Solubility Rules - MCAT Chemical and Physical Foundations of Biological Systems
Card 1 of 56
Which of the following molecules is insoluble?
Which of the following molecules is insoluble?
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These solubility rules should be known for the MCAT and are presented as a hierarchy.
1. All group 1 salts and ammonium salts are soluble
2. All nitrates, perchlorates, and acetates are soluble
3. All mercury, lead, and silver salts are NOT soluble
Understanding these solubility rules as a hierarchy, we can understand why Mg(NO3)2 and AgNO3 are soluble and why AgCl is not soluble.
These solubility rules should be known for the MCAT and are presented as a hierarchy.
1. All group 1 salts and ammonium salts are soluble
2. All nitrates, perchlorates, and acetates are soluble
3. All mercury, lead, and silver salts are NOT soluble
Understanding these solubility rules as a hierarchy, we can understand why Mg(NO3)2 and AgNO3 are soluble and why AgCl is not soluble.
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Which of the following reactions will produce a precipitate?
Which of the following reactions will produce a precipitate?
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Knowledge of basic solubility rules is enough to answer this question. Nitrates and salts of alkali metals are always soluble, as are salts of ammonium. Acetates are also always soluble. Acid-base reactions, such as with hydrofluoric acid, produce a soluble salt and water. Sulfates are commonly soluble, with certain exceptions (mostly alkaline earth metals).
The only reaction that produces an insoluble product is that between silver nitrate and potassium chloride. Silver chloride is a common precipitate obtained in double replacement reactions.
Knowledge of basic solubility rules is enough to answer this question. Nitrates and salts of alkali metals are always soluble, as are salts of ammonium. Acetates are also always soluble. Acid-base reactions, such as with hydrofluoric acid, produce a soluble salt and water. Sulfates are commonly soluble, with certain exceptions (mostly alkaline earth metals).
The only reaction that produces an insoluble product is that between silver nitrate and potassium chloride. Silver chloride is a common precipitate obtained in double replacement reactions.
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Which of the following compounds would be generally insoluble in an aqueous solution?
Which of the following compounds would be generally insoluble in an aqueous solution?
Tap to reveal answer
Knowing some of the general solubility trends will greatly facilitate your understanding of solubility in chemistry. Here are a couple guidelines you can follow in order to predict which compounds are soluble.
1. Compounds containing alkali metals, ammonium cations, or nitrate anions are soluble.
2. Compounds containing halogen anions are soluble. Key exceptions are halogens attached to silver, mercury, and lead.
3. Sulfates are soluble, except when attached to heavier alkaline metals, like barium (thus the correct answer).
4. Carbonates, phosphates, and hydroxides are generally insoluble; however, if they are attached to one of the ions mentioned in one of the above points, they are soluble.
Knowing some of the general solubility trends will greatly facilitate your understanding of solubility in chemistry. Here are a couple guidelines you can follow in order to predict which compounds are soluble.
1. Compounds containing alkali metals, ammonium cations, or nitrate anions are soluble.
2. Compounds containing halogen anions are soluble. Key exceptions are halogens attached to silver, mercury, and lead.
3. Sulfates are soluble, except when attached to heavier alkaline metals, like barium (thus the correct answer).
4. Carbonates, phosphates, and hydroxides are generally insoluble; however, if they are attached to one of the ions mentioned in one of the above points, they are soluble.
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Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law, 
is the mole fraction of the solvent, 
is the vapor pressure of the pure solvent, and 
is the vapor pressure of the solution. When this vapor pressure is equal to the local atmospheric pressure, the solution boils.
A scientist is studying boiling point changes with the addition of solutes, and creates a colloid. A colloid is similar to a solution because both will possess which of the following characteristics?
I. They both show the Tyndall effect on light
II. They both involve the suspension of only molecular-sized particles
III. They both involve the suspension of particles that are too small to be individually distinguished with the naked eye
Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law,
A scientist is studying boiling point changes with the addition of solutes, and creates a colloid. A colloid is similar to a solution because both will possess which of the following characteristics?
