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Chapter 15: Problem 87

What is meant by acid-base neutralization? Write a net ionic equation to go along with your answer.

Short Answer

Expert verified
Acid-base neutralization is a chemical reaction between an acid and a base, resulting in the formation of water and a salt. It can be understood as a reaction in which a proton (H+) from an acid combines with a hydroxide ion (OH-) from a base to form water (H2O). The remaining cation and anion from the initial reactants form a salt. For example, the net ionic equation for the neutralization between hydrochloric acid (HCl) and sodium hydroxide (NaOH) is: \( H^{+}(aq) + OH^{-}(aq) \rightarrow H_{2}O(l) \)

Step by step solution

01

Define Acid-Base Neutralization

Acid-base neutralization is a chemical reaction that occurs between an acid and a base, resulting in the formation of water and a salt. This process can be understood as a reaction in which a proton (H+) from an acid combines with a hydroxide ion (OH-) from a base to form water (H2O). The remaining cation and anion from the initial reactants form a salt.
02

Choose an Acid and a Base for the Example

Let's consider a simple example of an acid-base neutralization reaction. We'll use hydrochloric acid (HCl - a strong acid) and sodium hydroxide (NaOH - a strong base) for this demonstration.
03

Write the Balanced Chemical Equation

Write the balanced chemical equation for the reaction between hydrochloric acid and sodium hydroxide: HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l) This balanced equation shows that one molecule of hydrochloric acid reacts with one molecule of sodium hydroxide to produce one molecule of sodium chloride (the salt) and one molecule of water.
04

Write the Total Ionic Equation

The total ionic equation shows all of the ions present in the reaction. To write the total ionic equation, break the reactants and products into their respective ions: H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) → Na+(aq) + Cl-(aq) + H2O(l)
05

Write the Net Ionic Equation

The net ionic equation is derived from the total ionic equation by cancelling out the spectator ions, which are the ions that do not participate in the reaction (Na+ and Cl-, in this case). The net ionic equation for the acid-base neutralization between hydrochloric acid and sodium hydroxide is: H+(aq) + OH-(aq) → H2O(l) This equation illustrates the key process in an acid-base neutralization: the combination of a proton (H+) from an acid and a hydroxide ion (OH-) from a base to form water.

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Most popular questions from this chapter

\(\mathrm{HZ}\) is a weak acid. An aqueous solution of \(\mathrm{HZ}\) is prepared by dissolving \(0.020\) mol of \(\mathrm{HZ}\) in sufficient water to yield \(1.0 \mathrm{~L}\) of solution. The \(\mathrm{pH}\) of the solution was \(4.93\) at \(25.0{ }^{\circ} \mathrm{C}\). What is the \(K_{\mathrm{a}}\) of \(\mathrm{HZ}\) ?

Why aren't ionic compounds like \(\mathrm{NaOH}\) and \(\mathrm{Mg}(\mathrm{OH})_{2}\) weak bases?

A solution has an \(\mathrm{OH}\) concentration of \(10^{-11} \mathrm{M}\). (a) Is this solution basic or acidic? Explain how you know. (b) Without using a calculator, explain how you could quickly determine the \(\mathrm{H}_{3} \mathrm{O}\) concentration of this solution. What is that concentration?

An aqueous solution has an \(\mathrm{H}_{3} \mathrm{O}\) ' concentration of \(1.0 \mathrm{M}\). What is the OH concentration? Is this solution acidic or basic? Justify your answer.

(a) List all the weak bases phosphoric acid, \(\mathrm{H}_{3} \mathrm{PO}_{4}\), can produce via successive losses of its protons. (b) Of the bases you listed, which has no ability to serve as a weak acid? (c) Phosphorous acid, \(\mathrm{H}_{3} \mathrm{PO}_{3}\), is a diprotic acid, even though there are three \(\mathrm{H}\) atoms in the formula. Draw a Lewis dot diagram for phosphorous acid. (Hint: Only H bound directly to \(\mathrm{O}\) is acidic).
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