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Chapter 4: Problem 42

Analysis of an unknown acid shows that \(24.55 \mathrm{~mL}\) of \(0.128 \mathrm{M} \mathrm{NaOH}\) are required to react completely with \(0.566 \mathrm{~g}\) of the acid. The equation for. the reaction is $$ \mathrm{HB}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}+\mathrm{B}^{-}(a q) $$ What is the molar mass of the acid?

Short Answer

Expert verified
Based on the given information and solution steps, here is a short answer question for students: Question: A 0.566 g sample of an unknown acid, HB, was neutralized by 24.55 mL of 0.128 M NaOH solution. Calculate the molar mass of the unknown acid.

Step by step solution

01

Determine the moles of OH- in the NaOH solution.

We are given the volume and molarity of NaOH solution. We can calculate the moles of OH- in the solution by multiplying the volume by the molarity: Moles of OH- = Volume x Molarity We have the volume in mL, so we need to convert it to L first: \(24.55\ \mathrm{ mL} = 24.55 / 1000 = 0.02455\ \mathrm{ L}\) Now, we can find the moles of OH-: Moles of OH- = \((0.02455\ \mathrm{L})({0.128\ \mathrm{M\:NaOH}})\)
02

Determine the moles of HB.

Since the reaction equation shows that there is a 1:1 ratio between the moles of HB and the moles of OH-, the moles of HB are equal to the moles of OH-. Moles of HB = Moles of OH- from Step 1
03

Calculate the molar mass of the acid HB.

We can find the molar mass of the acid HB by dividing the mass of the acid (given in grams) by the moles of HB (calculated in Step 2): Molar mass of HB = \(\frac{Mass\ of\ HB}{Moles\ of\ HB}\) Substitute the known values into the equation and calculate the molar mass of HB: Molar mass of HB = \(\frac{0.566\ \mathrm{g}}{Moles\ of\ HB}\) Remember to calculate and substitute the moles of OH- from Step 1 and use it as the moles of HB in the formula.

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