Question 1

Suppose you have just added 100.0 ml of a solution containing 1.00 mole of acetic acid per liter to 500.0 ml of 0.100 M KOH.What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

Accepted Answer

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Question 2

________ analysis determines how much of a given substance is present.

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The answer of ________ analysis determines how much of a...

Question 3

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 ________.

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Question 4

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

Accepted Answer

This statement is true and represents the solubility product constant expression, Ksp, for a compound in solution. For example, the Ksp expression for the dissociation of the ionic compound silver chloride (AgCl) in aqueous solution is Ksp = [Ag+][Cl-], where the concentration of silver ions and chloride ions are each raised to the power of 1 (their coefficients in the dissociation reaction).

Question 5

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

Accepted Answer

The presence of a second solute that provides a common ion usually decreases the solubility of a slightly soluble salt due to the common ion effect, which shifts the equilibrium towards the reactants, reducing solubility.

Question 6

Suppose you have just added 500.0 ml of a solution containing 0.2000 moles of acetic acid per liter to 200.0 ml of 0.250 M NaOH.What is the final pH? The K_a of acetic acid is 1.77 × 10^-5.

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Question 7

CaCO₃ is very soluble in the presence of ________.

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Question 8

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

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Question 9

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

Accepted Answer

Buffer capacity is determined by the concentration of both the weak acid and its conjugate base or the weak base and its conjugate acid in the buffer solution. The more acid and base present, the greater the buffer capacity. Therefore, the statement is true.

Question 10

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

Accepted Answer

The solubility of slightly soluble salts containing basic anions is inversely proportional to the pH of the solution because increasing pH decreases the concentration of H+ ions, which can react with the basic anions to form less soluble compounds.

Question 11

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.

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Question 12

A solution of NaF is added dropwise to a solution that is 0.0122 M in  .When the concentration of  exceeds ________ M,  will precipitate.Neglect volume changes.For  ,

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Question 13

Calculate the pH of a buffer solution that contains 0.010 moles of A^- and 0.010 moles of HA in 100 ml of water.The K_a of HA is 1.77 × 10^-5.

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Question 14

A complex ion is when a metal ion binds to a ________.

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Question 15

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 16

Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0 ml of 0.6000 M NaOH.What is the final pH? The K_a of HA is 1.77 × 10^-5.

Accepted Answer

The answer of Suppose you have just added 50.0 ml...

Quiz 17: Additional Aspects of Aqueous Equilibria

Suppose you have just added 100.0 ml of a solution containing 1.00 mole of acetic acid per liter to 500.0 ml of 0.100 M KOH.What is the final pH? The Ka of acetic acid is 1.77 × 10-5.