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Chapter 4: Problem 93

A \(3.664-\mathrm{g}\) sample of a monoprotic acid was dissolved in water and required \(20.27 \mathrm{~mL}\) of a \(0.1578 \mathrm{M}\) \(\mathrm{NaOH}\) solution for neutralization. Calculate the molar mass of the acid.

Short Answer

Expert verified
The molar mass of the acid is approximately 1145 g/mol.

Step by step solution

01

Calculate moles of $\mathrm{NaOH}$ using concentration and volume

Firstly, calculate the moles (n) of the $\mathrm{NaOH}$ used in the reaction by using the equation n = c × V, where c is the concentration and V is the volume. In this case, c = \(0.1578 \mathrm{M}\) and V = \(20.27 \mathrm{~mL} = 20.27 \times 10^{-3} \mathrm{L}\). Therefore n = \(0.1578 \times 20.27 \times 10^{-3} = 3.200 \times 10^{-3}\) moles.
02

Determine moles of the acid

Since each acid molecule reacts with one $\mathrm{NaOH}$ molecule, the moles of the acid are also \(3.20 \times 10^{-3}\) moles.
03

Calculation of the Molar mass of the acid

Finally, calculate the molar mass (MM) of the acid by using the equation MM = m / n, where m is the mass and n is the moles. In this case m = 3.664 g and n = 3.20 x 10^{-3} mol, hence MM = 3.664 / \(3.20 \times 10^{-3} = 1145 \mathrm{g/mol}\).

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Most popular questions from this chapter

What factors qualify a compound as a salt? Specify which of the following compounds are salts: \(\mathrm{CH}_{4}\) \(\mathrm{NaF}, \mathrm{NaOH}, \mathrm{CaO}, \mathrm{BaSO}_{4}, \mathrm{HNO}_{3}, \mathrm{NH}_{3}, \mathrm{KBr} ?\)

Nitric acid is a strong oxidizing agent. State which of the following species is least likely to be produced when nitric acid reacts with a strong reducing agent such as zinc metal, and explain why: \(\mathrm{N}_{2} \mathrm{O},\) \(\mathrm{NO}, \mathrm{NO}_{2}, \mathrm{~N}_{2} \mathrm{O}_{4}, \mathrm{~N}_{2} \mathrm{O}_{5}, \mathrm{NH}_{4}^{+}\)

(a) Without referring to Figure 4.10 , give the oxidation numbers of the alkali and alkaline earth metals in their compounds. (b) Give the highest oxidation numbers that the Groups \(3 \mathrm{~A}-7 \mathrm{~A}\) elements can have.

Describe how to prepare \(1.00 \mathrm{~L}\) of \(0.646 \mathrm{M} \mathrm{HCl}\) solution, starting with a \(2.00 \mathrm{M} \mathrm{HCl}\) solution.

What is the advantage of writing net ionic equations?
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