I. They both show the Tyndall effect on light
II. They both involve the suspension of only molecular-sized particles
III. They both involve the suspension of particles that are too small to be individually distinguished with the naked eye
Tap to reveal answer
A colloid is a suspension of particles larger than molecules, but too small to be individually distinguished by the naked eye. Only colloids disperse light by the Tyndall effect. Milk is an example of a colloid.
A colloid is a suspension of particles larger than molecules, but too small to be individually distinguished by the naked eye. Only colloids disperse light by the Tyndall effect. Milk is an example of a colloid.
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All of the following compounds are soluble in water except .
All of the following compounds are soluble in water except .
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Compounds that contain sulfate groups ( 
)are soluble in water, unless they are bound to mercury, strontium, lead, calcium, or barium. Hence, barium sulfate, 
, is insoluble in water.
Compounds that contain nitrates (
), ammonium ( 
), and alkali metals are generally soluble in water. Compounds containing halogens are soluble in water unless they are bound to mercury, lead, or silver.
Compounds that contain sulfate groups (
Compounds that contain nitrates (
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Which compound is most likely to be soluble in pentane?
Which compound is most likely to be soluble in pentane?
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Molecules are most soluble in solvents that possess similar properties and intermolecular forces to the solute.
Pentane is a non-polar compound, which interacts predominately through london dispersion forces. Ammonia, silver chloride, and phosphorus trichloride are all polar molecules. Ammonia has a lone pair on the nitrogen; silver is an ionic compound; phosphorus trichloride has lone pairs on both the phosphorus and chlorine atoms.
In contrast, carbon dioxide has lone pairs only on the oxygen atoms and has a linear geometry. This creates a line of symmetry in the molecule such that the net polarities of the carbon-oxygen bonds cancel each other. Even though carbon dioxide has polar bonds, it is not a polar molecule and would likely dissolve in pentane.
Molecules are most soluble in solvents that possess similar properties and intermolecular forces to the solute.
Pentane is a non-polar compound, which interacts predominately through london dispersion forces. Ammonia, silver chloride, and phosphorus trichloride are all polar molecules. Ammonia has a lone pair on the nitrogen; silver is an ionic compound; phosphorus trichloride has lone pairs on both the phosphorus and chlorine atoms.
In contrast, carbon dioxide has lone pairs only on the oxygen atoms and has a linear geometry. This creates a line of symmetry in the molecule such that the net polarities of the carbon-oxygen bonds cancel each other. Even though carbon dioxide has polar bonds, it is not a polar molecule and would likely dissolve in pentane.
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Substances for which pure water would not be an efficient solvent are .
Substances for which pure water would not be an efficient solvent are .
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Since water is polar, it dissolves substances that have electrostatic charge due to electron arrangement. All of the answer choices describe molecules that would have positive and negative components except those with evenly dispersed electrons. This describes a nonpolar molecule, which would not dissolve in water.
Since water is polar, it dissolves substances that have electrostatic charge due to electron arrangement. All of the answer choices describe molecules that would have positive and negative components except those with evenly dispersed electrons. This describes a nonpolar molecule, which would not dissolve in water.
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Which salt will produce a basic solution when dissolved in water?
Which salt will produce a basic solution when dissolved in water?
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When 
is dissolved in water, it forms 
and 
. Both of these are basic compounds.
Each of the other answer options will result in at least one acidic compound when dissolved in solution.
When
Each of the other answer options will result in at least one acidic compound when dissolved in solution.
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Which of the following molecules is insoluble?
Which of the following molecules is insoluble?
Tap to reveal answer
These solubility rules should be known for the MCAT and are presented as a hierarchy.
1. All group 1 salts and ammonium salts are soluble
2. All nitrates, perchlorates, and acetates are soluble
3. All mercury, lead, and silver salts are NOT soluble
Understanding these solubility rules as a hierarchy, we can understand why Mg(NO3)2 and AgNO3 are soluble and why AgCl is not soluble.
