![]() First, for PbSO4, we can see that compounds containing sulfate anions are generally water-soluble, unless the compound also contains lead(II) cations, which our product does contain. Let’s predict the solubility of our products by checking the water solubility rules. So our first product will be composed of lead(II) cations and sulfate anions, forming PbSO4, with our next product containing magnesium cations and nitrate anions to form Mg(NO3)2. These ions will recombine to form new compounds. ![]() Our first reactant Pb(NO3)2 contains lead(II) cations and nitrate anions, and MgSO4 contains magnesium cations and sulfate anions. We can predict the products by first identifying the cations and anions present in each reactant. In double-replacement reactions, cations and anions dissociate in water and recombine to form new compounds. Answer choices (A), (B), (C), and (E) are all examples of double-replacement reactions, while answer choice (D) is an example of an acid–base reaction. Let’s predict the products of each of our answer choices to determine which would form a precipitate. And sulfides or hydroxides also containing calcium, barium, or strontium cations would be soluble in water. Compounds containing alkali metal cations or ammonium cations are always soluble in water. Compounds that are insoluble in water contain carbonate anions, phosphate anions, sulfide anions, or hydroxide anions, with the following exceptions. Sulfates that contain silver, calcium, strontium, barium, mercury(I), or lead(II) ions would be insoluble in water. For compounds containing halides, if the compound also contains silver, mercury(I), or lead(II) ions, the compound would then be insoluble in water. Compounds that are generally water-soluble and would not form a precipitate contain alkaline metal cations, ammonium cations, nitrate anions, bicarbonate anions, chlorate anions, acetate anions, halide anions, or sulfate anions.Ĭompounds containing halides or sulfate ions have some exceptions to their solubility in water. We can use the water solubility rules to predict which product will be insoluble in water. A precipitate can be formed from a reaction with reactants that are often both aqueous or, in other words, dissolved in water that when mixed together react to form the insoluble compound that is the precipitate and most likely another aqueous compound. A precipitate is an insoluble product that separates from a solution. ![]() We must identify the reaction where one of the products is a precipitate. (B) Ca(OH)2 aqueous plus two HCl aqueous. For which of the following reactions is a precipitate likely to form? (A) Pb(NO3)2 aqueous plus MgSO4 aqueous.
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