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Questions and Answers
What is the term for a substance that is capable of being dissolved?
What is the term for a substance that is capable of being dissolved?
- Suspension
- Solute
- Soluble (correct)
- Solvent
What is a homogeneous mixture of two or more substances in a single phase called?
What is a homogeneous mixture of two or more substances in a single phase called?
solution
The dissolving medium in a solution is called the ___
The dissolving medium in a solution is called the ___
solvent
The substance dissolved in a solution is called the ___
The substance dissolved in a solution is called the ___
If particles in a solvent are so large that they settle out unless the mixture is constantly stirred or agitated, the mixture is called a ___
If particles in a solvent are so large that they settle out unless the mixture is constantly stirred or agitated, the mixture is called a ___
Particles that are intermediate in size between those in solutions and suspensions form mixtures known as ___
Particles that are intermediate in size between those in solutions and suspensions form mixtures known as ___
What happens when an ionic compound dissolves?
What happens when an ionic compound dissolves?
Solutions that can conduct electric current are known as ____
Solutions that can conduct electric current are known as ____
What are three ways to increase the rate of dissolution?
What are three ways to increase the rate of dissolution?
What governs solubility?
What governs solubility?
What are the types of intermolecular forces?
What are the types of intermolecular forces?
Non-polar molecules dissolve in ___ solvents
Non-polar molecules dissolve in ___ solvents
Polar molecules dissolve ___ and ___
Polar molecules dissolve ___ and ___
Two liquids that dissolve in each other are called ___
Two liquids that dissolve in each other are called ___
Two liquids that do not dissolve into each other are called ___
Two liquids that do not dissolve into each other are called ___
The solubility of a gas in a liquid is ____ proportional to the partial pressure of that gas on the surface of the liquid.
The solubility of a gas in a liquid is ____ proportional to the partial pressure of that gas on the surface of the liquid.
What is the rapid escape of a gas from a liquid in which it is dissolved called?
What is the rapid escape of a gas from a liquid in which it is dissolved called?
The solubility of gases in water usually ___ with ___ temperature.
The solubility of gases in water usually ___ with ___ temperature.
A ___ is heat that can either be released or absorbed when a compound is dissolved.
A ___ is heat that can either be released or absorbed when a compound is dissolved.
What is the net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent called?
What is the net amount of energy absorbed as heat by the solution when a specific amount of solute dissolves in a solvent called?
What is amount of solute dissolved per a given amount of solvent known as?
What is amount of solute dissolved per a given amount of solvent known as?
In the chemistry world, the most common unit of concentration is _()
In the chemistry world, the most common unit of concentration is _()
What is the concentration of a solution expressed in moles of solute per kilogram of solvent?
What is the concentration of a solution expressed in moles of solute per kilogram of solvent?
What are characteristics of ionic compounds?
What are characteristics of ionic compounds?
What are characteristics of covalent compounds?
What are characteristics of covalent compounds?
What are electrostatic interactions?
What are electrostatic interactions?
What are the three types of compounds?
What are the three types of compounds?
Anions are __ or __
Anions are __ or __
__ can change state
__ can change state
Molecules means ___
Molecules means ___
Two solutes, ionic salt, polar molecule, are called ___
Two solutes, ionic salt, polar molecule, are called ___
One solute, nonpolar molecule is called ___
One solute, nonpolar molecule is called ___
What are some examples of polar covalent molecules?
What are some examples of polar covalent molecules?
What are some examples of non-polar covalent molecules?
What are some examples of non-polar covalent molecules?
In enthalpy of solution, a solution gets colder, energy is a reactant required/absorbed, 'take', is classified as ___
In enthalpy of solution, a solution gets colder, energy is a reactant required/absorbed, 'take', is classified as ___
In enthalpy of solution, a solution gets warmer, energy is a product or released, 'make', is classified as ___
In enthalpy of solution, a solution gets warmer, energy is a product or released, 'make', is classified as ___
What are the three steps to dissolve?
What are the three steps to dissolve?
What are strong electrolytes?
What are strong electrolytes?
What is considered a weak electrolyte?
What is considered a weak electrolyte?
What produces ions when dissolved?
What produces ions when dissolved?
What allows solutions to conduct electric current?
What allows solutions to conduct electric current?
When dissolving gases in water, you should __ pressure and __ in temperature.