These solubility rules should be known for the MCAT and are presented as a hierarchy.
1. All group 1 salts and ammonium salts are soluble
2. All nitrates, perchlorates, and acetates are soluble
3. All mercury, lead, and silver salts are NOT soluble
Understanding these solubility rules as a hierarchy, we can understand why Mg(NO3)2 and AgNO3 are soluble and why AgCl is not soluble.
← Didn't Know|Knew It →
Which of the following reactions will produce a precipitate?
Which of the following reactions will produce a precipitate?
Tap to reveal answer
Knowledge of basic solubility rules is enough to answer this question. Nitrates and salts of alkali metals are always soluble, as are salts of ammonium. Acetates are also always soluble. Acid-base reactions, such as with hydrofluoric acid, produce a soluble salt and water. Sulfates are commonly soluble, with certain exceptions (mostly alkaline earth metals).
The only reaction that produces an insoluble product is that between silver nitrate and potassium chloride. Silver chloride is a common precipitate obtained in double replacement reactions.
Knowledge of basic solubility rules is enough to answer this question. Nitrates and salts of alkali metals are always soluble, as are salts of ammonium. Acetates are also always soluble. Acid-base reactions, such as with hydrofluoric acid, produce a soluble salt and water. Sulfates are commonly soluble, with certain exceptions (mostly alkaline earth metals).
The only reaction that produces an insoluble product is that between silver nitrate and potassium chloride. Silver chloride is a common precipitate obtained in double replacement reactions.
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Which of the following compounds would be generally insoluble in an aqueous solution?
Which of the following compounds would be generally insoluble in an aqueous solution?
Tap to reveal answer
Knowing some of the general solubility trends will greatly facilitate your understanding of solubility in chemistry. Here are a couple guidelines you can follow in order to predict which compounds are soluble.
1. Compounds containing alkali metals, ammonium cations, or nitrate anions are soluble.
2. Compounds containing halogen anions are soluble. Key exceptions are halogens attached to silver, mercury, and lead.
3. Sulfates are soluble, except when attached to heavier alkaline metals, like barium (thus the correct answer).
4. Carbonates, phosphates, and hydroxides are generally insoluble; however, if they are attached to one of the ions mentioned in one of the above points, they are soluble.
Knowing some of the general solubility trends will greatly facilitate your understanding of solubility in chemistry. Here are a couple guidelines you can follow in order to predict which compounds are soluble.
1. Compounds containing alkali metals, ammonium cations, or nitrate anions are soluble.
2. Compounds containing halogen anions are soluble. Key exceptions are halogens attached to silver, mercury, and lead.
3. Sulfates are soluble, except when attached to heavier alkaline metals, like barium (thus the correct answer).
4. Carbonates, phosphates, and hydroxides are generally insoluble; however, if they are attached to one of the ions mentioned in one of the above points, they are soluble.
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Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law, is the mole fraction of the solvent, is the vapor pressure of the pure solvent, and is the vapor pressure of the solution. When this vapor pressure is equal to the local atmospheric pressure, the solution boils.
A scientist is studying boiling point changes with the addition of solutes, and creates a colloid. A colloid is similar to a solution because both will possess which of the following characteristics?
I. They both show the Tyndall effect on light
II. They both involve the suspension of only molecular-sized particles
III. They both involve the suspension of particles that are too small to be individually distinguished with the naked eye
Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law,
A scientist is studying boiling point changes with the addition of solutes, and creates a colloid. A colloid is similar to a solution because both will possess which of the following characteristics?
I. They both show the Tyndall effect on light
II. They both involve the suspension of only molecular-sized particles
III. They both involve the suspension of particles that are too small to be individually distinguished with the naked eye
Tap to reveal answer
A colloid is a suspension of particles larger than molecules, but too small to be individually distinguished by the naked eye. Only colloids disperse light by the Tyndall effect. Milk is an example of a colloid.
A colloid is a suspension of particles larger than molecules, but too small to be individually distinguished by the naked eye. Only colloids disperse light by the Tyndall effect. Milk is an example of a colloid.
