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Chapter 4: Problem 96

Acetylsalicylic acid is the active ingredient in aspirin. It took \(35.17 \mathrm{~mL}\) of \(0.5065 \mathrm{M}\) sodium hydroxide to react completely with \(3.210 \mathrm{~g}\) of acetylsalicylic acid. Acetylsalicylic acid has one acidic hydrogen. What is the molar mass of acetylsalicylic acid?

Short Answer

Expert verified
The molar mass of acetylsalicylic acid is approximately \(180.34\mathrm{~g/mol}\).

Step by step solution

01

Find moles of sodium hydroxide

First, we need to find the moles of sodium hydroxide that were used in the reaction. To do this, we can use the formula: moles = volume × concentration The volume of sodium hydroxide used is \(35.17\mathrm{~mL}\) and its concentration is \(0.5065 \mathrm{M}\). Therefore, the moles of sodium hydroxide can be calculated as follows: moles = \(35.17\mathrm{~mL}\) × \(0.5065 \mathrm{M}\) moles = \(0.03517\mathrm{~L}\) × \(0.5065 \mathrm{M}\) = \(0.01780 \mathrm{mol}\)
02

Use stoichiometry to find moles of acetylsalicylic acid

Since acetylsalicylic acid has one acidic hydrogen, it reacts with sodium hydroxide in a 1:1 ratio. Therefore, the moles of acetylsalicylic acid reacted will be the same as the moles of sodium hydroxide used. moles of acetylsalicylic acid = moles of sodium hydroxide moles of acetylsalicylic acid = \(0.01780 \mathrm{mol}\)
03

Calculate the molar mass of acetylsalicylic acid

Now that we have the moles of acetylsalicylic acid reacted, we can calculate its molar mass using the formula: molar mass = mass / moles The mass of acetylsalicylic acid is given as \(3.210\mathrm{~g}\). Therefore, the molar mass of acetylsalicylic acid can be calculated as follows: molar mass = \(3.210\mathrm{~g}\) / \(0.01780\mathrm{~mol}\) = \(180.34\mathrm{~g/mol}\) So, the molar mass of acetylsalicylic acid is approximately \(180.34\mathrm{~g/mol}\).

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Most popular questions from this chapter

A \(100.0-\mathrm{mL}\) aliquot of \(0.200 M\) aqueous potassium hydroxide is mixed with \(100.0 \mathrm{~mL}\) of \(0.200 M\) aqueous magnesium nitrate. a. Write a balanced chemical equation for any reaction that occurs. b. What precipitate forms? c. What mass of precipitate is produced? d. Calculate the concentration of each ion remaining in solution after precipitation is complete.

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{UO}_{2}^{2+}\) f. \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}\) b. \(\mathrm{As}_{2} \mathrm{O}_{3} \quad\) g. \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) c. \(\mathrm{NaBiO}_{3}\) h. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) d. As i. \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) e. \(\mathrm{HAsO}_{2}\)

You are given a \(1.50-\mathrm{g}\) mixture of sodium nitrate and sodium chloride. You dissolve this mixture into \(100 \mathrm{~mL}\) of water and then add an excess of \(0.500 \mathrm{M}\) silver nitrate solution. You produce a white solid, which you then collect, dry, and measure. The white solid has a mass of \(0.641 \mathrm{~g}\). a. If you had an extremely magnified view of the solution (to the atomic- molecular level), list the species you would see (include charges, if any). b. Write the balanced net ionic equation for the reaction that produces the solid. Include phases and charges. c. Calculate the percent sodium chloride in the original unknown mixture.

Consider the reaction of \(19.0 \mathrm{~g}\) of zinc with excess silver nitrite to produce silver metal and zinc nitrite. The reaction is stopped before all the zinc metal has reacted and \(29.0 \mathrm{~g}\) of solid metal is present. Calculate the mass of each metal in the \(29.0-\mathrm{g}\) mixture.

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{KMnO}_{4}\) f. \(\mathrm{Fe}_{2} \mathrm{O}_{4}\) \(\begin{array}{ll}\text { b. } \mathrm{NiO}_{2} & \text { g. } \mathrm{XeOF}_{4}\end{array}\) c. \(\mathrm{Na}_{4} \mathrm{Fe}(\mathrm{OH})_{6}\) h. \(\mathrm{SF}_{4}\) d. \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4}\) i. \(\mathrm{CO}\) e. \(\mathrm{P}_{4} \mathrm{O}_{6}\) j. \(\mathrm{C}_{6} \mathrm{H}_{1}, \mathrm{O}_{e}\)
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