Question 1

The solubility of slightly soluble salts containing basic anions is proportional to the pH of the solution.

Accepted Answer

The answer of The solubility of slightly soluble salts containing...

Question 2

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be ________.

Accepted Answer

The answer of Metal oxides and hydroxides that are relatively...

Question 3

A solution of NaF is added dropwise to a solution that is 0.0122 M in Ba²⁺. When the concentration of F^- exceeds ________ M, BaF₂ will precipitate. Neglect volume changes. For BaF, Ksp = 1.7 × 10^-⁶.

Accepted Answer

First, we can write the balanced chemical equation for the precipitation reaction:

BaS1U1P12+S1S1P0 + x NaFS1U1P12 -> BaFS1U1B12S1U1B0 + x NaS1S1P0

We can use the expression for the solubility product to find when BaF starts to precipitate:

Ksp = [BaFS1U1B12S1U1B0][NaS1S1P0]/[NaFS1U1P12]

Since we're adding NaF dropwise, we can assume that the concentration of NaF does not change significantly as we add more drops. Therefore, we can use the initial concentration of BaS1U1P12+S1S1P0 to find the initial concentration of NaFS1U1P12:

0.0122 M BaS1U1P12+S1S1P0 = x NaFS1U1P12
x = 0.0122 MNaFS1U1P12

Substituting into our expression for Ksp:

1.7 × 10S1U1P1-S1S1P0S1U1P16S1S1P0 = [BaFS1U1B12S1U1B0][NaS1S1P0]/(0.0122 MNaFS1U1P12)

Solving for [NaS1S1P0], we get:

[NaS1S1P0] = 1.2 × 10S1U1P1-2S1S1P0 M

Therefore, the concentration of FS1U1P1-S1S1P0 must exceed 1.2 × 10S1U1P1-2S1S1P0 M for BaFS1U1B12S1U1B0 to start precipitating.

Question 4

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Accepted Answer

The answer of 200.0 ml of a solution containing 0.5000...

Question 5

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF)and 0.180 M cesium fluoride (CsF). The K_a of hydrofluoric acid is 6.80 × 10^-4.

Accepted Answer

The answer of Calculate the pH of a buffer that...

Question 6

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

Accepted Answer

The buffer capacity is directly proportional to the concentration of the buffer components. Increasing the concentration of the acid and base in the buffer will increase its buffer capacity, allowing it to resist changes in pH to a greater extent.

Question 7

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Accepted Answer

The answer of Suppose you have just added 200.0 ml...

Question 8

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The K_a of acetic acid is 1.77 × 10^-5.

Accepted Answer

The answer of Calculate the pH of a buffer solution...

Question 9

An assembly of a metal ion and the Lewis bases bonded to it is called a(n)________.

Accepted Answer

The answer of An assembly of a metal ion and...

Question 10

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Accepted Answer

The answer of Suppose you have just added 100.0 ml...

Question 11

The solubility of a slightly soluble salt is decreased by the presence of a second solute that provides a common ion to the system.

Accepted Answer

When a second solute is added to the solution containing the slightly soluble salt, it provides a common ion which decreases the solubility of the salt. This is due to the common ion effect, which leads to a decrease in the concentration of ions in solution and a decrease in the solubility product of the salt.

Question 12

In general, the solubility of a slightly soluble salt is ________ by the presence of a second solute that furnishes a common ion.

Accepted Answer

The answer of In general, the solubility of a slightly...

Question 13

________ analysis determines only the presence or absence of a particular metal ion, whereas ________ analysis determines how much of a given substance is present.

Accepted Answer

The answer of ________ analysis determines only the presence or...

Question 14

The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.

Accepted Answer

Adding a strong electrolyte with a common ion to a solution of a weak electrolyte actually decreases the extent of ionization of the weak electrolyte due to the common ion effect, which shifts the equilibrium towards the un-ionized form of the weak electrolyte.

Question 15

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

Accepted Answer

The solubility product is the product of the concentrations of the ions, each raised to the power of its coefficient in the balanced chemical equation, not multiplied by it.

