CHEM 1122 Lecture Notes - Lecture 14: Iron(Iii) Sulfate, Ionic Compound, Potassium Carbonate
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Lecture 14 notes: practice distinguishing molecular, complete ionic, and net ionic equations, solubility. 1. if the ionic compound is aqueous (aq), then think about the cation and anion that it is made of. Mg(no3)2 (aq) mg2+ (aq) + 2 no3. 2. think of the elements in cations and anions as a whole since now they belong to a family. 3. balance the number of cations and anions on either side of the reaction equation. (aq) will always have 1 n and 3 o. _2_ nabr (aq) + _1_ mg(no3)2 (aq) _2_ na2(no3)2 (aq) + _1_ mgbr2 (aq) Note: any solid product formed does not break apart into ions precipitate, only aqueous salts will break apart into ions. 1. potassium carbonate + zinc nitrate zn2+(aq) + co3: iron(iii) sulfate + copper(1) iodide 2ki + fe2(so4)3 i2 + 2feso4 + k2so4. Analyzing the experimental data: write out the balanced precipitation reactions, 2agno3 + na2so4 = ag2so4 + 2nano3, 2nal + caso4 = na2so4 + cal2.
