Aqueous reactions ionic equations

In Lesson 6-2,1 mentioned that displacement reactions are a bit misleading at times. Sometimes, a product that is shown on the product side of the equation does not really appear in the physical chemical reaction. The reason for this has to do with the solubility of ionic substances in water. If a particular product is soluble, it will stay dissolved in the aqueous solution. If a product is insoluble, it will appear as a solid precipitate in the test vessel. It is important to know which products stay dissolved in the water, so we can make proper identification of the precipitates that do form as the result of the chemical reactions. Ionic equations are more realistic representations of these reactions that take place in aqueous solution. Ionic equations show the individual ions that exist in solution. When we take an ionic displacement reaction and remove the information that is misleading, we produce a net ionic equation. 

Write a net ionic equation for the reaction between aqueous solutions of... 

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. 

The products of the reaction between bromide ions and permanganate ions, Mn04, in basic aqueous solution are solid manganese(IV) oxide, MnO>, and bromate ions. Balance the net ionic equation for the reaction. 

Which is the more powerful oxidizing agent under standard conditions, an acidified aqueous permanganate solution or an acidified aqueous dichromate solution Specify the cell for the spontaneous reaction of the two couples by writing a cell diagram that under standard conditions has a positive emf. Determine the standard emf of the cell and write the net ionic equation for the spontaneous cell reaction. 

Self-Test 12.9A Which metal, zinc or nickel, is the stronger reducing agent in aqueous solution under standard conditions Evaluate the standard emf of the appropriate cell, specify the cell with a cell diagram, and write the net ionic equation for the spontaneous reaction. 

Sodium hydroxide, NaOH, is a soft, waxy, white, corrosive solid that is sold commercially as lye. It is an important industrial chemical because it is an inexpensive starting material for the production of other sodium salts. The amount of electricity used to electrolyze brine to produce NaOH in the chloralkali process (Section 12.13) is second only to the amount used to extract aluminum from its ores. The process produces chlorine and hydrogen gases as well as aqueous socFinn hydroxide (Fig. 14.17). The net ionic equation for the reaction is... 

Develop students understanding of the triplet relationship when describing and explaining the displaeement reaction between zinc and aqueous coppeifll) sulphate. Deduce the ionic equation for the chemical reaction. 

The K+ andN03 ions remain unchanged in aqueous solution as spectator ions . All ions involved in the reaction must be represented in the ionic equation. 

The ionic equations for both the reactions involving aqueous lead(II) nitrate are A similar. B dilferent. 

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. 

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 ... 

C04-0107. A white precipitate forms when aqueous calcium nitrate is mixed with aqueous ammonium sulfate, (a) Identify the precipitate and write the net ionic equation for the reaction, (b) What are the spectator ions ... 

C04-0126. Identify the species present in the following aqueous solutions. In each case, write a net ionic equation that describes what reaction occurs upon mixing equimolar portions of the two solutions, (a) NH3 and HCl (b) CaCl2 and Na2 SO4 (c) KOH and HBr and (d) HNO2 (a weak acid) and KOH. 

HCl(aq) and ZnCl2(aq) both exist as ions in aqueous solutions. Which of these is the complete ionic equation for this chemical reaction ... 

This equation, therefore, represents the reaction between any aqueous solution containing barium ions and any aqueous solution containing sulphate ions. This ionic equation summarises the test for a sulphate ion in aqueous solution. 

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. 

Our goal in this chapter is to help you learn about reactions in aqueous solutions, including titrations. We will present a set of solubility rules you can use to predict whether or not precipitation will take place when two solutions are mixed. You may want to talk to your instructor and/or check your text for other solubility rules. These rules will be useful as you learn to write net ionic equations. If you are unsure about mass/mole relationships, you may want to review Chapter 3. And remember—Practice, Practice, Practice. 

This net ionic equation focuses only on the substances that are actually involved in the reaction. It indicates that an aqueous solution containing Pb2+ (any solution, not just Pb(N03)2(aq)) will react with any solution containing the sulfate ion to form insoluble lead(II) sulfate. If this equation form is used, the spectator ions involved will not be known, but in most cases this is not a particular problem since the focus is really the general reaction, and not the specific one. You will be expected to write the balanced net ionic equation for many of the reactions on the test. 

Aqueous solutions of 0.2 mol/L Na2C03 and 0.2 mol/L AgNOs are mixed. Write a net ionic equation that represents the overall reaction. 

Write a balanced net ionic equation for the reaction of zinc with aqueous iron(II) chloride. Include the physical states of the reactants and products. 

As you saw earlier, the reaction of zinc with aqueous copper(II) sulfate can be represented by the following net ionic equation. 

Write balanced half-reactions from the net ionic equation for the reaction between solid aluminum and aqueous iron(in) sulfate. The sulfate ions are spectator ions, and are not included. 

Write the net ionic equation and the half-reactions for the disproportionation of mercury(I) ions in aqueous solution to give liquid mercury and aqueous mercury(II) ions. Assume that mercury(I)... 

You know from Investigation 10-A that magnesium metal, Mg(s), displaces aluminum from an aqueous solution of one of its compounds, such as aluminum nitrate, Al(N03)3(aq). To obtain a balanced net ionic equation for this reaction, you can start by looking at tbe half-reactions. Magnesium atoms undergo oxidation to form magnesium ions, which have a 2+ charge. The oxidation half-reaction is as follows. 

Combination Reaction also called synthesis, reaction in which two or more substances combine to form a compound Combustion burning of a fuel to produce heat, oxidation of a fuel source Complete Ionic Equation equation used to express reactions in aqueous solutions where reactants and products are written as ions rather than molecules or compounds Complete Reaction a chemical reaction in which one of the reactants is completely consumed... 

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