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All of the following compounds are soluble in water except .
All of the following compounds are soluble in water except .
Tap to reveal answer
Compounds that contain sulfate groups ( )are soluble in water, unless they are bound to mercury, strontium, lead, calcium, or barium. Hence, barium sulfate, , is insoluble in water.
Compounds that contain nitrates ( ), ammonium ( ), and alkali metals are generally soluble in water. Compounds containing halogens are soluble in water unless they are bound to mercury, lead, or silver.
Compounds that contain sulfate groups (
Compounds that contain nitrates (
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Which compound is most likely to be soluble in pentane?
Which compound is most likely to be soluble in pentane?
Tap to reveal answer
Molecules are most soluble in solvents that possess similar properties and intermolecular forces to the solute.
Pentane is a non-polar compound, which interacts predominately through london dispersion forces. Ammonia, silver chloride, and phosphorus trichloride are all polar molecules. Ammonia has a lone pair on the nitrogen; silver is an ionic compound; phosphorus trichloride has lone pairs on both the phosphorus and chlorine atoms.
In contrast, carbon dioxide has lone pairs only on the oxygen atoms and has a linear geometry. This creates a line of symmetry in the molecule such that the net polarities of the carbon-oxygen bonds cancel each other. Even though carbon dioxide has polar bonds, it is not a polar molecule and would likely dissolve in pentane.
Molecules are most soluble in solvents that possess similar properties and intermolecular forces to the solute.
Pentane is a non-polar compound, which interacts predominately through london dispersion forces. Ammonia, silver chloride, and phosphorus trichloride are all polar molecules. Ammonia has a lone pair on the nitrogen; silver is an ionic compound; phosphorus trichloride has lone pairs on both the phosphorus and chlorine atoms.
In contrast, carbon dioxide has lone pairs only on the oxygen atoms and has a linear geometry. This creates a line of symmetry in the molecule such that the net polarities of the carbon-oxygen bonds cancel each other. Even though carbon dioxide has polar bonds, it is not a polar molecule and would likely dissolve in pentane.
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Substances for which pure water would not be an efficient solvent are .
Substances for which pure water would not be an efficient solvent are .
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Since water is polar, it dissolves substances that have electrostatic charge due to electron arrangement. All of the answer choices describe molecules that would have positive and negative components except those with evenly dispersed electrons. This describes a nonpolar molecule, which would not dissolve in water.
Since water is polar, it dissolves substances that have electrostatic charge due to electron arrangement. All of the answer choices describe molecules that would have positive and negative components except those with evenly dispersed electrons. This describes a nonpolar molecule, which would not dissolve in water.
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Which salt will produce a basic solution when dissolved in water?
Which salt will produce a basic solution when dissolved in water?
Tap to reveal answer
When is dissolved in water, it forms and . Both of these are basic compounds.
Each of the other answer options will result in at least one acidic compound when dissolved in solution.
When
Each of the other answer options will result in at least one acidic compound when dissolved in solution.
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Which of the following molecules is insoluble?
Which of the following molecules is insoluble?
Tap to reveal answer
These solubility rules should be known for the MCAT and are presented as a hierarchy.
1. All group 1 salts and ammonium salts are soluble
2. All nitrates, perchlorates, and acetates are soluble
3. All mercury, lead, and silver salts are NOT soluble
Understanding these solubility rules as a hierarchy, we can understand why Mg(NO3)2 and AgNO3 are soluble and why AgCl is not soluble.
These solubility rules should be known for the MCAT and are presented as a hierarchy.
1. All group 1 salts and ammonium salts are soluble
2. All nitrates, perchlorates, and acetates are soluble
3. All mercury, lead, and silver salts are NOT soluble
Understanding these solubility rules as a hierarchy, we can understand why Mg(NO3)2 and AgNO3 are soluble and why AgCl is not soluble.
← Didn't Know|Knew It →
Which of the following reactions will produce a precipitate?
Which of the following reactions will produce a precipitate?
