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Aqueous solution
A solution where water is the solvent.
Polar molecule
A molecule with uneven distribution of charge, leading to partial positive and negative ends.
Hydration
The process of water molecules surrounding and dissolving ions or molecules.
Solubility
The ability of a solute to dissolve in a solvent.
Solute
The substance being dissolved in a solution.
Solvent
The substance doing the dissolving in a solution (e.g., water in an aqueous solution).
Electrical conductivity
The ability of a solution to conduct electricity, depends on the presence of ions.
Strong electrolyte
A substance that completely dissociates into ions in solution (e.g., NaCl).
Weak electrolyte
A substance that only partially dissociates into ions in solution (e.g., CH₃COOH).
Nonelectrolyte
A substance that does not dissociate into ions in solution (e.g., sugar).
Strong acid
An acid that fully dissociates into ions in water (e.g., HCl).
Strong base
A base that fully dissociates into ions in water (e.g., NaOH).
Weak acid
An acid that only partially dissociates in water (e.g., acetic acid).
Weak base
A base that only partially dissociates in water (e.g., ammonia).
Molarity
Concentration of a solution, moles of solute per liter of solution (mol/L).
Standard solution
A solution with a known concentration, often used in titrations.
Dilution
Adding solvent to a solution to decrease its concentration.
Precipitation reaction
A reaction where two aqueous solutions form an insoluble solid (precipitate).
Precipitate
The solid that forms during a precipitation reaction.
Molecular equation
A chemical equation showing the complete formulas of all reactants and products.
Complete ionic equation
A chemical equation that shows all ions in the reaction.
Spectator ions
Ions that do not participate in the actual chemical reaction and remain unchanged.
Net ionic equation
A chemical equation that shows only the species that undergo change in a reaction.
Arrhenius acid
A substance that increases the concentration of H⁺ ions in water.
Arrhenius base
A substance that increases the concentration of OH⁻ ions in water.
Brønsted-Lowry acid
A proton (H⁺) donor.
Brønsted-Lowry base
A proton (H⁺) acceptor.
Neutralization reaction
A reaction between an acid and a base that produces water and a salt.
Volumetric analysis
A technique to determine the concentration of a solution through volume measurements.
Titration
A technique where a solution of known concentration is used to determine the concentration of another solution.
Titrant
The solution of known concentration in a titration.
Analyte
The substance being analyzed in a titration.
Equivalence point (stoichiometric point)
The point in a titration where moles of titrant equal moles of analyte.
Indicator
A substance that changes color at or near the equivalence point in a titration.
Endpoint
The point in a titration where the indicator changes color, signaling the titration is complete.
Acid-base titration
A titration process used to determine the concentration of an acid or base.
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