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Precipitation Reactions (Double Replacement Reactions)

(s). Precipitation Reactions (Double Replacement Reactions). 4.16 Write balanced net ionic equations for the reactions that occur in each of the following cases. Cr 2 (CO 3 ) 3 + (NH 4 ) 2 SO 4. 3. (a) Cr 2 (SO 4 ) 3 ( aq ) + (NH 4 ) 2 CO 3 ( aq ) . 3. Chromium(III)

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Precipitation Reactions (Double Replacement Reactions)

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  1. (s) Precipitation Reactions (Double Replacement Reactions) 4.16 Write balanced net ionic equations for the reactions that occur in each of the following cases. Cr2(CO3)3 + (NH4)2SO4 3 (a) Cr2(SO4)3(aq) + (NH4)2CO3(aq)  3 Chromium(III) carbonate Ammonium sulfate Chromium(III) sulfate Ammonium carbonate Step 1: Write correct formulas for products Step 2: Balance complete reaction Step 3: Use solubility rules to determine which product is the precipitate. • All nitrates are soluble. • All Group 1 and ammonium compounds are soluble. Step 4: Write and balance the net ionic equation (NIE). 2 Cr3+ + CO32 3 Cr2(CO3)3(s)

  2. (s) (b) AgNO3 (aq) + K2SO4(aq)  2 Ag2SO4 + 2 KNO3 Silver nitrate Potassium sulfate Silver sulfate Potassium nitrate NIE: 2 Ag+ + SO42 Ag2SO4(s) Spectator ions: the ions that are not involved in forming a precipitate or a molecular species Ex: Na2S (aq) + 2 HCl (aq) H2S (g) + 2 NaCl (aq) Complete ionic equation: 2 Na+ + S2 + 2 H+ + 2Cl H2S (g) + 2 Na+ + 2 Cl Cancel out the spectators and you get the NIE: S2 + 2 H+ H2S (g)

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