Question 16

Although CaCO₃ has a relatively small solubility product, it is quite soluble in the presence of ________.

Accepted Answer

The answer of Although CaCO₃ has a relatively small solubility...

Quiz 17: Additional Aspects of Aqueous Equilibria

The solubility of slightly soluble salts containing basic anions is proportional to the pH of the solution.

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be ________.

A solution of NaF is added dropwise to a solution that is 0.0122 M in Ba²⁺. When the concentration of F^- exceeds ________ M, BaF₂ will precipitate. Neglect volume changes. For BaF, Ksp = 1.7 × 10^-⁶.

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF)and 0.180 M cesium fluoride (CsF). The K_a of hydrofluoric acid is 6.80 × 10^-4.

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The K_a of acetic acid is 1.77 × 10^-5.

An assembly of a metal ion and the Lewis bases bonded to it is called a(n)________.

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

The solubility of a slightly soluble salt is decreased by the presence of a second solute that provides a common ion to the system.

In general, the solubility of a slightly soluble salt is ________ by the presence of a second solute that furnishes a common ion.

analysis determines only the presence or absence of a particular metal ion, whereas analysis determines how much of a given substance is present.

The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

Although CaCO₃ has a relatively small solubility product, it is quite soluble in the presence of ________.

Quiz 17: Additional Aspects of Aqueous Equilibria

The solubility of slightly soluble salts containing basic anions is proportional to the pH of the solution.

Metal oxides and hydroxides that are relatively insoluble in neutral water, but are soluble in both strongly acidic and strongly basic solutions are said to be ________.

A solution of NaF is added dropwise to a solution that is 0.0122 M in Ba2+. When the concentration of F- exceeds ________ M, BaF2 will precipitate. Neglect volume changes. For BaF, Ksp = 1.7 × 10-6.

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF)and 0.180 M cesium fluoride (CsF). The Ka of hydrofluoric acid is 6.80 × 10-4.

For any buffer system, the buffer capacity depends on the amount of acid and base from which the buffer is made.

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 × 10-5.

An assembly of a metal ion and the Lewis bases bonded to it is called a(n)________.

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The Ka of acetic acid is 1.77 × 10-5.

The solubility of a slightly soluble salt is decreased by the presence of a second solute that provides a common ion to the system.

In general, the solubility of a slightly soluble salt is ________ by the presence of a second solute that furnishes a common ion.

________ analysis determines only the presence or absence of a particular metal ion, whereas ________ analysis determines how much of a given substance is present.

The extent of ionization of a weak electrolyte is increased by adding to the solution a strong electrolyte that has an ion in common with the weak electrolyte.

The solubility product of a compound is numerically equal to the product of the concentration of the ions involved in the equilibrium, each multiplied by its coefficient in the equilibrium reaction.

Although CaCO3 has a relatively small solubility product, it is quite soluble in the presence of ________.

A solution of NaF is added dropwise to a solution that is 0.0122 M in Ba²⁺. When the concentration of F^- exceeds ________ M, BaF₂ will precipitate. Neglect volume changes. For BaF, Ksp = 1.7 × 10^-⁶.

200.0 ml of a solution containing 0.5000 moles of acetic acid per liter is added to 200.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Calculate the pH of a buffer that contains 0.270 M hydrofluoric acid (HF)and 0.180 M cesium fluoride (CsF). The K_a of hydrofluoric acid is 6.80 × 10^-4.

Suppose you have just added 200.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 100.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate and 0.010 moles of acetic acid in 100 ml of water. The K_a of acetic acid is 1.77 × 10^-5.

Suppose you have just added 100.0 ml of a solution containing 0.5000 moles of acetic acid per liter to 400.0 ml of 0.5000 M NaOH. What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

analysis determines only the presence or absence of a particular metal ion, whereas analysis determines how much of a given substance is present.

Although CaCO₃ has a relatively small solubility product, it is quite soluble in the presence of ________.