Question

0 Chapter 7 Nov Solid aluminum sulfate is produced by reacting aluminum nitrate and potassium sulfate. The other product is aqueous potessium nitrate. 1. a) Write the balanced chemical equation. Be careful with naming. [Don't just google chemical formulael Use this as valuable practice for your naming. You can always check afterwards.1 If 109 g of aluminum nitrate and 0.626 moles of potassium sulfate are placed in a beaker, how many grams of solid could be formed? b) c) lf 15.26 g solid aluminum sulfate are isolated in the laboratory, calculate the % yield. Concentrated 'smoking, hydrochloric acid solution is 37.0% HCl by mass and has a density of 1.19 g/mL. Calculate the moles of HCl used if 25.00 mL of concentrated HCI solution is used. 2. 3. Hydrochloric acid reacts with calcium carbonate as shown in the reaction below. cacods) + 2 HCI(aq) → CaCl2(aq) + H,O(l) + CO2(g) If 80.0 mL of 15% (mass per volume) hydrochloric acid is reacted with 1959 g calcium carbonate, calculate the moles of the excess reactant that remains after the reaction is complete? Be clear about which species you are calculating. a) This question is unrelated to part(a) but uses the same reaction. reaction is found to be 81.2%. If you require 12.5 kg of calcium chloride for a subsequent reaction, how many kilograms of calcium carbonate must be added to excess hydrochloric acid? The percent yield of the above b) 9

Answer 1