ICO Part B (ORI) study plan

Derive the titration error equations for strong acid–strong base, weak acid, and redox titrations, and compute the theoretical titration curve for three assigned systems by hand.

Calculate the equivalence-point pH for weak acid and weak base titrations from Ka/Kb and concentration, verifying each result against a mass-balance check.

Distinguish random from systematic error in a set of 20 hypothetical burette readings, and compute mean, standard deviation, and 95% confidence interval for each subset.

Propagate uncertainty through a gravimetric calculation (mass of precipitate to molarity of analyte) using both the quadrature and worst-case methods, and compare the outcomes.

Set up a spreadsheet that plots a titration curve from raw volume–pH data and marks the first and second derivative endpoints.

Solve five gravimetric problems requiring correction for solubility loss, coprecipitation, and ignition stoichiometry, and justify each correction numerically.

Derive the Beer–Lambert relationship from first principles and calculate the concentration of an unknown from a five-point calibration using least-squares regression.

Construct a calibration curve by hand from provided absorbance data, compute the slope, intercept, and R², and interpret whether the intercept is statistically different from zero.

Design a spectrophotometric determination for a two-component mixture using simultaneous equations, and state the wavelength-selection criteria you would apply.

Identify three sources of systematic bias in a colorimetric assay and propose a control experiment for each.

Derive integrated rate laws for zero-, first-, and second-order reactions and determine reaction order from three data sets using graphical and half-life methods.

Apply the Arrhenius equation to extract activation energy from rate constants at four temperatures, including correct units and error propagation.

Distinguish pseudo-first-order from true first-order kinetics and design an experiment that confirms the assumption.

Compute thermodynamic quantities (ΔG, ΔH, ΔS) from a van't Hoff plot and from calorimetric data, and reconcile any discrepancy between the two.

Explain how to treat non-linear Arrhenius behavior and state what experimental evidence would support it.

Calculate cell potentials from standard reduction potentials, apply the Nernst equation to concentration cells, and predict the direction of spontaneous reaction for five cells.

Interpret a potentiometric titration curve to locate the endpoint and explain the role of the indicator electrode in each of three cases.

Determine the number of ions and the transport number from conductivity measurements on a dilute electrolyte series.

Predict the geometry and magnetic moment of a set of coordination complexes using crystal-field theory, and identify which cases require ligand-field or Jahn–Teller arguments.

Explain how to measure a stability constant by potentiometric or spectrophotometric titration and state the assumptions of each method.

Assign the d–d transitions in an octahedral complex from a UV–vis spectrum and calculate Δo and the Racah parameter B.

Interpret IR spectra of coordination compounds to identify metal–ligand stretching modes and distinguish bridging from terminal ligands.

Predict the number of unpaired electrons and the expected magnetic moment for ten complexes, and flag the cases where spin-orbit coupling invalidates the spin-only formula.

Outline a synthesis of a coordination compound (e.g., a metal–acetylacetonate or a Werner-type complex) including purification by recrystallization and yield calculation.

Evaluate a set of analytical data (elemental analysis, IR, UV–vis, magnetic moment) to propose a structure and defend the proposal against one alternative.

Predict the outcome of ten named organic reactions and justify regioselectivity and stereoselectivity using mechanistic reasoning.

Design a separation scheme for a three-component mixture (acidic, basic, neutral) using liquid–liquid extraction, and specify the pH at each step.

Select a chromatographic method (TLC, column, GC, HPLC) for four given mixtures and justify each choice by polarity and volatility.

Interpret a combined ¹H NMR, ¹³C NMR, IR, and MS data set to assign a structure, and rationalize the fragmentation pattern.

Explain how to determine purity by melting point, chromatographic peak area, and elemental analysis, and state the limitations of each.

Classify ten laboratory hazards using GHS criteria and specify the control measure (substitution, engineering, administrative, PPE) for each.

Design a risk assessment for a reaction involving a pyrophoric reagent, a toxic gas, and a high-pressure vessel, including emergency procedures.

Select the correct waste stream and disposal route for eight chemical residues, and justify each classification.

Explain the safe handling of cryogenic liquids, compressed gas cylinders, and vacuum lines, and identify the failure mode of each system.

Describe the correct response to a mercury spill, a solvent fire, and a chemical splash, and state what documentation follows each.

Complete a full-length timed mock examination under exam conditions and record the score per domain.

Diagnose the three weakest domains from the mock and write a targeted revision list for each.

Re-derive from memory the key equations for titrimetry, kinetics, thermodynamics, and error propagation without reference material.

Review every flagged or uncertain item from earlier weeks and resolve each with a written justification.

Explain your reasoning aloud for five multi-step calculation problems to confirm fluency under time pressure.