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Chapter 4: Problem 145

Acetylsalicylic acid ( \(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\) ) is a monoprotic acid commonly known as "aspirin." A typical aspirin tablet, however, contains only a small amount of the acid. In an experiment to determine its composition, an aspirin tablet was crushed and dissolved in water. It took \(12.25 \mathrm{~mL}\) of \(0.1466 \mathrm{M} \mathrm{NaOH}\) to neutralize the solution. Calculate the number of grains of aspirin in the tablet. (One grain \(=0.0648\) g.)

Short Answer

Expert verified
Therefore, there are 5.0 grains of aspirin in the tablet.

Step by step solution

01

Calculate the number of moles of NaOH

The molarity of a solution is defined as the number of moles of solute per liter of solution. To find the number of moles of NaOH used, multiply the volume of the NaOH solution (in liters) by its molarity. \[ \text{moles of NaOH} = \text{Volume (in L)} \times \text{Molarity} = 12.25 \times 10^{-3} \, \text{L} \times 0.1466 \, \text{M} = 0.001795 \, \text{moles}\]
02

Determine the moles of acetylsalicylic acid

In a neutralization reaction, moles of acid equal moles of base since acetylsalicylic acid is monoprotic. So, the moles of acetylsalicylic acid is also 0.001795 moles.
03

Calculate the mass of acetylsalicylic acid

We can find the mass of the acetylsalicylic acid by multiplying the number of moles by the molar mass of acetylsalicylic acid. The molar mass of acetylsalicylic acid (C9H8O4) can be calculated as (9*12.01 + 8*1.008 + 4*16.00) g/mol = 180.157 g/mol. Therefore, the mass is \[ \text{Mass (in g)} = \text{moles} \times \text{Molar mass} = 0.001795 \, \text{moles} \times 180.157 \, \text{g/mol} = 0.323 \, \text{g}\]
04

Convert mass to grains

Finally, we can convert the mass in grams to grains using the conversion factor that one grain equals 0.0648 g. \[ \text{Mass (in grains)} = \frac{\text{Mass (in g)}}{\text{grain/g}} = \frac{0.323 \, \text{g}}{0.0648 \, \text{g/grain}} = 5.0 \, \text{grains}\]

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Most popular questions from this chapter

Describe the laboratory preparation for the following gases: (a) hydrogen, (b) oxygen, (c) carbon dioxide, (d) nitrogen. Indicate the physical states of the reactants and products in each case. [Hint: Nitrogen can be obtained by heating ammonium nitrite \(\left(\mathrm{NH}_{4} \mathrm{NO}_{2}\right)\).]

The \(\mathrm{SO}_{2}\) present in air is mainly responsible for the acid rain phenomenon. Its concentration can be determined by titrating against a standard permanganate solution as follows: \(5 \mathrm{SO}_{2}+2 \mathrm{MnO}_{4}^{-}+2 \mathrm{H}_{2} \mathrm{O} \longrightarrow\) \(5 \mathrm{SO}_{4}^{2-}+2 \mathrm{Mn}^{2+}+4 \mathrm{H}^{+}\) Calculate the number of grams of \(\mathrm{SO}_{2}\) in a sample of air if \(7.37 \mathrm{~mL}\) of \(0.00800 \mathrm{M} \mathrm{KMnO}_{4}\) solution are required for the titration.

On the basis of oxidation number considerations, one of the following oxides would not react with molecular oxygen: \(\mathrm{NO}, \mathrm{N}_{2} \mathrm{O}, \mathrm{SO}_{2}, \mathrm{SO}_{3}, \mathrm{P}_{4} \mathrm{O}_{6}\) Which one is it? Why?

Classify the following reactions according to the types discussed in the chapter. (a) \(\mathrm{Cl}_{2}+2 \mathrm{OH}^{-} \longrightarrow \mathrm{Cl}^{-}+\mathrm{ClO}^{-}+\mathrm{H}_{2} \mathrm{O}\) (b) \(\mathrm{Ca}^{2+}+\mathrm{CO}_{3}^{2-} \longrightarrow \mathrm{CaCO}_{3}\) (c) \(\mathrm{NH}_{3}+\mathrm{H}^{+} \longrightarrow \mathrm{NH}_{4}^{+}\) (d) \(2 \mathrm{CCl}_{4}+\mathrm{CrO}_{4}^{2-} \longrightarrow\) \(2 \mathrm{COCl}_{2}+\mathrm{CrO}_{2} \mathrm{Cl}_{2}+2 \mathrm{Cl}^{-}\) (e) \(\mathrm{Ca}+\mathrm{F}_{2} \longrightarrow \mathrm{CaF}_{2}\) (f) \(2 \mathrm{Li}+\mathrm{H}_{2} \longrightarrow 2 \mathrm{LiH}\) (g) \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{SO}_{4} \longrightarrow 2 \mathrm{NaNO}_{3}+\mathrm{BaSO}_{4}\) (h) \(\mathrm{CuO}+\mathrm{H}_{2} \longrightarrow \mathrm{Cu}+\mathrm{H}_{2} \mathrm{O}\) (i) \(\mathrm{Zn}+2 \mathrm{HCl} \longrightarrow \mathrm{ZnCl}_{2}+\mathrm{H}_{2}\) (j) \(2 \mathrm{FeCl}_{2}+\mathrm{Cl}_{2} \longrightarrow 2 \mathrm{FeCl}_{3}\) (k) \(\mathrm{LiOH}+\mathrm{HNO}_{3} \longrightarrow \mathrm{LiNO}_{3}+\mathrm{H}_{2} \mathrm{O}\)

Oxygen \(\left(\mathrm{O}_{2}\right)\) and carbon dioxide \(\left(\mathrm{CO}_{2}\right)\) are colorless and odorless gases. Suggest two chemical tests that would enable you to distinguish between these two gases.
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