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17. Acid and Base Equilibrium

pH of Strong Acids and Bases

17. Acid and Base Equilibrium

pH of Strong Acids and Bases

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Strong Acids and Bases

Strong Acids and Bases

pH of Strong Acids and Bases Example

pH of Strong Acids and Bases Example

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Multiple Choice

An aqueous solution of HBrO₄ has a pH of 4.34. Find the molar concentration of HBrO₄ solution.

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Multiple Choice

Calculate the pH of a 25 mL of 5.45 × 10⁻² M LiOH solution.

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Multiple Choice

HI is a strong acid (K_a = 3.2 × 10⁹). Calculate [H⁺], [OH⁻], pH and pOH of a 7.1 × 10⁻² M HI solution.

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Textbook Question

Calculate the pH of solutions prepared by:

(d) Mixing equal volumes of 0.20 M HCl and 0.50 M HNO3.

(Assume that volumes are additive.)

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Textbook Question

What mass of HI must be present in 0.250 L of solution to obtain a solution with each pH value?

b. pH = 1.75

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Textbook Question

Two 25.0-mL samples, one 0.100 M HCl and the other 0.100 M HF, are titrated with 0.200 M KOH.

d. Sketch each titration curve.

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Textbook Question

What is the pH and the principal source of H3O+ ions in 1.0 * 10-10 M HCl? (Hint: The pH of an acid solution can’t exceed 7.) What is the pH of 1.0 * 10-7 M HCl?

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Textbook Question

A 100.0 mL sample of a solution that is 0.100 M in HCl and 0.100 M in HCN is titrated with 0.100 M NaOH. Calculate the pH after the addition of the following volumes of NaOH:

(a) 0.0 mL

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Textbook Question

The probe of the pH meter shown here is sitting in a beaker that contains a clear liquid. You are told the liquid is pure water, a solution of HCl(aq), or a solution of KOH(aq). (b) If the liquid is one of the solutions, what is its molarity?

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Textbook Question

What is the pH of an aqueous solution of Ca1OH22 at 25.0 °C with a concentration of 6.3 * 10-5 M? (LO 16.7) (a) 4.20 (b) 10.10 (c) 11.36 (d) 9.80

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Textbook Question

Which of the following solutions is the most basic? (a) 0.6 M NaCl, (b) 0.150 M CsOH, (c) 0.100 M Sr1OH22.

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Textbook Question

Calculate the pH of each of the following strong acid solutions: (b) 1.52 g of HNO3 in 575 mL of solution

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Textbook Question

Calculate the pH of each of the following strong acid solutions: (b) 0.225 g of HClO3 in 2.00 L of solution

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Textbook Question

Calculate 3OH-4 and pH for each of the following strong base solutions: (c) 10.0 mL of 0.0105 M Ca1OH22 diluted to 500.0 mL

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Textbook Question

Calculate the concentration of an aqueous solution of Ca1OH22 that has a pH of 10.05.

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Textbook Question

For each strong acid solution, determine [H3O+], [OH-], and pH. c. a solution that is 0.052 M in HBr and 0.020 M in HNO3

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Textbook Question

For each strong acid solution, determine [H3O+], [OH-], and pH. a. 0.25 M HCl

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Textbook Question

For each strong acid solution, determine [H3O+], [OH-], and pH. b. 0.015 M HNO3

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Textbook Question

For each strong acid solution, determine [H3O+], [OH-], and pH. d. a solution that is 0.655% HNO3 by mass (assume a density of 1.01 g>mL for the solution)

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Textbook Question

What mass of HClO4 must be present in 0.500 L of solution to obtain a solution with each pH value? b. pH = 1.50

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Textbook Question

What is the pH of a solution in which 224 mL of HCl(g), measured at 27.2 °C and 1.02 atm, is dissolved in 1.5 L of aqueous solution?

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Textbook Question

Find the pH of each mixture of acids. a. 0.115 M in HBr and 0.125 M in HCHO2

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Textbook Question

For each strong base solution, determine [OH-], [H3O+], pH, and pOH. b. 1.5 * 10-3 M Ca(OH)2

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Textbook Question

For each strong base solution, determine [OH-], [H3O+], pH, and pOH. d. 5.0 * 10-4 M Ca(OH)2

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Textbook Question

For each strong base solution, determine [OH-], [H3O+], pH, and pOH. c. 1.9 * 10-4 M KOH

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Textbook Question

For each strong base solution, determine [OH-], [H3O+], pH, and pOH. b. 0.0112 M Ba(OH)2

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Textbook Question

For each strong base solution, determine [OH-], [H3O+], pH, and pOH. a. 8.77 * 10-3 M LiOH

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Textbook Question

Determine the pH of a solution that is 3.85% KOH by mass. Assume that the solution has density of 1.01 g>mL.

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Textbook Question

Calculate the pH of the following solutions: (c) 0.075 M NaOH

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Textbook Question

Calculate the pH of solutions prepared by: (d) Mixing 100.0 mL of 2.0 * 10-3 M HCl and 400.0 mL of 1.0 * 10-3 M HClO4. (Assume that volumes are additive.)

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Textbook Question

Calculate the pH of solutions prepared by: (a) Dissolving 4.8 g of lithium hydroxide in water to give 250 mL of solution.

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Textbook Question

Calculate the pH of solutions prepared by: (a) Dissolving 0.20 g of sodium oxide in water to give 100.0 mL of solution.

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Textbook Question

How many grams of CaO should be dissolved in sufficient water to make 1.00 L of a solution with a pH of 10.50?

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Textbook Question

Calculate the pH of a solution made by adding 2.50 g of lithium oxide 1Li2O2 to enough water to make 1.500 L of solution.

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Textbook Question

The volume of an adult's stomach ranges from about 50 mL when empty to 1 L when full. If the stomach volume is 400 mL and its contents have a pH of 2, how many moles of H+ does the stomach contain? Assuming that all the H+ comes from HCl, how many grams of sodium hydrogen carbonate will totally neutralize the stomach acid?

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Textbook Question

People often take milk of magnesia to reduce the discomfort associated with acid stomach or heartburn. The recommended dose is 1 teaspoon, which contains 4.00 * 102 mg of Mg(OH)2. What volume of an HCl solution with a pH of 1.3 can be neutralized by one dose of milk of magnesia? If the stomach contains 2.00 * 102 mL of pH 1.3 solution, is all the acid neutralized? If not, what fraction is neutralized?

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Textbook Question

Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO3). How much limestone (in kg) is required to completely neutralize a 4.3 billion liter lake with a pH of 5.5?

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What is the pH of an HCl solution if [H⁺] = 0.03?

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The flask shown here contains 10 mL of HCl and a few drops of phenolphthalein indicator

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