18. Aqueous Equilibrium

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?

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

How many milliliters of 0.0850 M NaOH are required to titrate each of the following solutions to the equivalence point: (c) 50.0 mL of a solution that contains 1.85 g of HCl per liter?

A 20.0-mL sample of 0.200 M HBr solution is titrated with 0.200 M NaOH solution. Calculate the pH of the solution after the following volumes of base have been added: (e) 35.0 mL.

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

A 20.0-mL sample of 0.150 M KOH is titrated with 0.125 M HClO4 solution. Calculate the pH after the following volumes of acid have been added: (c) 24.0 mL.

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

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

Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (a) hydrobromic acid (HBr).

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

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

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

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

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)

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

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?

Two 25.0-mL samples, one 0.100 M HCl and the other 0.100 M HF, are titrated with 0.200 M KOH. c. Which titration curve has the lower initial pH?

Two 25.0-mL samples, one 0.100 M HCl and the other 0.100 M HF, are titrated with 0.200 M KOH. b. Is the pH at the equivalence point for each titration acidic, basic, or neutral?

Two 20.0-mL samples, one 0.200 M KOH and the other 0.200 M CH3NH2, are titrated with 0.100 M HI. b. Is the pH at the equivalence point for each titration acidic, basic, or neutral?

Two 20.0-mL samples, one 0.200 M KOH and the other 0.200 M CH3NH2, are titrated with 0.100 M HI. c. Which titration curve has the lower initial pH?

Two 20.0-mL samples, one 0.200 M KOH and the other 0.200 M CH3NH2, are titrated with 0.100 M HI. a. What is the volume of added acid at the equivalence point for each titration?

Two 20.0-mL samples, one 0.200 M KOH and the other 0.200 M CH3NH2, are titrated with 0.100 M HI. d. Sketch each titration curve.

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. e. the pH after adding 5.0 mL of base beyond the equivalence point

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. c. the pH at 10.0 mL of added base

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. d. the pH at the equivalence point

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. b. the volume of added base required to reach the equivalence point

Consider the titration of a 35.0-mL sample of 0.175 M HBr with 0.200 M KOH. Determine each quantity. a. the initial pH

A 20.0-mL sample of 0.125 M HNO3 is titrated with 0.150 M NaOH. Calculate the pH for at least five different points throughout the titration curve and sketch the curve. Indicate the volume at the equivalence point on your graph.

Consider the titration of a 25.0-mL sample of 0.115 M RbOH with 0.100 M HCl. Determine each quantity. c. the pH at 5.0 mL of added acid

Consider the titration of a 25.0-mL sample of 0.115 M RbOH with 0.100 M HCl. Determine each quantity. b. the volume of added acid required to reach the equivalence point

Consider the titration of 60.0 mL of 0.150 M HNO3 with 0.450 M NaOH. (a) How many millimoles of HNO3 are present at the start of the titration? (b) How many milliliters of NaOH are required to reach the equivalence point? (c) What is the pH at the equivalence point? (d) Sketch the general shape of the pH titration curve.

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

(a) What volume of 0.115 M HClO4 solution is needed to neutralize 50.00 mL of 0.0875 M NaOH?

Make a rough plot of pH versus milliliters of acid added for the titration of 50.0 mL of 1.0 M NaOH with 1.0 M HCl. Indicate the pH at the following points, and tell how many milliliters of acid are required to reach the equivalence point. (a) At the start of the titration (b) At the equivalence point (c) After the addition of a large excess of acid

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

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

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

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

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

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

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.)

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

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

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?

A 25.00-mL sample of an unknown HClO4 solution requires titration with 22.62 mL of 0.2000 M NaOH to reach the equivalence point. What is the concentration of the unknown HClO4 solution? The neutralization reaction is HClO4(aq) + NaOH(aq)¡H2O(l ) + NaClO4(aq)

What is the pH at the equivalence point for the titration of 0.20 M solutions of the following acids and bases? Which of the indicators in Figure 17.5 would be suitable for each titration? (c) Ba(OH)2 and HBr

A solution is made by adding 0.300 g Ca1OH221s2, 50.0 mL of 1.40 M HNO3, and enough water to make a final volume of 75.0 mL. Assuming that all of the solid dissolves, what is the pH of the final solution?

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.

A solid sample of Fe1OH23 is added to 0.500 L of 0.250 M aqueous H2SO4. The solution that remains is still acidic. It is then titrated with 0.500 M NaOH solution, and it takes 12.5 mL of the NaOH solution to reach the equivalence point. What mass of Fe1OH23 was added to the H2SO4 solution?

If the following solutions are mixed, is the resulting solution acidic, basic, or neutral? (a) 50.0 mL of 0.100 M HBr and 30.0 mL of 0.200 M KOH

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?

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?

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?

Determine the pH of each two-component solution. d. 0.088 M HClO4 and 0.022 M KOH

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: (b) 75.0 mL