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12 Dec 2019

Complete and balance each of the following formula unit or net ionic equations. Write NR if no reaction occurs. Include the states of all products (s,l,g,or aq)
a)Mg (s) + Al(NO3)3 (aq)
b)Ag (s) + FeCl3 (aq)
c)Ni (s) + 2Na+(aq)
d)Ba(OH)2 (aq) + H2SO4 (aq)
e)NH3 (aq)+ HClO4 (aq)
f)HCO3- (aq) + OH- (aq)
g)NH4Cl(aq) + Li3PO4 (aq)
h)Pb(NO3)2(aq) + MgSO4(aq)

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9. Based on the equations below, which metal is the most active? Pb(NO3)2 (aq) + Ni (s) â Ni(NOJ2 (aq) +pb (s) Pb(NO3)2 (aq) + Ag (s)--No reaction Cu(NO): (aq) + Ni (s) â Ni(NO3)2 (aq) + Cu (s) [a] Ni [b] Ag [c] Cu [d] Pb [e] N 10. The net ionic equation for the reaction between sulfuric acid and sodium hydroxide is [a] H+(aq) + HS04 (aq)-20H-(aq) 2 H20 (l) + S -(aq) [b] H+ (aq) + HSo; (aq) + 2 Na+(aq) + 2 OH-(aq) â 2 H20 () + 2 Na+(aq) + S [c] S04-(aq) 2 Na+(aq) â 2 Na+(aq) + Sof-(aq) [d] H+ (aq) + OH-(aq) â H2O (/) [e] 2 H + (aq) + S04-(aq)-2Na+(aq) + 2 0H-(aq) 2 H 20 () +2 Na+(aq) + S -(ag) -(aq) 11. In which reaction does the oxidation number of oxygen increase? [a] Ba(NO3)2 (aq) + K2SO4 (aq) â BaSO4(s) +2 KNO3 (aq) [b] HCl (aq)-NaOH (aq) â NaCl (aq) + H20 (!) [c] MgO (s) + H20 (l) â Mg(OH)2 (s) [d] 2 SO2 (g) + 02(g) 2 SO3 (g) [e] 2 H20 (1) â 2 H2(g) + 02(g) 12. Based on the activity series, which one of the reactions below will occur? Corrected typo [a] Zn (s) + Mn12 (aq) â Zn12 (aq) + Mn (s) [b] SnCl2 (aq) + Cu (s) â Sn (s) + CuCl2 (aq) [c] 2 AgNO3 (a)Pb (s)-2 Ag (s) + Pb(NO3)2 (aq) [d] 3 Hig (l) 2 Cr(N03)3 (aq) â 3 AgN03 (aq) + 2 Cr(s) [c] 3 FeBr2 (aq) + 2 Au (s) â 3 Fe (s) + 2 AuBr3 (aq) 13. Which of the following is an oxidation-reduction reaction? [a] Cu (s) + 2 AgNO3 (aq) â 2 Ag (s)-Cu(NOJ2 (aq) [b] HCl (aq)-NaOH (aq) â H20 (1)-NaCl (aq) [c] AgNO3 (aq) + HCl (aq) â AgCl (s) + HNO3 (aq) [d] Ba(C2H302)2 (aq)-Na,so, (aq) â BaS04 (s) t. 2 NaC2H,02 (aq) [e] H2C03 (aq) + Ca(NO3)2 (aq) â 2 HNO3 (aq)-CaCO3 (s) 14. A 0.355 M K-SO4 solution can be prepared by- [a] dissolving 46.7 g of K SO4 in water and diluting to a total volume of 250.0 mL [b] dissolving 46.7 g of K2SO, in water and diluting to 500.0 mL, then diluting 25.0 mL of this solution to a total volume of 500.0 mL [c] dilution of 1.00 mL of 0.355 M K,SO, to 1.00 L [d] diluting 46.7 mL of 1.90 M K SO, solution to 250.0 mL

Determine if the following reactions will form a precipitate when solutions of the reactants are mixed. If a
precipitate is formed when the reactants are mixed, write the balanced formula unit, the complete ionic and
the net ionic equations for the reactions. If a precipitate does not form when the reactants are mixed, write NR (no reaction) to the right of the arrow. Do not forget to include the physical states of the reactants and products; (aq), (s), (l), (g) in your three solution equations.

a. Fe(NO3)2 (aq) + K3PO4 (aq)
b. Ba(OH)2 (aq) + Pb(ClO3)2 (aq)
c. Al(ClO4)3 (aq) + Na2SO3 (aq)
d. CaCl2 (aq) + (NH4)2SO4 (aq)
e. LiCH3COO (aq) + MgCl2 (aq)

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