Precipitation ionic equations

A precipitation reaction occurs when two or more soluble species combine to form an insoluble product that we call a precipitate. The most common precipitation reaction is a metathesis reaction, in which two soluble ionic compounds exchange parts. When a solution of lead nitrate is added to a solution of potassium chloride, for example, a precipitate of lead chloride forms. We usually write the balanced reaction as a net ionic equation, in which only the precipitate and those ions involved in the reaction are included. Thus, the precipitation of PbCl2 is written as... 

Write a net ionic equation for any precipitation reaction that occurs when solutions of the following ionic compounds are mixed. 

Although we have introduced net ionic equations to represent precipitation reactions, they have a much wider application. Indeed, we will use them for all kinds of reactions in water solution. In particular all of the chemical equations written throughout this chapter are net ionic equations. 

Decide whether a precipitate will form when the following solutions are mixed. If a precipitate forms, write a net ionic equation for the reaction,... 

As we saw in Chapter 4, a precipitate forms when a cation from one solution combines with an anion from another solution to form an insoluble ionic solid. We also considered how to predict whether such a reaction would occur and, if so, how to represent it by a net ionic equation. 

Write balanced net ionic equations to explain why a precipitate dissolves in... 

A solution of potassium dichromate is made basic with sodium hydroxide the color changes from red to yellow. Addition of silver nitrate to the yellow solution gives a precipitate. This precipitate dissolves in concentrated ammonia but re-forms when nitric acid is added. Write balanced net ionic equations for all the reactions in this sequence. 

A complete ionic equation for a precipitation reaction shows all the dissolved ions explicitly. For example, the complete ionic equation for the silver chloride precipitation reaction shown in Fig. 1.5 is... 

The net ionic equation shows that Ag+ ions combine with Cl ions to precipitate as solid silver chloride, AgCl (see Fig. 1.5). A net ionic equation focuses our attention on the change that results from the chemical reaction. 

Self-Test I.2A Write the net ionic equation for the reaction in Fig. 1.1, in which aqueous solutions of colorless silver nitrate and yellow potassium chromate react to give a precipitate of red silver chromate. 

Self-Test I.2B The mercury(I) ion, Hg22+, consists of two Hg+ ions joined together. Write the net ionic equation for the reaction in which colorless aqueous solutions of mercury(I) nitrate, Hg2(N03)2, and potassium phosphate, K3P04, react to give a white precipitate of mercurv(I) phosphate. 

Predict the precipitate if any, likely to be formed when aqueous solutions of sodium phosphate, and lead(II) nitrate are mixed. Write the net ionic equation for the reaction. 

Self-Test I.3A Predict the identity of the precipitate that forms, if any, when aqueous solutions of ammonium sulfide and copper(II) sulfate are mixed, and write the net ionic equation for the reaction. 

How would you use the solubility rules in Table 1.1 to separate the following pairs of ions In each case indicate what reagent you would add and write the net ionic equation for the precipitation reaction (a) lead(II) and copper(II) ions ... 

When the solution in Beaker 1 is mixed with the solution in Beaker 2, a precipitate forms. Using the following table, write the net ionic equation describing the formation of the precipitate, and then identify the spectator ions. 

Each of the following five procedures results in the formation of a precipitate. For each reaction, write the chemical equations describing the formation of the precipitate the overall equation, the complete ionic equation, and the net ionic equation. Identify the spectator ions. 

We saw in Section I that the net chemical change in a precipitation reaction is clarified by writing its net ionic equation. The same is true of neutralization reactions. First, we write the complete ionic equation for the neutralization reaction between nitric acid and barium hydroxide in water ... 

K.20 Classify each of the following reactions as precipitation, acid-base neutralization, or redox. If a precipitation reaction, write a net ionic equation if a neutralization reaction, identify the acid and the base if a redox reaction, identify the oxidizing agent and the reducing agent. 

The next step is to write the chemical equation and derive the ionic equation which more adequately describes the precipitation process. Thus, students will be... 

A similar observation was made in the ionic precipitation of lead(ll) iodide. When aqueous solutions of potassium iodide and sodium iodide were separately added to aqueous leadfll) nitrate, 12% of students believed that the ionic equation for the precipitation reactions was different in the two instances even though the stoichiometry of the two chemical reactions had no influence on the ionic equation. 

The simplest balanced chemical equation for a precipitation reaction is a net ionic equation that has ions as the reactants and a neutral solid as the product. In a precipitation reaction, reactant ions combine to form a neutral ionic solid. One reactant carries positive charge and the other carries negative charge, but the product is electrically neutral. Because electrical charge always is conserved, the total positive charge of the reacting cations... 

Another example of a precipitation reaction is the process that occurs when we mix aqueous solutions of potassium hydroxide (KOH) and iron(III) chloride (FeCl3). A precipitate forms. A list of species present helps us to determine the net ionic equation describing this process ... 

Species present K, Fe, Cl, OH, H2 O other experments show that KCl is a soluble salt, so the only possible precipitate contains Fe cations and OH" anions. We describe this precipitation by a balanced net ionic equation that contains only those species involved in the reaction. The substance that forms contains three OH anions combined with every Fe cation, resulting in a neutral product. Thus, the reactant species are Fe " " cations and OH anions with stoichiometric coefficients of 1 and 3. Here is the net ionic equation ... 

A net ionic equation contains only those species that participate in a chemical reaction. Notice that neither K nor Cr appears in the equation for the precipitation of Fe (OH). Similarly, neither K nor NO3 appears in the equation for the precipitation of Pbl2. Although these other ions are present in the solution, they undergo no change during the precipitation reaction. Ions that are not involved in the chemical change are referred to as spectator ions. Spectator ions are omitted from net ionic equations. 

The solution that results from mixing contains all the ions of the original solutions. If any cation-anion combination results in an insoluble salt, that salt will precipitate from solution. List the ions and then apply the flowchart to find out whether any new combination of cations and anions gives an insoluble salt. If there is an insoluble salt, write the net ionic equation for its formation. 

We need a balanced net ionic equation. The precipitate, AgBr, forms from two ions, Ag and... 

A white precipitate forms when 2.00 X 10 mL of 0.200 M potassium phosphate solution is mixed with 3.00 X 10 mL of 0.250 M calcium chloride solution. Write the net ionic equation that describes this process. Calculate the mass of the precipitate that forms, and identify the ions remaining in solution. 

Predict what will happen when the following pairs of substances are allowed to react. Write a balanced chemical equation for each reaction. When the reaction involves ions, write a net ionic equation. Identify each reaction as precipitation, as acid-base, or as redox, (a) AgN03(a q) and NaCl(a q) (b)... 

C04-0086. Write the baianced net ionic equation for each of these precipitation reactions. Also, identify the spectator ions. 

Identify the precipitate, write the net ionic equation for the solubility equilibrium, and identify the spectator species. 

These ionic equations summarise the following types of reaction (a) the precipitation reaction between aqueous silver and aqueous chloride ions (b) the redox reaction between zinc metal and dilute acid (c) the neutralisation reaction between an acid and an alkali. 

These problems involve mixing two solutions. Each solution is a water solution of an ionic compound. From the mixture of the two solutions, at least one insoluble precipitate will form. The other ions present are probably soluble and are called spectator ions they are not included in the net ionic equation. You must know your solubility rules to do these problems. 

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