1.) A solution of 0.156m NaOH is used to titrate 32.0mL of a solution of H2SO4.

Question

1.) A solution of 0.156m NaOH is used to titrate 32.0mL of a solution of H2SO4. If 23.8mL 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(aq)

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

2a.) What is the [H3O+] of stomach acid?

2b.) One chewable tablet of the antacid Maalox contains 600mg of CaCO3. Write the balanced equation for the neutralization stomach acid by tablets of Maalox

2c.)Calculate the milliliters of stomach acid neutralized by two tablets of Maalox.

2d.)The antacid milk of magnesia contains 400mg of Mg(OH)2 per teaspoon. Write the balanced equation for the neutralization stomach acid by milk of magnesia. Express your answer as a chemical equation. Identify all of the phases in your answer.

2e.) Calculate the number of milliliters of stomach acid that are neutralized by 1 tablespoon of milk of magnesia (1 tablespoon = 3 teaspoons).

3.)Calculate the volume, in milliliters, of a 0.214M NaOH solution that will completely neutralize each of the following:

3a.)3.72mL of a 1.28M HNO3 solution.

3b.) 8.60mL of a 0.815M H3PO4 solution.

Explanation / Answer

1.) A solution of 0.156m NaOH is used to titrate 32.0mL of a solution of H2SO4. If 23.8mL 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(aq)

mol of NaOH = MV = 0.156*23.8 = 3.7128 mmol of NaOH

ratio is 1:2

mmol of H2SO4 = 1/2*3.7128 = 1.8564 mmol of H2SO4

so

M = mmol/mL

M = 1.8564/32

M = 0.058012 mol per liter of H2SO4

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