Balancing chemical equations acid-base reactions

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)... 

The balanced chemical equation for this reaction shows that 1 mol of nitric acid reacts with 1 mol of sodium hydroxide. If equal molar quantities of nitric acid and sodium hydroxide are used, the result is a neutral (pH 7) aqueous solution of sodium nitrate. In fact, when any strong acid reacts with any strong base in the mole ratio from the balanced chemical equation, a neutral aqueous solution of a salt is formed. Reactions between acids and bases of different strengths usually do not result in neutral solutions. 

Suppose that a solution of an acid reacts with a solution of a base. You can determine the concentration of one solution if you know the concentration of the other. (This assumes that the volumes of both are accurately measured.) Use the concentration and volume of one solution to determine the amount (in moles) of reactant that it contains. The balanced chemical equation for the reaction describes the mole ratio in which the compounds combine. In the following Sample Problems and Practice Problems, you will see how to do these calculations. 

A. Write a balanced chemical equation for the reaction of H2SO4 and Ba(OH)2, as well as the acid or base with the anhydride of the other, and of the two anhydrides themselves. 

IF5 undergoes autodissociation into IF4 -t IF5 . SbFs acts as an acid and KF acts as a base when dissolved in IF5. Write balanced chemical equations for these reactions. 

The enthalpy of neutralization of a strong acid with a strong base is —55.2 l /mol of water formed. If 100.0 ml of 1.00 M NaOH and 100.0 ml of 1.00 M HCI, both at 25.0°C, are mixed, assume that the heat capacity of the resulting solution is 4.18 J/g °C and that the density of that solution is 1.02 g/mL. (a) Write a balanced chemical equation for the reaction, (b) Determine the number of moles of water that will be formed, (c) Determine the quantity of heat that the reaction will release, (d) How much heat is absorbed by the resulting solution (e) Calculate the mass of the solution. 

You must first write the balanced chemical equation for the reaction between the acid and the base (see Example 14.2). 

Acetic acid, CH3COOH, is a weak acid and NaOH is a strong base. The reaction between CH3COOH and NaOH is an acid-base neutralization reaction. We start by writing a balanced chemical equation for the reaction. We must convert mL NaOH to g CH3COOH. The necessary conversions are as follows ... 

Write the balanced chemical equation for (a) the thermal decomposition of potassium chlorate without a catalyst (b) the reaction of bromine with water (c) the reaction between sodium chloride and concentrated sulfuric acid, (d) Identify each reaction as a Bronsted acid—base, Lewis acid—base, or redox reaction. 

You need some idea of the balanced chemical equation. In the case of an acid-base reaction, an acid reacts with a base. The acid supplies H and the base accepts the H+. If the acid is diprotic, such as H2SO4, it can donate two H. ... 

The pipeted volume is converted to moles by multiplying the liters of solution by its molarity. The moles of titrant are determined using the mole ratio in the balanced chemical equation for the acid—base reaction. The molarity of the solution is calculated by dividing the moles of titrant by the liters of titrant used. 

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. 

The characteristic features of parameter estimation in a molecular model of adsorption are illustrated in Table 9.9, taking the simple example of the constant-capacitance model as applied to the acid-base reactions on a hydroxylated mineral surface. (It is instructive to work out the correspondence between equation (9.2) and the two reactions in Table 9.9.) Given the assumption of an average surface hydroxyl, there are just two chemical reactions involved (the background electrolyte is not considered). The constraint equations prescribe mass and charge balance (in terms of mole fractions, x) and two complex stability constants. Parameter estimation then requires the determination of the two equilibrium constants and the capacitance density simultaneously from experimental data on the species mole fractions as functions of pH. 

Write balanced chemical equations for each of the following reactions that involve acids and bases. 

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. 

Neutralization reactions are important in maintaining the necessary balance of chemicals in your body, and they help keep a similar balance in our oceans and lakes. Neutralization reactions are used in industry to make a wide range of products, including pharmaceuticals, food additives, and fertilizers. Let s look at some of the different forms of Arrhenius acid-base reactions, how they can be visualized, and how to describe them with chemical equations. 

Two "driving forces" for reactions discussed in this section are the formation of water in an acid-base reaction and the formation of a gaseous product. Write balanced chemical equations showing two examples of... 

Analyze We are given fhe chemical formulas for an acid and a base and asked to wrife a balanced chemical equation and fhen a nef ionic equation for fheir neufralizafion reaction. 

Whenever you perform a titration calculation, be sure that you have taken into account the stoichiometry of the reaction between the acid and base (use the balanced chemical equation). In this case, two moles of NaOH are required to neutralize each mole of acid. Furthermore, when performing titration calculations, do not be tempted to apply the dilution equation to solve the problem. If you were to take such an approach here, you would arrive at an incorrect result since the dilution equation fails to take into account the stoichiometry of the reaction. 

This is an acid-base reaction. The other products of the reaction are Na2S04 and H2O. The reaction does not involve changes in oxidation states, and thus the equation can be balanced by inspection. The balanced chemical equation is given below ... 

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