Here, barium chloride (BaCl 2) is added to sodium chloride (NaCl). Sodium Chloride with Barium Chloride Play Movie(duration 7 seconds, size 404 K) Here, sodium chloride (NaCl) is added to barium chloride (BaCl 2). The result is no visible reaction.īarium Chloride with Sodium Chloride Play Movie(duration 8.9 seconds, size 540 K) Here, barium chloride (BaCl 2) is added to hydrochloric acid (HCl). Hydrochloric Acid with Barium Chloride Play Movie(duration 7 seconds, size 418 K) Here, hydrochloric acid (HCl) is added to barium chloride (BaCl 2). The result is a white precipitate.īarium Chloride with Hydrochloric Acid Play Movie(duration 11 seconds, size 651 K) Here, barium chloride (BaCl 2) is added to sulfuric acid (H 2SO 4). Sulfuric Acid with Barium Chloride Play Movie(duration 7 seconds, size 424 K) Here, sulfuric acid (H 2SO 4) is added to barium chloride (BaCl 2). The result is a white precipitate.īarium Chloride with Sulfuric Acid Play Movie(duration 8.2 seconds, size 470 K) Here, barium chloride (BaCl 2) is added to copper(II) sulfate (CuSO 4). The blue color is due to Cu 2+ (aq).Ĭopper(II) Sulfate with Barium Chloride Play Movie(duration 7 seconds, size 425 K) The result is a pale blue solution and white precipitate. Here, copper(II) sulfate (CuSO 4) is added to barium chloride (BaCl 2). The result is no visible reaction.īarium Chloride with Copper(II) Sulfate Play Movie(duration 10.9 seconds, size 622 K) Here, barium chloride (BaCl 2) is added to copper(II) nitrate (Cu(NO 3) 2). The result is no visible reaction.Ĭopper(II) Nitrate with Barium Chloride Play Movie(duration 7.5 seconds, size 411 K) Here, copper(II) nitrate (Cu(NO 3) 2) is added to barium chloride (BaCl 2). The result is no visible reaction.īarium Chloride with Copper(II) Nitrate Play Movie(duration 7.9 seconds, size 477 K) Here, barium chloride (BaCl 2) is added to cobalt(II) chloride (CoCl 2). The result is no visible reaction.Ĭobalt(II) Chloride with Barium Chloride Play Movie(duration 6.5 seconds, size 367 K) Here, cobalt(II) chloride (CoCl 2) is added to barium chloride (BaCl 2). So we might predict that a non-polar solvent that doesn't dissolve salts would be a bad solvent for a double replacement reaction.Aqueous Reactions: Barium Chloride Aqueous Reactions: Barium Chlorideīarium Chloride with Cobalt(II) Chloride Play Movie(duration 10 seconds, size 590 K) The more you know about how the reaction occurs, and the more you know about the properties of different solvents (like their polarity), the more educated of a guess you can make! For example, in double replacement reactions, we know that the solubility of the reactants is important because we need free ions around. In general, it's tricky to predict for any random reaction what medium it might need. Water is a really great solvent whenever you want to have ions around. Double replacement reactions always occur in water, with the reactants in the aqueous state. Luckily, there aren't that many strong acids and bases, and you can learn morem about this from this video: Īnything that is soluble in water and dissolved (separated into individual cations and anions) is in the aqueous state. It is helpful to have the strong acids and bases memorized, since they have special reactivity. The cation (or positively charged ion) of the salt comes from the base, and the anion (or negatively charged ion) comes from the acid. If you have tried this reaction at home, you probably remember a lot of fizzing because the neutralization reaction is accompanied by a gas-producing reaction, where the carbonic acid decomposes into carbon dioxide gas-bubbles!-and water.Ī salt is generally any ionic compound, though I have also seen it defined as an ionic compound that is formed when you react an acid and a base. A + B − + C + D − → A + D − + C + B − \greenD NaCH 3 COO start text, N, a, C, H, end text, start subscript, 3, end subscript, start text, C, O, O, end text.
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