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Chapter 8: Problem 96

What is the number of molecules of \(\mathrm{NaOH}\) required to neutralize one molecule of: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (b) HI (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}\) (d) \(\mathrm{HNO}_{3}\) (e) \(\mathrm{CH}_{3} \mathrm{COOH}\)

Short Answer

Expert verified
The number of molecules of \(\mathrm{NaOH}\) required to neutralize one molecule of the given acids are as follows: (a) \(\mathrm{H}_{2} \mathrm{SO}_{4}\): 2 molecules (b) HI: 1 molecule (c) \(\mathrm{H}_{3} \mathrm{PO}_{4}\): 3 molecules (d) \(\mathrm{HNO}_{3}\): 1 molecule (e) \(\mathrm{CH}_{3} \mathrm{COOH}\): 1 molecule

Step by step solution

01

(a) Neutralization of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) with \(\mathrm{NaOH}\)

First, let's look at the neutralization reaction of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) with \(\mathrm{NaOH}\): \(\mathrm{H}_{2} \mathrm{SO}_{4} + 2 \, \mathrm{NaOH} \rightarrow \mathrm{Na}_{2} \mathrm{SO}_{4} + 2 \, \mathrm{H}_{2}\mathrm{O}\) In this reaction, 2 moles of \(\mathrm{NaOH}\) are needed to neutralize 1 mole of \(\mathrm{H}_{2} \mathrm{SO}_{4}\). Therefore, the number of molecules of \(\mathrm{NaOH}\) required to neutralize one molecule of \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is 2.
02

(b) Neutralization of HI with \(\mathrm{NaOH}\)

Now let's consider the neutralization reaction of HI with \(\mathrm{NaOH}\): \(\mathrm{HI} + \mathrm{NaOH} \rightarrow \mathrm{NaI} + \mathrm{H}_{2}\mathrm{O}\) In this reaction, 1 mole of \(\mathrm{NaOH}\) is needed to neutralize 1 mole of HI. Therefore, the number of molecules of \(\mathrm{NaOH}\) required to neutralize one molecule of HI is 1.
03

(c) Neutralization of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) with \(\mathrm{NaOH}\)

Now let's look at the neutralization reaction of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) with \(\mathrm{NaOH}\): \(\mathrm{H}_{3} \mathrm{PO}_{4} + 3 \, \mathrm{NaOH} \rightarrow \mathrm{Na}_{3} \mathrm{PO}_{4} + 3 \, \mathrm{H}_{2}\mathrm{O}\) In this reaction, 3 moles of \(\mathrm{NaOH}\) are needed to neutralize 1 mole of \(\mathrm{H}_{3} \mathrm{PO}_{4}\). Therefore, the number of molecules of \(\mathrm{NaOH}\) required to neutralize one molecule of \(\mathrm{H}_{3} \mathrm{PO}_{4}\) is 3.
04

(d) Neutralization of \(\mathrm{HNO}_{3}\) with \(\mathrm{NaOH}\)

Now let's consider the neutralization reaction of \(\mathrm{HNO}_{3}\) with \(\mathrm{NaOH}\): \(\mathrm{HNO}_{3} + \mathrm{NaOH} \rightarrow \mathrm{NaNO}_{3} + \mathrm{H}_{2}\mathrm{O}\) In this reaction, 1 mole of \(\mathrm{NaOH}\) is needed to neutralize 1 mole of \(\mathrm{HNO}_{3}\). Therefore, the number of molecules of \(\mathrm{NaOH}\) required to neutralize one molecule of \(\mathrm{HNO}_{3}\) is 1.
05

(e) Neutralization of \(\mathrm{CH}_{3} \mathrm{COOH}\) with \(\mathrm{NaOH}\)

Finally, let's look at the neutralization reaction of \(\mathrm{CH}_{3} \mathrm{COOH}\) with \(\mathrm{NaOH}\): \(\mathrm{CH}_{3} \mathrm{COOH} + \mathrm{NaOH} \rightarrow \mathrm{CH}_{3} \mathrm{COONa} + \mathrm{H}_{2}\mathrm{O}\) In this reaction, 1 mole of \(\mathrm{NaOH}\) is needed to neutralize 1 mole of \(\mathrm{CH}_{3} \mathrm{COOH}\). Therefore, the number of molecules of \(\mathrm{NaOH}\) required to neutralize one molecule of \(\mathrm{CH}_{3} \mathrm{COOH}\) is 1.

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Most popular questions from this chapter

"Hard" water is hard because it contains \(\mathrm{Ca}^{2+}(a q)\) and \(\mathrm{Mg}^{2+}(a q)\) ions. It can be softened by adding borax powder, which is sodium tetraborate, \(\mathrm{Na}_{2} \mathrm{~B}_{4} \mathrm{O}_{7} .\) Adding borax removes the \(\mathrm{Ca}^{2+}(a q)\) and \(\mathrm{Mg}^{2+}(a q)\) from solution. Write a net ionic equation for each of these two reactions. What ion replaces the \(\mathrm{Ca}^{2+}(a q)\) and \(\mathrm{Mg}^{2+}(a q)\) ions in the water?

Consider the covalent bond in \(\mathrm{H}_{2}\). Why must energy be added to break this bond (in other words, what is the added energy used for)?

Balance this chemical equation by inspection: \(\mathrm{Fe}_{2} \mathrm{O}_{3}+\mathrm{C} \rightarrow \mathrm{Fe}+\mathrm{CO}_{2}\)

Suppose you had oxalic acid, \(\mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\), and you wanted to make sodium oxalate, \(\mathrm{Na}_{2} \mathrm{C}_{2} \mathrm{O}_{4} .\) How might you do this?

When an aqueous solution of ammonium sulfate is added to an aqueous solution of calcium nitrate, a precipitate forms. (a) Write a net ionic equation for the precipitation. (b) Write the precipitation reaction in a way that emphasizes that a double- replacement reaction has taken place.
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