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Questions and Answers
Why is water considered an excellent solvent?
Why is water considered an excellent solvent?
- It is non-polar and repulsive to other molecules.
- It is linear, allowing for easy penetration into crystal lattices.
- It is bent, polar, and capable of forming attractions with solutes. (correct)
- It is large and can easily surround molecules.
Dissolving a solute in a solvent always results in a chemical reaction that alters the solute's chemical properties.
Dissolving a solute in a solvent always results in a chemical reaction that alters the solute's chemical properties.
False (B)
What two factors primarily determine the solubility of ionic solids, influencing whether they will dissolve readily in water?
What two factors primarily determine the solubility of ionic solids, influencing whether they will dissolve readily in water?
size and charge
When an ionic compound dissociates in water, creating a solution that can conduct electricity, the compound is referred to as a(n) ________ .
When an ionic compound dissociates in water, creating a solution that can conduct electricity, the compound is referred to as a(n) ________ .
What best describes the effect of increased pressure on gas solubility in a liquid?
What best describes the effect of increased pressure on gas solubility in a liquid?
Saturated solutions contain less than the maximum amount of solute that can dissolve in a solvent at a given temperature.
Saturated solutions contain less than the maximum amount of solute that can dissolve in a solvent at a given temperature.
State two methods by which the dissolution rate of a solid solute in a solvent may be increased.
State two methods by which the dissolution rate of a solid solute in a solvent may be increased.
Match each type of solution with its property:
Match each type of solution with its property:
In a chemical reaction occurring in a solution producing a precipitate, what are the ions that do not participate in the reaction and remain free-floating called?
In a chemical reaction occurring in a solution producing a precipitate, what are the ions that do not participate in the reaction and remain free-floating called?
When diluting a solution by adding more solvent, the number of moles of solute changes proportionally with the volume increase.
When diluting a solution by adding more solvent, the number of moles of solute changes proportionally with the volume increase.
When preparing a solution from a solid solute, what is the correct procedure to ensure accuracy?
When preparing a solution from a solid solute, what is the correct procedure to ensure accuracy?
A solution which you have made, and for which you know the accurate concentration, is a(n) ________ .
A solution which you have made, and for which you know the accurate concentration, is a(n) ________ .
How does the addition of acids influence the hydrogen ion concentration in a solution?
How does the addition of acids influence the hydrogen ion concentration in a solution?
The number of significant figures in a concentration value is the same as the number of decimal places in its corresponding pH value.
The number of significant figures in a concentration value is the same as the number of decimal places in its corresponding pH value.
In the context of acid-base chemistry, what term describes the capability of a substance to act as both a proton donor and a proton acceptor?
In the context of acid-base chemistry, what term describes the capability of a substance to act as both a proton donor and a proton acceptor?
According to the Bronsted-Lowry concept, a(n) _________ is defined as a proton acceptor.
According to the Bronsted-Lowry concept, a(n) _________ is defined as a proton acceptor.
Within the context of acids that contain polyatomic ions, what suffix replacement is used to name the acids when an -ate suffix is present in the polyatomic ion?
Within the context of acids that contain polyatomic ions, what suffix replacement is used to name the acids when an -ate suffix is present in the polyatomic ion?
Halogen-containing acids always ionize completely in water and are therefore classified as weak acids.
Halogen-containing acids always ionize completely in water and are therefore classified as weak acids.
Describe the key distinction between a Lewis acid and a Lewis base in terms of electron pair behavior.
Describe the key distinction between a Lewis acid and a Lewis base in terms of electron pair behavior.
The process of determining the concentration of a solution by reacting it with a known amount of another solution is called ________ .
The process of determining the concentration of a solution by reacting it with a known amount of another solution is called ________ .
Flashcards
Solvent
Solvent
The component that retains its phase; usually present in a larger amount.
Solute
Solute
The component that dissolves in the solvent, often changing phase
Saturated Solution
Saturated Solution
A solution that contains the maximum amount of solute that can dissolve at a given temperature.
Electrolyte
Electrolyte
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Saturated
Saturated
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Unsaturated
Unsaturated
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Gas Solubility
Gas Solubility
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Solution
Solution
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Solubility
Solubility
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pH
pH
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Base
Base
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Acid
Acid
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Standard Solution
Standard Solution
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Amphiprotic
Amphiprotic
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Bronsted-Lowry Acid
Bronsted-Lowry Acid
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Bronsted-Lowry Base
Bronsted-Lowry Base
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Titration
Titration
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Aqueous Solution
Aqueous Solution
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Lewis Acid
Lewis Acid
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Lewis Base
Lewis Base
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Study Notes
- Solution chemistry involves dissolving chemicals in solvents to facilitate reactions.
- For reactions needing physical collisions, being dissolved maximizes surface area.
Water as a Solvent
- Water is a bent, polar, and small molecule.
- It is effective at attracting and surrounding solutes.
- Hydration occurs when water interacts with and surrounds ions/molecules.
- These water molecules orient themselves properly around the solute.
- These processes have thermochemical aspects.
Components of solutions
- The solvent retains its phase and is usually the larger amount in a solution
- Solutes dissolve into the solvent and usually change phase, and are the smaller amount in solution
Types of solutions
- solutions are classified as anything dissolved in anything else
- Oxygen in nitrogen and tin in copper are examples of non-liquid solutions
- Making a solution is a physical change, not a chemical reaction.
- The process is reversible
Key factor for dissolving
- Solute must be capable of being attracted to the solvent to dissolve.
Solubility rule
- Polarity determines the solubility of molecular compounds
- Polar dissolves in polar
- Non-polar dissolves in non-polar
- Size is also a solubility factor.
- Small molecules dissolve better than large ones.
Ionic compounds
- Ionic compounds dissociate into ions when in water.
- Example: Na2CO3(s) → 2 Na+(aq) + CO32-(aq)
- The subscript (aq) indicates ions dissolved in water.
Solubility vs Lattice Enthalpy Trends
- Solubility is related to lattice enthalpy.
- High lattice enthalpies result in lower solubility in H2O.
Electrolytes
- Solutions conduct electricity when ionic compounds dissociate in water
- Pure water and Gatorade are examples
Electrolytes classification
- Strong electrolytes efficiently conduct current.
- NaCl and HNO3 are strong electrolytes
- weak electrolytes conduct small amount of current due to a small amount of ions present
- Vinegar and tap water are weak electrolytes
- Non-electrolytes don't conduct current and only have molecules present
- Pure water and sugar solution are non-electrolytes
Effects of temperature
- Solid solubility increases at higher temperatures.
- Liquid-liquid solubility is negligibly affected
- Gas solubility decreases at higher temperatures
- Solubility trends can be visualized using a Solubility Curve
Effects Of Pressure
- Pressure changes negligibly affect liquids and solids.
- Gas solubility is directly proportional to the pressure of the gas above the liquid.
Solubility and oceans
- Increase in atmospheric partial pressure of CO2 leads to more CO2 dissolving in oceans
- Carbonic acid forms and lowers the pH, harming certain wildlife
Soap
- Surrounds non-polar fats/greases for dissolving into water due to its polar and non-polar ends
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