Question

Identify the spectator ions present (if any) when aqueous solutions of AgNO3 and MgCl, are mixed. Periodic Table TABLE 8.1 Solubility Rules for Ionic Compounds in Water Compounds Containing the Following Ions Are Generally Soluble Exceptions Lit, Nat, Kt, and NHA None NO, and C2H30 None CI, Br, and When these ions pair with Agt, Hg2+, or Pb2+, the resulting compounds are insoluble. SO2- When SO 2 pairs with Sr?+, Ba²+, Pb2+, Ag+, or Ca't, the resulting compound is insoluble. Compounds Containing the Following Ions Are Generally Insoluble Exceptions OH and S2 When these ions pair with Li*, Na, K, or NH4, the resulting compounds are soluble. When 52 pairs with Ca²+, Sr2+, or Ba2+, the resulting compound is soluble. When OH pairs with Ca2+, Sr2t, or Ba2+, the resulting compound is slightly soluble. CO2- and PO 3- When these ions pair with Lit, Nat, Kt, or NHA", the resulting compounds are soluble. Ag+ (aq), Noz (aq), Mg2+ (aq), CT (aq) ONOz (aq), Mg2+ (aq) O Ag+ (aq), C1 (aq) Othere are no spectator ions present

Answer 1

The total equation of reaction will be-

$\large 2AgNO_{3}(aq)+MgCl_{2}(aq)\rightarrow 2AgCl(s)+Mg(NO_{3})_{2}0(aq)$

The complete ionic equation will be-

$\large 2Ag^{+}(aq)+2NO_{3}^{-}(aq)+Mg^{2+}(aq)+2Cl^{-}(aq)\rightarrow 2AgCl(s)+Mg^{2+}(aq)2NO_{3}^{-}(aq)$

So, net equation becomes-

$\large 2Ag^{+}(aq)+2Cl^{-}(aq)\rightarrow 2AgCl(s)$

So, there is no role of Mg2+ and NO3- is net equation.

So, spectator ions are- Mg2+(aq) and NO3- (aq). [OPTION B}