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Understanding Titration Errors & Purity Calculations in Chemistry Lab

This guide explains titration concepts, standardization calculations, and purity determination in chemistry labs. Learn about titration types and techniques for accurate measurements. Explore gravimetric analysis procedures and precipitation mechanisms.

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Understanding Titration Errors & Purity Calculations in Chemistry Lab

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  1. Ch 6: Good Titrations

  2. aA + tT → products analyte titrant e.g. H2SO4 + 2 NaOH → 2H2O + Na2SO4 indicator = added compound that undergoes a color change at the eq. pt. end point = end of titration when analyte moles are completely consumed and the indicator changes color equivalence point = theoretical end of titration as calculated using stoichiometry, e.g. 1 mol H2SO4/2 mol NaOH titration error = difference between the end point and the eq. pt. volumes

  3. "Standardization" = process where the concentration of the titrant is determined exactly using a…. "Primary Standard" = ultrapure reagent where the number of moles is known exactly so it can be used to accurately measure the titrant concentration, e.g. 2HCl + Na2CO3→ CO2 + H2O + 2NaCl ?? M primary standard (MW = 105.99) 99.99% pure

  4. Titration Types 1. acid-base HCl + NaOH → H2O + NaCl 2. redox 5NaC2O4 + 2 KMnO4 + 6H+→ 10CO2 + 2Mn2+ +8H2O 3. precipitation Ag+ + X- → AgX(s) 4. complex formation (EDTA) ethylenediaminetetraacetic acid

  5. Percent Purity Calculations Weigh accurately a portion of the impure sample and dissolve it in an arbitrary amount of solvent.

  6. Lab #2 %Purity Calculation A sample of impure KHP weighing 2.1283 g required 42.58 mL of a 0.1084 M NaOH solution for titration to the phenolphthalein end point. Calculate the %purity of the sample.

  7. Lab #3 Standardization Calculation A sample of primary standard Na2CO3 weighing 0.3542 g is dissolved in H2O and titrated with HCl. 30.23 mL of HCl is required to reach the end point. The reaction is - 2HCl + Na2CO3→ CO2 + H2O + 2NaCl Calculate the molarity of the HCl.

  8. Back-Titration = a known amount of excess standard reagent is added to the sample. Then a second standard reagent is used to titrate the excess of the first reagent. A 0.2178 g sample of impure Mg(OH)2 was dissolved in 50.00 mL of 0.1204 M HCl (1st standard reagent). Back-titration of the excess acid required 3.76 mL of 0.0948 M NaOH (2nd reagent). Calculate the %purity of the Mg(OH)2.

  9. Ch 7: Gravimetric and Combustion Analysis

  10. General Gravimetric Procedure aA(aq) + rR(aq)→ AaRr(s) precipitating reagent(in excess) analyte precipitate weight of A determined using stoichiometric ratio between A and AaRr

  11. moles AaRr moles A mass A stoichiometric ratio FM FM Stoichiometry Calculations mass AaRr

  12. EXAMPLE, p.145: A Simple Gravimetric Calculation A 10.00-mL solution containing Cl- was treated with excess AgNO3 to precipitate 0.4368-g of AgCl (FM = 143.321). What was the molarity of Cl- in the unknown?

  13. Selected Analyses and "Masking"

  14. Impurities such as Ag+, Mn2+, Zn2+, Cd2+, Hg2+, Fe2+, and Ga3+ are masked using -

  15. EXAMPLE, p. 156: When the Stoichiometry is Not 1:1 Solid residue weighing 8.4448-g from an aluminum refining process was dissolved in acid, treated with 8-hydroxyquinoline, and ignited to give Al2O3 weighing 0.8554-g. Find the weight precent of Al in the original mixture.

  16. Precipitates (Sec. 7-2) • large particle size ease of filtering • colloids 1-500 nm, charged (migrate in an electric field), don't settle out (suspended by Brownian motion), pass through filter paper • need to promote particle growth over nucleation • precipitation mechanisms are still poorly understood, but they do depend on - • solubility • temperature • reactant concentrations • rate of mixing

  17. Relative Supersaturation (RS) • Two competing mechanisms: nucleation vs. particle growth • supersaturated solutions result in nucleation (the formation of many small colloids) S 0 Q = supersaturated concentration S = equilibrium concentration 1 2S 2 3S

  18. Control of Particle Size = Minimize Supersaturation • elevate the temperature (increases S) • use dilute solutions (decreases Q) • slow mixing with lots of stirring (decreases Q)

  19. Precipitation in the Presence of Electrolyte (e.g. 0.10 M HNO3) • we want the particles to coagulate together to make bigger particles • since the colloids are charged however, they repel each other • the charge on the colloid depends on which lattice ions are in excess in solution, e.g. for AgCl the lattice ions are Ag+ and Cl- • if excess Ag+ in solution, then + colloids • if excess Cl- in solution, then - colloids • if unknown = Cl- and it's being precipitated out with Ag+, then initially the excess lattice ion is Cl- and the colloids are negatively charged. • after all of the Cl- is precipitated out, adding more Ag+ will change the colloid charge to +

  20. A AgCl colloid growing in a solution of excess Cl- will be nagatively charged - The added electrolyte HNO3 = H+ + NO3- adds to the region around the colloid which is called the "ionic atmosphere". The added electrolyte shrinks the ionic atmosphere and makes it easier for colloids to "stick" together.

  21. Stirring and heating adds kinetic energy to the colloids, while the added electrolyte shrinks the ionic atmosphere. Both effects reduce repulsion between particles and they can then coagulate together.

  22. Thermogravimetric Analysis The mass of the sample is measured as a function of temperature.

  23. For this gravimetric analysis, the precipitate must be heated to at least 800 oC in order to drive off all the water, volatilize the HNO3, and reduce the sample to CaO. = "heating to constant weight"

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