Analytical Chemistry I

What you'll learn

• Describe the analytical process from problem definition to report, distinguish classical from instrumental and absolute from relative methods, and convert among concentration units including mg/L as CaCO₃ and nitrate as nitrogen.
• Use the analytical balance and Class A volumetric glassware correctly, weigh by difference, apply buoyancy corrections, calibrate glassware by weighing water, and prepare standard solutions from primary standards.
• Classify errors as systematic, random or gross, calculate means, standard deviations and relative standard deviations, propagate uncertainty through calculations, and build an uncertainty budget with standard and expanded uncertainties.
• Calculate confidence intervals with Student's t, compare a mean with a known value, compare two means with pooled, Welch and paired t tests, compare precisions with the F test, and apply the Grubbs test to suspected outliers.
• Construct least-squares calibration curves, interpret residual plots, calculate the concentration of an unknown with its uncertainty, determine detection and quantitation limits, and use standard additions and internal standards to deal with matrix effects.
• Calculate ionic strength and activity coefficients with the extended Debye–Hückel equation, explain the salt effect, and solve multi-equilibrium problems by the systematic treatment using charge and mass balances.
• Calculate fractional compositions of monoprotic and polyprotic acids, the pH of amphiprotic salts and any acid–base mixture from the charge balance, and design buffers with appropriate capacity, allowing for ionic strength and temperature.
• Standardize acid and base titrants, calculate exact titration curves for strong, weak and polyprotic acids, choose indicators, locate endpoints by derivative and Gran methods, and determine alkalinity and Kjeldahl nitrogen.
• Explain the chelate effect and EDTA complexation, calculate conditional formation constants and EDTA titration curves, choose metal ion indicators and titration techniques, and determine total and calcium hardness.
• Calculate argentometric titration curves, apply the Mohr, Volhard and Fajans methods, control particle size and purity in gravimetric analysis, and calculate results with gravimetric factors.
• Use formal potentials to calculate redox titration curves, choose redox indicators and titrants, carry out permanganate, cerium, iodimetric and iodometric calculations including the Winkler method, and explain potentiometry with pH and ion-selective electrodes.
• Apply quality assurance and quality control, validate a method, interpret control charts with Westgard rules and proficiency-test z-scores, check a water analysis with an ion balance, and write a clear analytical report.