Tap to reveal answer
Knowledge of basic solubility rules is enough to answer this question. Nitrates and salts of alkali metals are always soluble, as are salts of ammonium. Acetates are also always soluble. Acid-base reactions, such as with hydrofluoric acid, produce a soluble salt and water. Sulfates are commonly soluble, with certain exceptions (mostly alkaline earth metals).
The only reaction that produces an insoluble product is that between silver nitrate and potassium chloride. Silver chloride is a common precipitate obtained in double replacement reactions.
Knowledge of basic solubility rules is enough to answer this question. Nitrates and salts of alkali metals are always soluble, as are salts of ammonium. Acetates are also always soluble. Acid-base reactions, such as with hydrofluoric acid, produce a soluble salt and water. Sulfates are commonly soluble, with certain exceptions (mostly alkaline earth metals).
The only reaction that produces an insoluble product is that between silver nitrate and potassium chloride. Silver chloride is a common precipitate obtained in double replacement reactions.
← Didn't Know|Knew It →
Which of the following compounds would be generally insoluble in an aqueous solution?
Which of the following compounds would be generally insoluble in an aqueous solution?
Tap to reveal answer
Knowing some of the general solubility trends will greatly facilitate your understanding of solubility in chemistry. Here are a couple guidelines you can follow in order to predict which compounds are soluble.
1. Compounds containing alkali metals, ammonium cations, or nitrate anions are soluble.
2. Compounds containing halogen anions are soluble. Key exceptions are halogens attached to silver, mercury, and lead.
3. Sulfates are soluble, except when attached to heavier alkaline metals, like barium (thus the correct answer).
4. Carbonates, phosphates, and hydroxides are generally insoluble; however, if they are attached to one of the ions mentioned in one of the above points, they are soluble.
Knowing some of the general solubility trends will greatly facilitate your understanding of solubility in chemistry. Here are a couple guidelines you can follow in order to predict which compounds are soluble.
1. Compounds containing alkali metals, ammonium cations, or nitrate anions are soluble.
2. Compounds containing halogen anions are soluble. Key exceptions are halogens attached to silver, mercury, and lead.
3. Sulfates are soluble, except when attached to heavier alkaline metals, like barium (thus the correct answer).
4. Carbonates, phosphates, and hydroxides are generally insoluble; however, if they are attached to one of the ions mentioned in one of the above points, they are soluble.
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Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law, is the mole fraction of the solvent, is the vapor pressure of the pure solvent, and is the vapor pressure of the solution. When this vapor pressure is equal to the local atmospheric pressure, the solution boils.
A scientist is studying boiling point changes with the addition of solutes, and creates a colloid. A colloid is similar to a solution because both will possess which of the following characteristics?
I. They both show the Tyndall effect on light
II. They both involve the suspension of only molecular-sized particles
III. They both involve the suspension of particles that are too small to be individually distinguished with the naked eye
Boiling point is the temperature a liquid needs to achieve in order to begin its transformation into a gaseous state. Campers and hikers who prepare food during their trips have to account for differences in atmospheric pressure as they ascend in elevation. During the ascent, the decrease in atmospheric pressure changes the temperature at which water boils.
Further complicating the matter is the observation that addition of a solute to a pure liquid also changes the boiling point. Raoult’s Law can be used to understand the changes in boiling point if a non-volatile solute is present, as expressed here.
In this law,
A scientist is studying boiling point changes with the addition of solutes, and creates a colloid. A colloid is similar to a solution because both will possess which of the following characteristics?
I. They both show the Tyndall effect on light
II. They both involve the suspension of only molecular-sized particles
III. They both involve the suspension of particles that are too small to be individually distinguished with the naked eye
Tap to reveal answer
A colloid is a suspension of particles larger than molecules, but too small to be individually distinguished by the naked eye. Only colloids disperse light by the Tyndall effect. Milk is an example of a colloid.
A colloid is a suspension of particles larger than molecules, but too small to be individually distinguished by the naked eye. Only colloids disperse light by the Tyndall effect. Milk is an example of a colloid.
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