CHEM 105 10/1/19 Solution Stoichiometry and Redox ____________________________________________________________________________ Learning Objectives: By the end of the session students should be able to: ● Combine their stoichiometry skills with their knowledge of solutions to solve solution stoichiometry problems ● Identify the oxidation state of an element within a compound ● Determine if a reaction is a redox reaction, along with which compound is reduced/oxidized ____________________________________________________________________________ Review: Complete and balance the following equations. Then write the net ionic equation: a. BaBr2(aq)+ H2SO4(aq) → b. CaCl2(aq) + Na3PO4(aq) → c. KNO3(aq) + LiC2H3O2(aq) → d. KOH (aq) + HCl (aq) → Notes: 1.)What is the theoretical yield of the precipitate upon mixing 25.0 mL of 0.150 M Na2CO3 with 15.0 mL of 0.175 M Al(NO3)3? 2.)25.0 g of K2C2O4 is reacted with KMnO4 according to the following unbalanced chemical equation. K2C2O4 (aq) + KMnO4 (aq) + H2O(l) → CO2 (g) + Mn(OH)2 (s) + KOH (aq) a. How many grams of KMnO4 are required for this reaction? b. How many grams of Mn(OH)2 will be produced? c. If the reaction is done in 2.5 L of solution, what will the concentration of OH
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- Fall '08