata consigliata dai nostri tutor come utile per risolvere questo problema.

Durata del video:

Guarda un video:

0 Commenti

Problema precedenteProssimo problema

3:39m

Guarda il prossimo

Padroneggia Common Ion Effect Example con una breve spiegazione video di Jules Bruno

Video correlati

Pratica correlata

Domanda del libro di testo

Use Le Châtelier's principle to predict whether the solubility of BaF2 will increase, decrease, or remain the same on addition of each of the following substances. (a) HCl

902

views

Domanda del libro di testo

Calculate the molar solubility of PbCrO4 in: (a) Pure Water (d) 1.0 x 10^-3 M K2CrO4

1134

views

rank

Domanda del libro di testo

Is the solubility of Zn(OH)₂ increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (a) HCl

702

views

Domanda del libro di testo

Is the solubility of Fe(OH)3 increased, decreased, or unchanged on addition of each of the following substances? Write a balanced net ionic equation for each dissolution reaction. (See Appendix C.6 for formulas of complex ions.) (b) NaOH(aq)

901

views

Domanda aperta

Which of the following does not increase the rate of dissolving a solid in water?

851

views

Domanda aperta

A beaker full of acid is added to a beaker full of base the ph of the base will