relevant Ksp values. 2B: Generate or use a particulate representation of an 6.21 acid and a strong base to explain the species that will have large versus small concentrations at equilibrium. 6.11 4: Interpret data regarding solubility 3C: Identify a given solution as being the solution of a monoprotic of salts to determine, 2C: Identify and define titration, equivalence point, weak acid or base (including salts in which one ion is a weak acid or rank, the relevant indicator, monoprotic, diprotic, polyprotic. or base), calculate the pH and concentration of all species in the Ksp values. 6.22 solution, and/or infer the relative strengths of the weak acids or 2C: Distinguish between strong and weak acid solutions bases from given equilibrium concentrations. (6.15) 4: Interpret data with similar values of pH, including the percent regarding the ionization of the acids, the concentrations needed to relative solubility of achieve the same pH, and the amount of base needed to salts in terms of reach the equivalence point in a titration. 6.12 factors (common ions, pH) that 3D: Given an arbitrary mixture of weak and strong acids and bases, influence the 2D: Identify and define weak acid, strong acid, weak determine which species will react strongly with one another and solubility. 6.23 base, strong acid. what species will be present in large concentrations at equilibrium. (6.17) 2D: Identify and define acid/base indicators. 2D: Determine the appropriate indicator for use in a titration 3E: Design a buffer solution with a target pH and buffer capacity by selecting an appropriate conjugate acid-base pair and estimating the 2E: Identify and define conjugate acid/base pairs, buffer, concentrations needed to achieve the desired capacity. (6.18) buffer capacity. 2E: Identify a solution as being a buffer solution and explain the buffer mechanism in terms of the reactions that would occur on addition of acid or base. 3F: Relate the predominant form of a chemical species involving a labile proton to the pH of a solution and the pK associated with the 2F: Identify and define pKa, Henderson-Hasselbalch labile proton. (6.19) equation.
relevant Ksp values. 6.21 4: Interpret data regarding solubility of salts to determine, or rank, the relevant Ksp values. 6.22 4: Interpret data regarding the relative solubility of salts in terms of factors (common ions, pH) that influence the solubility. 6.23 3C: Identify a given solution as being the solution of a monoprotic weak acid or base (including salts in which one ion is a weak acid or base), calculate the pH and concentration of all species in the solution, and/or infer the relative strengths of the weak acids or bases from given equilibrium concentrations. (6.15) 3D: Given an arbitrary mixture of weak and strong acids and bases, determine which species will react strongly with one another and what species will be present in large concentrations at equilibrium. (6.17) 3E: Design a buffer solution with a target pH and buffer capacity by selecting an appropriate conjugate acid-base pair and estimating the concentrations needed to achieve the desired capacity. (6.18) 3F: Relate the predominant form of a chemical species involving a labile proton to the pH of a solution and the pK associated with the labile proton. (6.19) 2B: Generate or use a particulate representation of an acid and a strong base to explain the species that will have large versus small concentrations at equilibrium. 6.11 2C: Identify and define titration, equivalence point, indicator, monoprotic, diprotic, polyprotic. 2C: Distinguish 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. 6.12 2D: Identify and define weak acid, strong acid, weak base, strong acid. 2D: Identify and define acid/base indicators. 2D: Determine the appropriate indicator for use in a titration 2E: Identify and define conjugate acid/base pairs, buffer, buffer capacity. 2E: Identify a solution as being a buffer solution and explain the buffer mechanism in terms of the reactions that would occur on addition of acid or base. 2F: Identify and define pKa, Henderson-Hasselbalch equation.
ap_chemistry_curriculum_guide_17-18.docx