Term
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Definition
| Homogenous mixtures of two or more substances and consists of a solvent(usually water) and one or more solutes. |
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Term
| What is the nature of solutes in solutions? |
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Definition
Spread evenly throughout the solution.
Cannot be seperated from the solvent by filtration.
Can be seperated by evaporation.
Are not visible, but can give a color to the solution. |
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Term
| What are the properties of water in solutions? |
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Definition
Water is the most common solvent and is known as the universal solvent.
Water solutions are known as aqueous(aq) solutions.
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Term
| What causes hydrogen bonding in water molecules? |
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Definition
| because each end of the water molecule are opposite charges the attract one another giving water a high boiling point for such a small molecule. |
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Term
| What happens when an ionic compound is placed in water? |
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Definition
| water molecules can start to interact with ions in the crystal lattice and pull the bonds apart. |
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Term
| How is an ionic compound insoluble? |
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Definition
| If the pull of the water molecules is not strong enough to overcome the attractions among ions in the crystal lattice, the compound will not dissolve. |
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Term
| How is an ionic compound soluble? |
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Definition
| if the pull of water molecules is strong enough to overcome attractions among the ions, water can pull the crystal apart and dissolve the compound. |
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Term
| What are properties of strong electrolytes? |
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Definition
dissociate in water, producing positive and negative ions.
conduct an electric current in water.
in equations show the formation of ions in aqueous(aq) solutions. |
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Term
| What are properties of weak electolytes? |
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Definition
dissociate only slightly in water.
in water forms a solution of a few ions and mostly undissociated molecules |
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Term
| What are properties of nonelectrolytes? |
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Definition
dissolve as molecules in water.
do not produce ions in water.
form solutions that do not conduct an electric current. |
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Term
| What are metathesis reactions? |
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Definition
are also called double replacement reactions.
involve a trading of ion partners.
are driven by a) the formation of participates, b) the formation of a molecular liquid, or c) the formation of a molecular gas |
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Term
| What are precipitation reactions? |
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Definition
| Metathesis reactions that result in the formation of an insoluble solid. |
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Term
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Definition
| a physical property describing how readily a substance will dissolve in a given solvent. |
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Term
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Definition
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Term
| What do acid base neutralization reactions produce? |
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Definition
| Salt(any ionic compound that is not a hydroxide or oxide) and water |
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Term
| What do oxidation reduction reactions involve? |
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Definition
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Term
| What are oxidation number(oxidation states)? |
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Definition
| number assigned to atoms to help keep track of electrons lost or gained during a redox reaction. |
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Term
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Definition
| increase in oxidation number or loss of electrons |
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Term
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Definition
| decrease in oxidation number or gain of electrons |
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Term
| What is the oxidizing agent or oxidant? |
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Definition
reactant that causes another reactant to become oxidized in a reaction.
oxidants are reduced in a reaction |
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Term
| What is the reducing agent or reductant? |
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Definition
reactant that causes another reactant to become reduced.
reductants are oxidized in a reaction |
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Term
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Definition
the amount of substance dissolved in a solvent. expressed as
g of solute
100 g water |
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Term
| What are unsaturated solutions? |
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Definition
| solutions that contain less than the maximum amount of solute that can be dissolved in the solvent. |
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Term
| What are saturated solutions? |
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Definition
contain maximum amount of solute that can be dissolved in the solvent.
has particles of undissolved solute in the bottom of container |
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Term
| How do you find the mass percent of a solution? |
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Definition
grams of solute/grams of solute+grams of solvent
then multiply by 100
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Term
| how do you find the concentration of a solution? |
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Definition
| amount of solute/amount of solution |
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Term
| How do you find the volume percent of a solution? |
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Definition
mL of solute/mL of solution
multiply by 100 |
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Term
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Definition
| a concentration term for solution and is represented as moles of solute per liter of solution |
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