When dissolving gases in water, you should __ pressure and __ in temperature.
What are the three steps to make a molarity solution?
What are the three steps to make a molarity solution?
What is the density of water?
What is the density of water?
You don't need a volumetric flask in ___
You don't need a volumetric flask in ___
What are the three steps to make a molality solution?
What are the three steps to make a molality solution?
Flashcards
Soluble
Soluble
Capable of being dissolved.
Solution
Solution
A homogeneous mixture of two or more substances in a single phase.
Solvent
Solvent
The dissolving medium in a solution.
Solute
Solute
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Suspension
Suspension
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Colloid
Colloid
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Electrolyte
Electrolyte
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Dissolution rate
Dissolution rate
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Intermolecular forces
Intermolecular forces
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Intramolecular forces
Intramolecular forces
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Miscible
Miscible
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Immiscible
Immiscible
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Gas solubility
Gas solubility
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Effervescence
Effervescence
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Enthalpy
Enthalpy
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Enthalpy of solution
Enthalpy of solution
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Concentration
Concentration
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Molarity(M)
Molarity(M)
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Molality
Molality
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Ionic compounds
Ionic compounds
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Covalent compounds
Covalent compounds
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Anions
Anions
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Polyatomic Ions
Polyatomic Ions
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Solution Preparation
Solution Preparation
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Strong Electrolytes
Strong Electrolytes
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Study Notes
Solutions and Mixtures
- Soluble: Capable of being dissolved.
- Solution: A homogeneous mixture of two or more substances in a single phase.
- Solvent: The dissolving medium in a solution.
- Solute: The substance dissolved in a solution.
- Suspension: Mixture with large particles that settle unless stirred.
- Colloids: Intermediate-sized particles between solutions and suspensions.
Properties of Solutions
- Electrolytes: Solutions that can conduct electric current.
- Increasing dissolution rate: Achieved by increasing surface area, agitating the solution, or heating it.
Molecular Interactions
- Intermolecular forces: Attractions between molecules that influence solubility.
- Intramolecular forces: Attractions within a molecule, such as covalent bonds.
- Types of intermolecular forces: Ion-dipole, dipole-dipole, hydrogen bonding, and London dispersion forces.
Solubility Concepts
- Polar molecules dissolve in polar solvents and ionic compounds.
- Non-polar molecules dissolve in non-polar solvents.
- Miscible: Two liquids that dissolve in each other.
- Immiscible: Two liquids that do not dissolve into each other.
- Gas solubility in liquids is directly proportional to the gas's partial pressure.
Thermodynamics of Solutions
- Effervescence: Rapid escape of gas from a liquid.
- Gas solubility decreases with increasing temperature.
- Enthalpy: Heat absorbed or released during dissolution.
- Enthalpy of solution: Net energy absorbed by the solution when a solute dissolves.
Concentration Metrics
- Concentration: Amount of solute per given solvent.
- Molarity (M): Common concentration unit expressed as moles of solute per liter of solution.
- Molality: Concentration expressed in moles of solute per kilogram of solvent.
Compound Characteristics
- Ionic compounds: Typically involve electron transfer, have high electronegativity (>1.7), and form crystals.
- Covalent compounds: Involve electron sharing, have lower electronegativity (<1.7), and primarily consist of nonmetals.
Types of Compounds
- Types include ionic salts, polar covalent molecules, and non-polar covalent molecules.
- Anions can be single elements or polyatomic ions.
- Molecules can change state and are defined by covalent bonding.
Solution Preparation
- Process of dissolving involves breaking solute and solvent interactions, followed by forming solute-solvent interactions.
- Strong electrolytes include ionic salts; weak electrolytes generally refer to acids.
- Steps to prepare molarity solutions: Mass out moles, place in a volumetric flask, and add solvent to the mark.
- Density of water is 1 kg/L; molality preparation does not require volumetric flasks.
Overall Summary
- Important principles of solubility, thermodynamics, and preparation of solutions; distinctions between electrolytes, types of molecular interactions, and methods to calculate concentration are foundational in chemistry.
Studying That Suits You
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Description
Test your understanding of key terms from Chemistry Chapter 12. This quiz covers important concepts such as solutions, solutes, and solvents. Use these flashcards to reinforce your knowledge and prepare for your chemistry exams.
