Chemical equations aqueous ionic reactions

A molecular equation for an aqueous ionic reaction shows undissociated substances. A total Ionic equation shows all soluble Ionic compounds as separate, solvated ions. Spectator ions appear unchanged on both sides of the equation. By eliminating them, you see the actual chemical change in a net ionic equation. 

Manganese silicide has the empirical formula MnSi and melts at 1280 C. It is insoluble in water but does dissolve in aqueous HF. (a) What type of compound do you expect MnSi to be metallic, molecular, covalent-network, or ionic (b) Write a likely balanced chemical equation for the reaction of MnSi with concentrated aqueous HF. 

To describe an aqueous ionic reaction, chemists use a net ionic equation because it eliminates spectator ions (those not involved in the reaction) and shows the actual chemical change taking place. 

Earlier treatment of reactions in aqueous solution a number of our users and non-user reviewers told us that they wanted students to learn about this topic before stoichiometry. Chapter 9 addresses this request. We now have a two-chapter treatment of chemical reactivity with a qualitative emphasis, preceding the quantitative chapter on stoichiometry. Chapter 8 provides an introduction to chemical reactivity, with an emphasis on writing and balancing chemical equations and recognizing reaction types based on the nature of the equation. After students have become confident with the fundamentals, we then increase the level of sophistication of our presentation on chemical change by introducing solutions of ionic compounds and net ionic equations. 

EXAMPLE 3.24 Balancing Chemical Equations Containing Ionic Compounds with Polyatomic Ions Write a balanced equation for the reaction between aqueous strontium chloride and aqueous lithium phosphate to form solid strontium phosphate and aqueous Uthium chloride. SOLUTION ... 

Write the balanced chemical equation for the reaction between aqueous solutions of strontium nitrate and potassium sulfate, which forms the precipitate strontium sulfate. Then write the complete ionic and net ionic equations. 

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... 

Reactions of cations in aqueous solution with sodium hydroxide - Al3+, Fe2+, Fe3+, Cu2+, Ca2+, Zn2, Cr3+,. An excess of sodium hydroxide solution is added slowly to a small volume of the solution containing the cation. This is an exercise in observation, organisational and recording skills and in the ability to write chemical equations - word, molecular and ionic. 

When you mix two aqueous ionic compounds together, there are two possible outcomes. Either the compounds will remain in solution without reacting, or one aqueous ionic compound will chemically react with the other. How can you predict which outcome will occur Figure 9.4 shows what happens when an aqueous solution of lead(II) nitrate is added to an aqueous solution of potassium iodide. As you can see, a yellow solid—a precipitate—is forming. This is a double displacement reaction. Recall, from Chapter 4, that a double displacement reaction is a chemical reaction that involves the exchange of ions to form two new compounds. It has the general equation... 

Note that the chemical equation does not show some details of this reaction. Sodium hydroxide and copper(II) chloride are ionic compounds. Therefore, in aqueous solutions they exist as Na+, OH, Cu +, and Cl ions. When their solutions are combined, Cu + ions in one solution and OH ions in the other solution react to form the precipitate copper(II) hydroxide, Cu(OH)2(s). The Na+ and CO ions remain dissolved in the new solution. 

To show the details of reactions that involve ions in aqueous solutions, chemists use ionic equations. Ionic equations differ from chemical equations in that substances that are ions in solution are written as ions in the equation. Look again at the reaction between aqueous solutions of sodium hydroxide and copper(II) chloride. To write the ionic equation for this reaction, you must show the reactants NaOH(aq) and CuCl2(aq) and the product NaCl(aq) as ions. 

Write the chemical, complete ionic, and net ionic equations for the reaction between aqueous solutions of barium nitrate and sodium carbonate that forms the precipitate barium carbonate. 

Thinking Criticaily Explain why net ionic equations communicate more than chemical equations about reactions in aqueous solutions. 

A reaction occurs when hydrosulfuric acid (H2S) is mixed with an aqueous solution of iron(III) bromide. Solid iron(III) sulfide is produced. Write the chemical and net ionic equations for the reaction. 

Applying Concepts Write the chemical equations and net ionic eqnations for each of the following reactions that may occur in aqueous solutions. If a reaction does not occur, write NR in place of the products. Magnesium phosphate precipitates in an aqueous solution. 

In this chapter we examine some types of chemical reactions. Millions of reactions are known, so it is useful to group them into classes, or types, so that we can deal systematically with these massive amounts of information. We will describe how some compounds behave in aqueous solution, including how well their solutions conduct electricity and whether or not the compounds dissolve in water. We introduce several ways to represent chemical reactions in aqueous solution—formula unit equations, total ionic equations, and net ionic equations—and the advantages and disadvantages of these methods. 

You are given the word equation for the reaction that occurs between hydrochloric acid and aqueous lithium hydroxide to produce water and aqueous lithium chloride. You must determine the chemical formulas for and relative amounts of all reactants and products to write the balanced chemical equation. To write the complete ionic equation, you need to show the ionic states of the reactants and products. By crossing out the spectator ions from the complete ionic equation, you can write the net ionic equation. 

What is a salt How are salts formed by acid-base reactions Write chemical equations showing the formation of three different salts. What other product is formed when an aqueous acid reacts with an aqueous base Write the net ionic equation for the formation of this substance. 

---