Unit 10: Big Idea 6
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Overview
Learning Objectives 1.20, 2.2, 3.3, 3.7, 6.11, 6.14, 6.19 Textbook Chapters 16 Time Frame: 5 |
10.1 Colorimetric pH Meter
LO 2.2 I can explain the relative strengths of acids and bases based on molecular structure, interparticle forces, ad solution equilibrium.
Groundwork for
LO 6.11 I can generate or use a particulate representation of an acid (strong or weak or polyprotic) and a strong base to explain the species that will have large versus small concentrations at equilibrium.
LO 6.15 I can identify a given solution as containing a mixture of strong acids and/or bases and calculate or estimate the pH (and concentrations of all chemical species) in the resulting solution.
Groundwork for
LO 6.11 I can generate or use a particulate representation of an acid (strong or weak or polyprotic) and a strong base to explain the species that will have large versus small concentrations at equilibrium.
LO 6.15 I can identify a given solution as containing a mixture of strong acids and/or bases and calculate or estimate the pH (and concentrations of all chemical species) in the resulting solution.
Exploration Objectives
- What is the difference in pH between an acid and a base?
- What is the relationship between pH & pOH?
- How are pH & pOH related to [H+] & [OH-] respectively?
- What differences did you observe between Universal Indicator and the other indicators?
- If you know a neutralization reaction will occur at a pH of 5 and a different neutralization reaction will occur around a pH of 9, would you choose the same indicator or different indicators? Why?
- What are indicators? How do they work? Do they have limits? (Provide specific examples from your lab.)
10.2 Acid Base Equilibria
LO 3.7 I can identify compounds as Bronsted-Lowry acids, bases, and/or conjugate acid-base pairs, using proton-transfer reactions to justify the identification.
LO 6.11 I can generate or use a particulate representation of an acid (strong or weak or polyprotic) and a strong base to explain the species that will have large versus small concentrations at equilibrium.
LO 6.14 I can, based on the dependence of Kw on temperature, reason that neutrality requires [H+]=[OH-] as opposed to requiring pH=7, including especially the applications to biological systems.
Groundwork for
LO 6.12 I can reason about the distinction between strong and weak acid solutions with similar values of pH, including the percent ionization of the acids, the concentrations needed to achieve the same pH, and the amount of base needed to reach the equivalence point in a titration.
LO 6.13 I can interpret titration data for monoprotic or polyprotic acids involving titration of a weak or strong acid by a strong base (or a weak or strong base by a strong acid) to determine the concentration of the titrant and the pKa for a weak acid, or the pKb for a weak base.
LO 6.19 I can relate the predominant form of a chemical species involving a labile proton (i.e., protonated/deprotonated form of a weak acid) to the pH of a solution and the pKa associated with the labile proton.
LO 6.11 I can generate or use a particulate representation of an acid (strong or weak or polyprotic) and a strong base to explain the species that will have large versus small concentrations at equilibrium.
LO 6.14 I can, based on the dependence of Kw on temperature, reason that neutrality requires [H+]=[OH-] as opposed to requiring pH=7, including especially the applications to biological systems.
Groundwork for
LO 6.12 I can reason about the distinction between strong and weak acid solutions with similar values of pH, including the percent ionization of the acids, the concentrations needed to achieve the same pH, and the amount of base needed to reach the equivalence point in a titration.
LO 6.13 I can interpret titration data for monoprotic or polyprotic acids involving titration of a weak or strong acid by a strong base (or a weak or strong base by a strong acid) to determine the concentration of the titrant and the pKa for a weak acid, or the pKb for a weak base.
LO 6.19 I can relate the predominant form of a chemical species involving a labile proton (i.e., protonated/deprotonated form of a weak acid) to the pH of a solution and the pKa associated with the labile proton.
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Quiz #1: Sect. 10.1-10.2
Guided Inquiry Lab - Investigation #4
LO 1.20 I can design, and/or interpret data from an experiment that uses titration to determine the concentration of an analyte in a solution.
LO 3.3 I can use stoichiometric calculations to predict the results of performing a reaction in the laboratory and/or to analyze deviations from the expected results.
LO 3.3 I can use stoichiometric calculations to predict the results of performing a reaction in the laboratory and/or to analyze deviations from the expected results.
Why do some foods, like carbonated beverages and orange juice, irritate the esophagus? Why do they exacerbate heart burn?
Titration is used to calculate specific ratios of different substances using volume measurements
- Determine how much acid is in fruit juice and soft drinks
Titration is used to calculate specific ratios of different substances using volume measurements
- by doctors and pharmacists to monitor blood glucose levels, to analyze urine samples, to conduct pregnancy tests, or when compounding drugs for a person's prescription.
- by food scientists when testing for levels of salt, sugar and vitamins in different foods; including determining if items like cheese or wine are fit for consumption.