Answer Happy

You must show all of your work as well as report all answers with proper significant figures and units. 1. Calculate the weight percent (w/w) of an aqueous solution containing 2.6*10-³ moles sodium chloride and 2.50 grams of water. 2. What is the concentration of OH in a saturated solution created by dissolving Zn(OH)2 (Ksp 3.0*10-16) in 0.040 M ZnCl₂? 3. What is the theoretical yield of copper (II) hydroxide if 25.0 mL of 0.350 M sodium hydroxide reacts with 45.0 mL of 0.125 M copper (II) sulfate? 2 NaOH (aq) + CuSO4 (aq) → Cu(OH)2 (s) + Na2SO4 (aq)

4. Write a balanced molecular equation, complete ionic equation and net ionic equation for each of the following precipitation reaction. Include appropriate phase for all compounds and use the solubility rules from the Lecture Notes. a. lithium sulfate and calcium nitrate b. cadmium (II) acetate and potassium phosphate Exceptions: None None None None None AgX, Hg2X2, PbX2 CaSO4, SrSO4, BaSO4, PbSO4 Exceptions: Group 1A cations and ammonium Group 1A cations and ammonium Group 1A cations and ammonium Group 1A cations and ammonium. Slightly Soluble: Sr(OH)2, Ba(OH)2 and Ca(OH)2 Group 1A cations and ammonium. Sparingly soluble: MgS, CaS and Bas Usually Soluble: Group 1A salts (Li*, Na, K, Rb*, Cs*) (NH4) (NO3-) (CH3COO-) (CIO3) and (CIO4¯) (CI), (Br) and (1) (SO4²-) Usually Insoluble: (PO4) (CO3²-) (C₂04²) (OH-) (S²-)