Solubility Rules

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Chemistry

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Dec 6, 2023

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Solubility Rules Goals: • Observe the formation of a precipitate and derive solubility rules • Write net ionic equations Background: Some salts (ionic compounds) are soluble in water, but many are not. For example, iron (III) chloride (FeCl 3 ) is soluble in water, but silver chloride (AgCl) is not. It is difficult to predict which compounds will be soluble in water, but some general rules can be derived from observations of experiments. By mixing together two ions and observing the resulting mixture, it can be determined if they have formed a precipitate. By trying several combinations, some general rules can be derived (for example, chlorides are soluble except silver chloride). In mixing together a solution of aqueous potassium chloride and aqueous silver nitrate, the following reaction occurs: KCl (aq) + AgNO 3 (aq) → KNO 3 (aq) + AgCl (s) The reactants are soluble in water and are in solution as ions. The products contain a solid (AgCl) and aqueous potassium nitrate (in solution as ions). K + (aq) + Cl - (aq) + Ag + (aq) + NO 3 - (aq) → K + (aq) + NO 3 - (aq) + AgCl (s) The K + and NO 3 - are called spectator ions - they are not involved in the formation of the solid. By removing these ions from both sides of the reaction, a net ionic reaction is obtained: Cl - (aq) + Ag + (aq) → AgCl (s) In this experiment you will observe the results when several cations (in solution as nitrate salts) and several anions (in solution as sodium salts) are mixed. The nitrate and sodium ions will not form precipitates and will not interfere with any of the tests.
Procedure: A1. Obtain an acetate sheet with a grid and place this on the bench top. A2. There will be one set of anions and one set of cations per table. Place one drop of each of the cations (Ag + , K + , etc) in each square of its row on the sheet. Drop the solutions onto the sheet carefully. If you make a mistake, blot up the liquid with a KimWipe tissue. A3. Place one drop of each of the anions (Cl - , OH - , etc) in each square of its column on the sheet (you are now mixing the anion with the cation which is already in the square). DO NOT touch the dropper to the sheet or it will become contaminated and all results will be incorrect. If you make a mistake, blot up the liquid with a KimWipe tissue. A4. Most of the drops will remain clear indicating that the salts are soluble and no reaction occurred. Some solutions will turn cloudy indicating the formation of a precipitate. There may or may not be a color change. The solids may be more apparent if observed against a dark background. Note on the report sheet any precipitate formation - place an X in those squares where a precipitate was seen. Write the formula of the precipitate. Leave the non-precipitate reactions blank. A5. For the precipitates which formed, write balanced net ionic reactions. A6. Develop a set of statements or rules about the solubilities of ions based on your observations (this should not just be a restatement of the rules learned in lecture). Write these rules on the report sheet. You should have about 4-6 rules. For example, “chlorides are soluble except AgCl” would be an acceptable rule. “Most chlorides are soluble” would not be acceptable - it is too vague. A7. The acetate sheet may be rinsed down the drain with lots of water when you are finished.
Data: Cl - Br - NO 3 - OH - CO 3 -2 SO 4 -2 PO 4 -3 Ag + X AgCl X AgBr X AgOH X Ag 2 CO 3 X Ag 3 PO 4 K + Cu +2 X CuOH 2 X CuCO 3 X Cu 3 PO 4 NH 4 + Ba +2 X BaOH 2 X BaCO 3 X BaSO 4 X Ba 3 PO 4 Na + Ni +2 X NiOH 2 X NiCO 3 X Ni 3 PO 4 Fe +3 X FeOH 3 X Fe 3 CO 3 X FePO 4 Solubility Rules: Match the Solubility Rule to the Exception to the Rule: Solubility Rule Exception to the Rule Rule #1: K + , NH 4 + , Na + , and NO 3 - remain soluble. Exception to this rule? ________B__ a. Precipitates will form when combined with Ag + Rule #2: Cl - and Br - tend to remain soluble. Exception to this rule? ______A____ b. There are no exceptions to this rule. Rule #3: SO 4 2- tends to remain soluble. Exception to this rule? ______D____ c. Only K + , NH 4 + , and Na + remain soluble with these ions. Rule #4: OH - , CO 3 2- , and PO 4 3- tend to produce precipitates. Exception to this rule? _____C____ d. Precipitates will form when combined with Ba 2+
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