1. 1965 to date Clad Coinage Composition: 75% copper, 25% nickel Weight: 2.27g Diameter: 17.9mm Edge: Reeded A.P. Chemistry. Gravimetric Analysis using PPT reaction information…a review and extension Numismatics is the scientific study of money and its history in all its varied forms. "All science is either Physics or stamp collecting." - Ernest Rutherford physicist and Noble Laureate.

2. Pre-1965 Composition: silver and copper… but how much of each typically??? This Roosevelt dime is different though.

3. A.P. Chem Gravimetric Analysis: PURPOSE: Procedure: 1. 2. 3. 4. 5. 6. 7. Calculations: Data To determine the silver composition of a pre-1965 dime Mass dime2.8357 g Dissolve the dime in HNO 3 Ag + NO 3 - + H + --> Ag + + NO + H 2 O Add HCl Ag + + Cl - --> AgCl Filter and dry Mass of Filter and Sample = 4.1860 g ( Filter paper = 0.7942 g) Mass AgClAgCl = 3.3918 g Find % comp. of AgCl % Ag = 75.265 % Find mass of AgAg = 2.5528 g 6.) 107.87 / 143.32 = 0.75265 7.) 3.3918 x 0.75265 = Answer: ( 2.5528 g / 2.8357 g ) x 100% = 90.024% A type of quantitative analysis in which the amount of one species in a material is determined by isolating and massing it

4. What volume of 6.0 M HCl would have been needed to completely precipitate out all of the silver ions from the solution if the concentration of the silver ion was 0.473 M and there was 50.0 mL of the solution?

5. 50.0 ml Ag + 0.473 mol = 1000.0 mL 0.0237 mol Ag + 0.0237 mol Ag + 1.0 mol HCl = 1.0 mol Ag + 0.0237 mol HCl 0.0237 mol HCl 1000.0 mL HCl = 4.0 mL HCl sol’n Ag + + Cl - --> AgCl Ag + + HCl (aq) --> AgCl + H + 6.0 mol HCl 50.0 ml Ag + 0.473 mol Ag + 1 mol HCl 1000.0 mL HCl 1 1000.0 mL Ag + 1 mol Ag + 6.0 mol HCl Ag + + H + + Cl - --> AgCl + H + =

6. What mass of Fe(OH) 3 is produced when 50.0 mL of 6.0 M LiOH sol’n reacts with an excess of 2.0 M Fe(NO 3 ) 3 sol’n? Fe(NO 3 ) 3(aq) + LiOH (aq) → Fe(OH) 3(s) + LiNO 3(aq) 33 50.0 ml LiOH 6.0 mol LiOH 1 mol Fe(OH) 3 106.8 g Fe(OH) 3 1 1000.0 mL LiOH 3 mol LiOH 1.0 mol Fe(OH) 3 = 11 g Fe(OH) 3

7. What volume of 6.0 M HCl would have been needed to completely precipitate out all of the silver ions from the solution if the concentration of the silver ion was 0.473 M and there was 50.0 mL of the solution? What mass of Fe(OH) 3 is produced when 50.0 mL of 6.0 M LiOH sol’n reacts with an excess of 2.0 M Fe(NO 3 ) 3 sol’n? What volume of 6.0 M HCl would have been needed to completely precipitate out all of the silver ions from the solution if the concentration of the silver ion was 0.473 M and there was 50.0 mL of the solution? What mass of Fe(OH) 3 is produced when 50.0 mL of 6.0 M LiOH sol’n reacts with an excess of 2.0 M Fe(NO 3 ) 3 sol’n?