Fall 08. Exam1

Fall 08. Exam1 - CHEMISTRY 2101 EXAM # 1 -- KOLPIN OCTOBER...

Info iconThis preview shows pages 1–6. Sign up to view the full content.

View Full Document Right Arrow Icon
Background image of page 1

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 2
Background image of page 3

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 4
Background image of page 5

Info iconThis preview has intentionally blurred sections. Sign up to view the full version.

View Full DocumentRight Arrow Icon
Background image of page 6
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: CHEMISTRY 2101 EXAM # 1 -- KOLPIN OCTOBER 8, 2008 NAME: NOTE WELL! You Must Show Your Work And A Logical Path To The Solution Of Each Problem To Receive Any Full Or Partial Credit. NO Credit Will Be Given For Numerical Answers Alone. 1) 24 points 2) 15 points 3) 20 points 4) 21 points 5) 20 points TOTAL 100 points l) 24 points Given the equilibrium reaction: A H 2B + C and Keq = 1.0 X 10 '9 Calculate the equilibrium concentrations of A, B, and C in a solution prepared by combining 2.00 Liters of 0.25 Molar A, 2.00 Liters of 0.30 Molar B, and 1.00 Liters of 0.20 Molar C. Be sure to define “x” when setting up your equilibrium expressions. 2 2) 15 points Homework Problem Set #1; problem — supplemental #2: A sample is known to contain only MgC03, CaC03, and BaCO3. When a 2.000 gm. Sample is heated to convert the carbonates to oxides, 0.910 gm. C02 is given off. When the heated sample containing the remaining oxides is cooled and weighed, it is found to weigh 1.089 gm. Other analyses show the original sample to be 6.94 weight % barium, 18.00 weight % calcium, and 12.95 weight % magnesium. Calculate the weight % values for MgC03, CaCO3 and BaC03 in the original sample. 3) 20 points a) 10 points Calculate the volume of 1.00 Molar NaOH that must be added to 0.50 mole of H3PO4 to prepare a buffer solution with pH = 7.00 a b) 10 points A buffer solution is prepared by adding 0.30 mole of formic acid and 0.5 0 mole of sodium formate to water and diluting to a final volume of 1.00 liter. Calculate the pH of the solution and the change in pH that occurs when 1.00 liter of 0.100 molar NaOH is added to this solution. 4 4) 21 points — 7 points each Calculate the pH of each of the following three solutions: a) Calculate the pH of 1.00 X 10 '2 Molar Cyanide (CN') b) Calculate the pH of 1.00 X 10 '3 Molar HCl c) Calculate the pH of 1.00 X 10'3 Molar Chloroacetic Acid 5) 20 points — 10 points for each part a) Homework #4 — supplemental problem 2a: Calculate how many mL of 0.050 molar NaOH must be added to 100 mL of 0.200 molar HCl to give a solution having a pH of 1.20. b) Calculate the change in pH that occurs when 50 mL of 0.200 molar NaOH is added to 1.00 liter of an aqueous HCl solution having a pH of 2.40 ...
View Full Document

Page1 / 6

Fall 08. Exam1 - CHEMISTRY 2101 EXAM # 1 -- KOLPIN OCTOBER...

This preview shows document pages 1 - 6. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online