1. (a) Write balanced molecular equations for the following potential precipitat

Question

1. (a) Write balanced molecular equations for the following potential precipitation reactions. Indicate the states of reactants and products [(aq) or (s)]. (b) In those cases where a precipitate forms, write the net ionic equation. If there is no reaction, state "No reaction." (i) CoCl2 (aq) + K2S (aq) (ii) NaCl (aq) + (NH4)2S (aq) (iii) (NH4)2SO4 (aq) + Ba(NO3)2 (aq) (iv) CuCl2 (aq) + K2S (aq)

2.         Each of the following salts can be prepared from an acid and a base. Write the balanced molecular equation and the net ionic equation for the preparation of each. Indicate states of the reactants and products [(aq), (s), (l)]. Review solubility rules if necessary to determine the solubility of the reactants.

(a) NaCH3CO2 (aq)                 (b) RbBr (aq)             (c) Co(NO3)2 (aq)

Explanation / Answer

i) K2S(aq) + CoCl2(aq)......> KCl(aq) + CoS(s)

net ionic eq. is S^-2(aq) + Co^+2(aq) .........> CoS(s)

ii) NaCl (aq) + (NH4)2S (aq)......> no reaction

iii) (NH4)2SO4(aq) + Ba(NO3)2(aq) .......>BaSO4(s) + 2 NH4NO3(g)

net ionic eq. is SO4^-2(aq) + Ba^+2 (aq) ..........> BaSO4(s)

iv)CuCl2(aq) + K2S(aq) .......> CuS(s) + 2KCl(aq)

net ionic eq. is Cu+2(aq) + S^-2(aq) ........> CuS(s)

2)

a) CH3COOH(aq) + NaOH(aq) ......>CH3COONa(aq) + H2O(l)

CH3COO- (aq) + Na+ (aq) ...............> CH3COONa(aq)

b) RbOH(aq) + HBr(aq) ...................> HBr (aq) + H2O(l)

Rb+ (aq) + Br- (aq).................> HBr(aq)

c) Co(OH)2 (S) + 2HNO3 (aq) ...........> Co(NO3)2 (aq) + 2H2O (l)

Co^+2(s) + 2NO3^-(aq) ...............> Co(NO3)2 (aq)

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