These reactions involve the transfer of electrons between atoms, and they play a crucial role in many chemical processes.īalancing redox reactions can be a challenging task, requiring knowledge of complex chemical equations and oxidation numbers. In the sections that follow, we discuss three of the most important kinds of reactions that occur in aqueous solutions: precipitation reactions (also known as exchange reactions), acid–base reactions, and oxidation–reduction reactions.Redox reactions are an essential part of chemistry, occurring in everything from rusting metal to the process of photosynthesis. The easiest way to make that kind of prediction is to attempt to place the reaction into one of several familiar classifications, refinements of the five general kinds of reactions introduced in Chapter 3 "Chemical Reactions" (acid–base, exchange, condensation, cleavage, and oxidation–reduction reactions). The most important step in analyzing an unknown reaction is to write down all the species-whether molecules or dissociated ions-that are actually present in the solution (not forgetting the solvent itself) so that you can assess which species are most likely to react with one another. Instead, you must begin by identifying the various reactions that could occur and then assessing which is the most probable (or least improbable) outcome. Nothing could be further from the truth: an infinite number of chemical reactions is possible, and neither you nor anyone else could possibly memorize them all. Students tend to think that this means they are supposed to “just know” what will happen when two substances are mixed. As you advance in chemistry, however, you will need to predict the results of mixing solutions of compounds, anticipate what kind of reaction (if any) will occur, and predict the identities of the products. So far, we have always indicated whether a reaction will occur when solutions are mixed and, if so, what products will form. Net ionic equation: 3Ag +(aq) + PO 4 3−(aq) → Ag 3PO 4(s) Write the overall chemical equation, the complete ionic equation, and the net ionic equation for the reaction of aqueous silver fluoride with aqueous sodium phosphate to give solid silver phosphate and a solution of sodium fluoride. The six NO 3 −(aq) ions and the six Na +(aq) ions that appear on both sides of the equation are spectator ions that can be canceled to give the net ionic equation: 3Ba 2+(aq) + 2PO 4 3−(aq) → Ba 3(PO 4) 2(s) To obtain the complete ionic equation, we write each soluble reactant and product in dissociated form: 3Ba 2+(aq) + 6NO 3 −(aq) + 6Na +(aq) + 2PO 4 3−(aq) → Ba 3(PO 4) 2(s) + 6Na +(aq) + 6NO 3 −(aq) This is the overall balanced chemical equation for the reaction, showing the reactants and products in their undissociated form. Write all the soluble reactants and products in their dissociated form to give the complete ionic equation then cancel species that appear on both sides of the complete ionic equation to give the net ionic equation.įrom the information given, we can write the unbalanced chemical equation for the reaction: Ba(NO 3) 2(aq) + Na 3PO 4(aq) → Ba 3(PO 4) 2(s) + NaNO 3(aq)īecause the product is Ba 3(PO 4) 2, which contains three Ba 2+ ions and two PO 4 3− ions per formula unit, we can balance the equation by inspection: 3Ba(NO 3) 2(aq) + 2Na 3PO 4(aq) → Ba 3(PO 4) 2(s) + 6NaNO 3(aq) Write and balance the overall chemical equation. Write the overall chemical equation, the complete ionic equation, and the net ionic equation for the reaction of aqueous barium nitrate with aqueous sodium phosphate to give solid barium phosphate and a solution of sodium nitrate.Īsked for: overall, complete ionic, and net ionic equations
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