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Chapter 4: Problem 126

A \(10.00-\mathrm{mL}\) sample of sulfuric acid from an automobile battery requires \(35.08 \mathrm{~mL}\) of \(2.12 \mathrm{M}\) sodium hydroxide solution for complete neutralization. What is the molarity of the sulfuric acid? Sulfuric acid contains two acidic hydrogens.

Short Answer

Expert verified
The molarity of the sulfuric acid is approximately \(3.72 M\).

Step by step solution

01

Calculate the moles of sodium hydroxide.

Using the volume and concentration of sodium hydroxide, we can find the moles of sodium hydroxide: Moles of NaOH = Volume of NaOH × Concentration of NaOH Volume of NaOH = \(35.08 mL\) Concentration of NaOH = \(2.12 M\) Moles of NaOH = \(35.08 mL × 2.12 M\) Moles of NaOH = \(74.3696 mmol\)
02

Determine the moles of sulfuric acid.

Now that we have the moles of sodium hydroxide, we need to use the stoichiometry between sulfuric acid and sodium hydroxide to find the moles of sulfuric acid: Moles of H₂SO₄ = Moles of NaOH × Stoichiometry Stoichiometry (ratio) of H₂SO₄ to NaOH is \(\frac{1}{2}\), As 1 mole of H₂SO₄ requires 2 moles of NaOH for complete neutralization. Moles of H₂SO₄ = \(74.3696mmol × \frac{1}{2}\) Moles of H₂SO₄ = \(37.1848 mmol\)
03

Calculate the molarity of sulfuric acid.

Finally, we have the moles of sulfuric acid and its volume, and we can find its molarity: Molarity of H₂SO₄ = \(\frac{Moles \:of \: H₂SO₄}{Volume \: of \: H₂SO₄}\) Volume of H₂SO₄ = \(10.00 mL\) Molarity of H₂SO₄ = \(\frac{37.1848 mmol}{10.00 mL}\) = \(\frac{37.1848 mmol}{10.00 mL} × \frac{1 L}{1000 mL} × \frac{1 mol}{1000 mmol}\) Molarity of H₂SO₄ = \(3.71848 M\) The molarity of the sulfuric acid is approximately \(3.72 M\).

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Most popular questions from this chapter

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?

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. ammonium sulfate and barium nitrate b. lead(II) nitrate and sodium chloride c. sodium phosphate and potassium nitrate d. sodium bromide and rubidium chloride e. copper(II) chloride and sodium hydroxide

How would you prepare \(1.00 \mathrm{~L}\) of a \(0.50 M\) solution of each of the following? a. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from "concentrated" \((18 M)\) sulfuric acid b. \(\mathrm{HCl}\) from "concentrated" \((12 \mathrm{M})\) reagent c. \(\mathrm{NiCl}_{2}\) from the salt \(\mathrm{NiCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) d. HNO \(_{3}\) from "concentrated" (16 M) reagent e. Sodium carbonate from the pure solid

Write the balanced formula equation for the acid-base reactions that occur when the following are mixed. a. potassium hydroxide (aqueous) and nitric acid b. barium hydroxide (aqueous) and hydrochloric acid c. perchloric acid \(\left[\mathrm{HClO}_{4}(a q)\right]\) and solid iron(III) hydroxide d. solid silver hydroxide and hydrobromic acid e. aqueous strontium hydroxide and hydroiodic acid

If \(10 . \mathrm{g}\) of \(\mathrm{AgNO}_{3}\) is available, what volume of \(0.25 \mathrm{M} \mathrm{AgNO}_{3}\) solution can be prepared?
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