Acid-base reactions equations, writing

SAMPLE PROBLEM 4.4 Writing Ionic Equations for Acid-Base Reactions Problem Write balanced molecular, total ionic, and net ionic equations for each of the following acid-base reactions and identify the spectator ions ... 

When a hydrochloric acid solution is combined with a potassium hydroxide solution, an acid-base reaction occurs. Write a balanced molecular equation and a net ionic equation for this reaction. 78. A beaker of nitric acid is neutralized with calcium hydroxide. Write a balanced molecular equation and a net ionic equation for this reaction. 

Write an equation for the Brpnsted acid-base reaction that occurs when each of the following acids reacts with water. Show all unshared electron pairs and formal charges, and use curved arrows to track electron movement. 

In earlier sections of this chapter, we showed how to write and balance equations for precipitation reactions (Section 4.2) and acid-base reactions (Section 4.3). In this section we will concentrate on balancing redox equations, given the identity of reactants and products. To do that, it is convenient to introduce a new concept, oxidation number. 

With the aid of Tables 4.1 and 4.2, write net ionic equations for acid-base reactions. (Example 4.6 Problems 29-36) 27,33... 

Write a balanced net ionic equation for each of the following acid-base reactions in water. 

For which of the following pairs would this be the correct prototype equation for the acid-base reaction in solution If it is not correct, write the proper equation for the acid-base reaction between the pair. 

In each case we indicate whether the compound is more soluble in acid than in water. We write the net ionic equation for the reaction in which the solid dissolves in acid. Substances are more soluble in acid if either (1) an acid-base reaction occurs [as in (b-d)] or (2) a gas is produced, since escape of the gas from the reaction mixture causes the reaction to shift to the right. 

To write a net ionic equation for an acid-base reaction between two solutions, use the following three steps ... 

J.3 Complete and write the overall equation, the complete ionic equation, and the net ionic equation for the following acid-base reactions. If the substance is a weak acid or base, leave it in its molecular form in writing the equations. 

In considering an acid-base reaction, it is important to realize that the choice of which acid is to be called the conjugate acid is completely arbitrary. In Equation 3.4 we could just as well have decided to call HaO the conjugate base of the acid HaO+ and CH3COOH the conjugate acid of the base CH3COO . It would perhaps be better to emphasize the fundamental symmetry of the situation by writing Equation 3.5 ... 

One model of an acid-base reaction involves proton transfer from the acid to a solvent water molecule to give an H30+ ion. Write balanced chemical equations that show how aqueous solutions of acidic oxides such as S02 and SO3 can yield H30+ ions. Which of these two oxides gives a higher concentration of H30+ ions Explain. 

One of the most useful features of the Bronsted system is that is takes into account what happens after an acid-base reaction occurs. You all know HC1 is an acid, so let s write an equation for it behaving as an acid. That is, let s allow HC1 to give away its hydrogen ion. 

Write equations for the following acid-base reactions. Use the information in Table 1-5 to predict whether the equilibrium will favor the reactants or the products. 

Identify nucleophiles (Lewis bases) and electrophiles (Lewis acids), and write equations for Lewis acid-base reactions using curved arrows to show the flow of electrons. 

Applying the Nernst equation for such a process, which is a combined redox and acid-base reaction, we can write... 

In Chapter 7, we learned how to do nnmerical calculations for compounds, using their formulas as a basis. This chapter lays the foundation for doing similar calculations for chemical reactions, using the balanced equation as a basis. The chemical equation is introduced in Section 8.1, and methods for balancing equations are presented in Section 8.2. To write equations, we must often be able to predict the products of a reaction from a knowledge of the properties of the reactants. Section 8.3 shows how to classify chemical reactions into types to predict the products of thousands of reactions. An important type of reaction— the acid-base reaction— is discussed in Section 8.4. 

Ionic fluorides such as KP behave as bases in Brp3, whereas some covalent fluorides such as Sbp5 behave as acids. On the basis of the solvent system concept, write balanced chemical equations for these acid-base reactions of fluorides with Brp3. 

Write the balanced formula equation for the acid-base reaction. 

Write a balanced equation for the acid-base reaction that leads to the production of each of the following salts. Name the acid, base, and salt. 

The alkylammonium cation is called the conjugate acid of the amine. Write down the general equation for a Bronsted-Lowry acid/base reaction, labelling the acid and the base, and the related conjugate base and acid. 

On rare occasions the acid/base reaction is the sole purpose of the reaction. For example, what will be the product when the benzoate anion, C6H5C02, dissolved in an aqueous solution, is treated with hydrochloric acid Write an equation for this reaction. 

Limestone, CaC03, is a water-insoluble material, whereas Ca(HC03)2 is soluble. Caves are formed when rainwater containing dissolved CO2 passes over limestone for long periods of time. Write a chemical equation for the acid-base reaction. 

We first write the balanced equation for the acid-base reaction and then construct the reaction summary that shows the amounts (moles) of HCl and NaOH. We determine the amount of salt formed from the reaction summary. The final (total) volume is the sum of the volumes mixed. Then we calculate the molarity of the salt. 

Write the balanced equation for an acid-base reaction that would produce each of the following salts predict whether an aqueous solution of each salt is acidic, basic, or neutral, (a) NaNO, (b) KCN (c) Al2(S04)3 (d) Mg(CH3COO)2 (e) (NH4)2S04. 

Teachers report that students get a much better idea of the role of chemistry in society. Contexts are effective in engaging the students. Students are confronted with a lot of knowledge in a short time. They learn a lot. There are still problems however. Using the knowledge gained in other contexts needs to be established more firmly. There is a need for more practice with skills like calculations in stoichiometry, writing equations in precipitation reactions or acid-base reactions. 

What are the three types of acid-base reactions that always go to completion Give an example of each by writing an overall equation. 

Transition-state representations are shown for two acid-base reactions. For each one, write the equation for the reaction it represents in the direction for which the eqnihbrinm lies to the right. Label the acid, the base, the conjugate acid, and the conjngate base, and nse cnrved arrows to show the flow of electrons. 

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