If 32.8 mL of a 0.162 M NaOH solution is required to titrate 25.0 mL of a solution of H 2 SO 4 , what is the molarity of the H 2 SO 4 solution? H 2 SO 4 (aq) + 2 KOH(aq) → 2 H 2 O(l) + K 2 SO 4 (aq)

Hello. In this problem, we are told shown below is a balanced neutralization reaction between barium hydroxide and nitric acid neutralization of 10 mL of nitric acid solution required 13.2 mL of a 0.150 molar barium hydroxide solution. We asked to solve for the molar of the nitric acid solution. The neutralization reaction we're given tells us that one mole of barium hydroxide reacts to two moles of nitric acid to form one mole of barium nitrate and two moles of water. We will begin with our volume and concentration of barium hydroxide and we will end with the volume of nitric acid. Since we are trying to find the molar of nitric acid, the volume should appear towards the end. We'll begin with our 13.2 mL of barium hydroxide. We will convert our volume from millis to liters. So we multiply it by one liter and divide by 1000 mL. Our units of milliliters, barium hydroxide cancels and we're left with liters will then make use of the concentration of barium hydroxide. We multiply by 0.150 moles of barium hydroxide and divide by one liter. Our Librium hydroxide solution cancels. Now that we're at moles of barium hydroxide, we go to our balanced reaction equation which tells us that one mole barium hydroxide reacts with two moles of nitric acid. So we multiply by two moles of nitric acid and divide by one mole of barium hydroxide. Our moles of barium hydroxide in the numerator and denominator cancel. And we're left with moles of nitric acid. We're trying to find its molar. So we already have moles. So we need to have volume in the denominator. So we'll divide by the 10 millis of nitric acid. We will convert our volume from milliliters to liters. We'll multiply by 1000 mL of nitric acid divide by one liter. The nitric acid arm millis of nitric acid in the denominator and numerator cancel were left with then moles per liter. So our concentration of nitric acid then is 0.396. Well, nitric acid, thanks for watching. Hope this helped.

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10. Acids and Bases

Strong Acid Strong Base Titrations (Simplified)

GOB Chemistry

10. Acids and Bases

Strong Acid Strong Base Titrations (Simplified)

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2:34 minutes

Problem 53

Textbook Question

If 32.8 mL of a 0.162 M NaOH solution is required to titrate 25.0 mL of a solution of H₂SO₄, what is the molarity of the H₂SO₄ solution?
H₂SO₄(aq) + 2 KOH(aq) → 2 H₂O(l) + K₂SO₄(aq)

Verified step by step guidance

Step 1: Write the balanced chemical equation for the reaction. The given equation is already balanced: H₂SO₄(aq) + 2NaOH(aq) → 2H₂O(l) + Na₂SO₄(aq). This shows that 1 mole of H₂SO₄ reacts with 2 moles of NaOH.

Step 2: Calculate the moles of NaOH used in the titration. Use the formula: moles = molarity × volume. Convert the volume of NaOH from mL to L by dividing by 1000, then multiply by the molarity (0.162 M).

Step 3: Use the stoichiometry of the reaction to determine the moles of H₂SO₄. From the balanced equation, 1 mole of H₂SO₄ reacts with 2 moles of NaOH. Divide the moles of NaOH by 2 to find the moles of H₂SO₄.

Step 4: Calculate the molarity of the H₂SO₄ solution. Use the formula: molarity = moles / volume. The volume of the H₂SO₄ solution is given as 25.0 mL, so convert it to liters by dividing by 1000, then divide the moles of H₂SO₄ by this volume.

Step 5: Double-check your units and calculations to ensure consistency and accuracy. The final molarity of the H₂SO₄ solution will be in units of moles per liter (M).

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Titration

Titration is a quantitative analytical technique used to determine the concentration of a solute in a solution. It involves the gradual addition of a titrant (a solution of known concentration) to a sample solution until the reaction reaches its endpoint, which is often indicated by a color change. In this case, NaOH is the titrant used to determine the molarity of H₂SO₄.

Stoichiometry

Stoichiometry is the calculation of reactants and products in chemical reactions based on the balanced chemical equation. It allows us to determine the relationships between the amounts of substances involved in the reaction. For the titration of H₂SO₄ with NaOH, the stoichiometric coefficients indicate that one mole of H₂SO₄ reacts with two moles of NaOH, which is crucial for calculating the molarity of the sulfuric acid solution.

Molarity

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (M). In this problem, the molarity of the H₂SO₄ solution can be calculated using the volume and molarity of the NaOH solution, along with the stoichiometric relationship from the balanced equation, to find the concentration of the sulfuric acid.

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Textbook Question

One of the most acidic lakes in the United States is Little Echo Pond in the Adirondacks in New York. Recently, this lake had a pH of 4.2, well below the recommended pH of 6.5.

c. One way to raise the pH (and restore aquatic life) is to add limestone (CaCO₃). How many grams of CaCO₃ are needed to neutralize 1.0 kL of the acidic water from Little Echo Pond if the acid is sulfuric acid?

H₂SO₄(aq) + CaCO₃(s) → CO₂(g) + H₂O(l) + CaSO₄(aq)

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Textbook Question

The daily output of stomach acid (gastric juice) is 1000 mL to 2000 mL. Prior to a meal, stomach acid (HCl) typically has a pH of 1.42.

c. The antacid milk of magnesia contains 400. mg of Mg(OH)₂ per teaspoon. Write the neutralization equation, and calculate the number of milliliters of stomach acid neutralized by 1 tablespoon of milk of magnesia (1tablespoon = 3teaspoons).

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Multiple Choice

How many grams of HNO₃ are required to completely neutralize 110.0 mL of 0.770 M LiOH?

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Multiple Choice

What is the molar mass of a 0.350 g sample of a HA acid if it requires 50.0 mL of 0.440 M Sr(OH)₂ to completely neutralize it? A is used as a place holder for the unknown nonmetal of the acid.

How many grams of Al(OH)₃ are required to neutralize 150. mL of stomach acid with a pH of 1.5?

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Textbook Question

A 0.205 M NaOH solution is used to titrate 20.0 mL of a solution of H₂SO₄. If 45.6 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H₂SO₄ solution?

H₂SO₄(aq) + 2NaOH(aq) → 2H₂O(l) + Na₂SO₄

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Textbook Question

Calculate the volume, in milliliters, of a 0.150 M NaOH solution that will completely neutralize each of the following:

a. 25.0 mL of a 0.288 M HCl solution

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Textbook Question

Determine each of the following for a 0.100 M HBr solution:

d. milliliters of the HBr solution required to neutralize 36.0 mL of a 0.250 M LiOH solution

873