1. The molality of a certain solution was determined to be 0.0382 mol solute kg solvent The solute weighs 0.4135 g and the solvent weighs 24.3 g. a). Determine the moles of solute. b) Divide the mass of the solute by its number of moles to calculate the molar mass (g/mol) of the solute.

2. Five milliliters (5.00 mL) of 0.002 M Fe3+ is mixed with 3.00 mL of 0.001 M of SCN and then 2.00 mL of aqueous solution is added. Assuming that the volumes are additive, calculate the final concentration (in M) of Fe3+ in the mixture. Fe3+ and SCN react to form FeSCN2+ in a 1:1 mole ratio. a) Determine initial Fe3+ moles b) Determine initial SCN moles c) After the reaction, how many moles of Fe3+ is remaining? d) What is the total volume in L of the solution? e) Calculate the final concentration of Fe3+

3. A monoprotic acid has a mass of 0.15 g. To reach the equivalence point (mol acid = mol KOH), 7.80 mL of 0.1003 M of KOH is required. a). How many moles of the base (KOH) were added to reach the equivalence point? b) Determine the molar mass (g/mol) of the acid. 4. Magnesium hydroxide dissociates partially according to the following equation Mg(OH)2 = Mg2+ + 2 HO- If the concentration of hydroxide (HO-) is determined experimentally to be 0.0523 M, then, a). What is the mole ratio of the two ions in the product? b) What is the concentration of Mg2+ (in M)?

5. Two moles of thiosulfate reacts with one mole of triiodide according to the equation (Note: triiodide is a reactant while iodide is a product in the reaction described below) 2 S2032- + 13 731- + S4062- + One millimeter (1.00 mL) of 0.02 M thiosulfate is consumed in 41 sec. a) Calculate the moles of thiosulfate. b) Calculate the moles of triiodide that will react in (a). c) Determine the rate of triiodide consumption in mol/sec.