Neutralization reactions writing chemical equations

The pH of a 0.2 M solution of CUSO4 is 4.0. Write chemical equations to explain why a solution of this salt is neither basic [from the reaction of S04 aq) with water] nor neutral, but acidic. 

Will a 0.05 M solution of FeCl3 be acidic, basic, or neutral Explain your answer by writing chemical equations to describe any reactions taking place. 

EXERCISE 4.7 Writing Chemical Equations for a Neutralization Reaction... 

PRACTICE EXAMPLE B The compound BeCl2 4 H2O cannot be dehydrated by heating and it dissolves in water to give an acidic solution. Conversely, CaClg 6 H2O can be dehydrated by heating and it dissolves in water to give a solution with neutral pH. Explain these observations and write chemical equations for the reactions that occur, if any, when the salts are heated and when they are dissolved in water. 

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 ... 

Self-Test J.2B Write the chemical equation for a neutralization reaction in which calcium phosphate is produced. 

Predict the outcome of neutralization reactions and write their chemical equations (Self-Test J.2). 

Step 3 Write the chemical equation for the neutralization reaction and use the reaction stoichiometry to find the amount of H. O ions (or OH ions if the analyte is a strong base) that remains in the analyte solution after all the added titrant reacts. Each mole of H30+ ions reacts with 1 mol OH ions therefore, subtract the number of moles of H30+ or OH ions that have reacted from the initial number of moles. 

Write the balanced chemical equation for the reaction of chlorine with water in (a) a neutral aqueous solution (b) a dilute basic solution (c) a concentrated basic solution. 

Writing the equation in the ionic form shows clearly which species are really reacting and which are not. In the example above, the Na+ and N03 appear on both sides of the equation. They do not react, but are simply there in order to maintain electrical neutrality of the solution. Ions like this, which are not actually involved in the chemical reaction, are spectator ions. 

Write the chemical equation for the neutralization reaction you observed. 

Write the balanced chemical equation for each neutralization reaction. 

Are solutions of the following salts acidic, basic, or neutral For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic. The relevant Ka and Kb values are found in Tables 7.2, 7.3, and 7.4. 

Write the chemical equation for the hydrolysis reaction that occurs when sodium hydrogen carbonate is dissolved in water. Is the resulting solution acidic, basic, or neutral ... 

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. 

Analyze We are given the chemical formulas for an add and a base and asked to write a balanced molecular equation, a complete ionic equation, and a net ionic equation for their neutralization reaction. 

The usefulness of the molarity concentration unit is readily apparent when dealing with reaction stoichiometry. For example, suppose that you want to know how many milliliters of 2.50 M sulfuric acid it t es to neutralize a solution containing 100.0 grams of sodium hydroxide. The first thing you must do is write the balanced chemical equation for the reaction ... 

Write a chemical equation to show the neutralization of nitric acid (HNOj) by strontium hydroxide (SrfOH) ). Identify the Bronsted Lowry add and base in each of the following reactions a. 

Strategy First, write and balance the chemical equation that corresponds to the neutralization reaction ... 

A hydrochloric acid solution will neutralize a sodium hydroxide solution. Look at the molecular views showing one beaker of HCl and four beakers of NaOH. Which NaOH beaker will just neutralize the HCl beaker Begin by writing a balanced chemical equation for the neutralization reaction. 

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 ... 

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