10. Acids and Bases

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) + 2KOH(aq) → 2H₂O(l) + K₂SO₄(aq)

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

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

Calculate the volume, in milliliters, of a 0.150 M NaOH solution that will completely neutralize each of the following: (10.7)a. 25.0 mL of a 0.288 M HCl solution

Determine each of the following for a 0.100 M HBr solution: (10.5, 10.6, 10.7)d. milliliters of the HBr solution required to neutralize 36.0 mL of a 0.250 M LiOH solution

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. (10.6, 10.7) 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) + CaCO₄(aq)

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. (10.6, 10.7)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).