Segment I: Titration Lab Results and pH
Segment I: Titration Lab Results and pH
In this segment, the students discuss the data from their titration lab. Our host explains the importance of titration in real world applications and discusses auto ionization of water and the calculation of pH.
Obtain, evaluate, and communicate information about the properties that describe solutions and the nature of acids and bases.
Use mathematics and computational thinking to compare, contrast, and evaluate the nature of acids and bases in terms of percent dissociation, hydronium ion concentration, and pH.
Plan and carry out an investigation to explore acid-base neutralization.
Obtain, evaluate, and communicate information to explain the properties of solutions.
Obtain and communicate information to explain the relationship between the structure and properties (e.g., pH, and color change in the presence of an indicator) of acids and bases.
Plan and carry out investigations to detect patterns in order to classify common household substances as acidic, basic, or neutral.
acid - substances that ionize in solutions to form H^+ ions.
amphoteric - a substance that can be an acid or a base.
Arrhenius Model - in aqueous solutions, acids form hydrogen ions (H^+).
base - substances that ionize in solutions and form OH^- ions.
binary acids - acids that do not contain oxygen in their chemical formula.
boiling point elevation - occurs when the boiling point of a solution is higher than the boiling point of the pure solvent alone.
Bronsted-Lowry Model - this model states that any compound that can transfer a proton to any other compound is an acid, and the compound that accepts the proton is a base.
colligative properties - properties of the solution that are different than those of a pure solvent by itself.
dilution - the process of adding more solvent to a solution.
electrolysis - the decomposition of water.
freezing point depression - a colligative property that describes how the freezing point of a solution is lowered compared to the freezing point of the pure solvent.
heterogeneous mixture - a combination of two or more substances in which the original substances are separated into physically distinct regions with differing properties.
homogeneous mixture - a combination of two or more substances that have uniform composition and chemical properties throughout; also known as a solution.
insoluble - a solid, liquid, or gas that will not dissolve in a particular solvent.
Lewis Model - bases donate pairs of electrons and acids accept pairs of electrons.
mass percent - a way of expressing how concentrated a solution is; is equal to the mass of the solute in a solution divided by the total mass of the solution and multiplying by 100.
mixture - a combination of two or more pure substances in which each pure substance retains its individual chemical properties.
molality - a ratio of moles of solute to the mass of the solvent in kilograms.
molarity - a ratio of moles of solute to the volume of the solution in liters.
oxyacids - acids that contain oxygen in their chemical formula.
pure substance - a material that has a constant composition and has consistent properties throughout the sample.
saturated solution - a solution in which the maximum amount of solute has been dissolved in a given amount of solvent at a particular temperature.
saturation point - the point at which no more solute can be dissolved in the solution at that particular temperature.
solubility - the maximum amount of a substance that can be dissolved in a given quantity of solvent at a given temperature to produce a saturated solution.
solute - the substance that is being dissolved in a solution.
solution - a liquid mixture in which the solute is uniformly distributed within the solvent.
solvent - the substance that is present in a greater amount in a solution.
supersaturated solution - a solution that is holding more dissolved solute than what it normally would hold at that temperature.
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