Question 1

In which of the following aqueous solutions would you expect PbCl₂to have the lowest solubility? A)0.020 M KCl B)0.020 M BaCl₂ C)0.015 M PbNO₃ D)pure water E)0.015 M NaCl

Accepted Answer

According to the common ion effect, the presence of a common ion (in this case, chloride) will decrease the solubility of a salt (PbCl2). Option B contains the highest concentration of chloride ions, thus it will have the greatest effect on decreasing the solubility of PbCl2. Therefore, PbCl2 would have the lowest solubility in 0.020 M BaCl2.

Question 2

A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The unknown compound is __________.
A)a strong acid
B)a strong base
C)a weak acid
D)a weak base
E)neither an acid nor a base

Accepted Answer

From the titration curve, we can see that the equivalence point is reached around 30 mL of NaOH added. Additionally, we can see that the pH at the equivalence point is greater than 7, indicating that the unknown compound was originally an acid. Since the pH at the equivalence point is not very high, this suggests that the acid is weak. Therefore, the best choice is (C) a weak acid.

Question 3

What are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood?
A)kidneys, liver
B)lungs, kidneys
C)spleen, liver
D)lungs, skin
E)brain stem, heart

Accepted Answer

The lungs and kidneys are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood. The lungs regulate the amount of carbon dioxide in the blood, which affects the level of carbonic acid, while the kidneys regulate the reabsorption and excretion of bicarbonate ions. The other options (A, C, D, and E) do not play a significant role in regulating this buffer system.

Question 4

In which of the following aqueous solutions would you expect CuBr to have the highest solubility? A)pure water B)0.10 M AgNO₃ C)0.20 M NaBr D)0.15 M KBr E)0.10 M LiBr

Accepted Answer

CuBr is more soluble in pure water compared to solutions containing common ions like Br⁻, which decrease its solubility due to the common ion effect.

Question 5

Which below best describe(s)the behavior of an amphoteric hydroxide in water?
A)With conc. aq. NaOH, its suspension dissolves.
B)With conc. aq. HCl, its suspension dissolves.
C)With conc. aq. NaOH, its clear solution forms a precipitate.
D)With conc. aq. HCl, its clear solution forms a precipitate.
E)With both conc. aq. NaOH and conc. aq. HCl, its suspension dissolves.

Accepted Answer

An amphoteric hydroxide can react with both acids and bases. Therefore, it will dissolve in both conc. aq. NaOH and conc. aq. HCl. None of the other options are true for all amphoteric hydroxides.

Question 6

The primary buffer system that controls the pH of the blood is the __________ buffer system.
A)carbon dioxide, carbonate
B)carbonate, bicarbonate
C)carbonic acid, carbon dioxide
D)carbonate, carbonic acid
E)carbonic acid, bicarbonate

Accepted Answer

The bicarbonate buffer system is the primary buffer system that controls the pH of the blood. This system involves the reversible reaction between carbonic acid and bicarbonate ions, with the enzyme carbonic anhydrase facilitating the conversion of carbon dioxide and water to carbonic acid. Changes in the concentration of either component can shift the balance of the system and adjust blood pH.

Question 7

Which compound listed below has the smallest molar solubility in water? A)ZnCO₃ B)Cd(OH)₂ C)CdCO₃ D)AgI E)CaF₂

Accepted Answer

AgI has the smallest molar solubility in water among the options given. This is because AgI is known for its very low solubility product (Ksp), indicating that it dissolves in water to a much lesser extent compared to the other compounds listed.

Question 8

The molar solubility of __________ is not affected by the pH of the solution. A)Na₃PO₄ B)NaF C)KNO₃ D)ACl₃ E)MnS

Accepted Answer

KNO₃ is a salt of a strong acid (HNO₃) and a strong base (KOH), so its solubility is not affected by the pH of the solution.

Question 9

Which one of the following will cause hemoglobin to release oxygen? A)increase in pH B)decrease in pH C)decrease in temperature D)decrease in CO₂ concentration E)increase in O₂ concentration

Accepted Answer

A decrease in pH, also known as an increase in acidity, causes hemoglobin to release oxygen to tissues in need of oxygen. This is known as the Bohr effect.

Question 10

In which of the following aqueous solutions would you expect AgCl to have the highest solubility? A)pure water B)0.020 M BaCl₂ C)0.015 NaCl D)0.020 AgNO₃ E)0.020 KCl

Accepted Answer

The solubility of AgCl is very low in pure water, but it can dissolve in the presence of Cl- ions due to the formation of AgCl complex. None of the given options contain Cl- ions except for pure water. Therefore, AgCl is expected to have the highest solubility in pure water.

Question 11

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility? A)pure water B)0.20 M NaBr C)0.10 M AgNO₃ D)0.15 M KBr E)0.10 M LiBr

Accepted Answer

AgBr has low solubility in a solution with a high concentration of Br- ions because the common ion effect causes the equilibrium to shift towards AgBr precipitation. Therefore, in the presence of a solution with a high concentration of Br- ions, AgBr will have the lowest solubility. Among the options given, option B has the highest concentration of Br- ions (0.20 M NaBr).

Question 12

Human blood is __________.
A)neutral
B)very basic
C)slightly acidic
D)very acidic
E)slightly basic

Accepted Answer

Human blood has a pH of approximately 7.4, which is slightly basic.

Question 13

Which one of the following is not amphoteric? A)Al(OH)₃ B)Ca(OH)₂ C)Cr(OH)₃ D)Zn(OH)₂ E)Sn(OH)₂

Accepted Answer

Calcium hydroxide (Ca(OH)2) is a base and does not exhibit amphoteric behavior, unlike the other compounds listed which can act as both acids and bases.

Question 14

Which compound listed below has the greatest molar solubility in water? A)CdCO₃ B)Cd(OH)₂ C)AgI D)CaF₂ E)ZnCO₃

Accepted Answer

CaF2 has the greatest molar solubility in water among the options given. This is because, compared to the other compounds listed, which are either sparingly soluble (such as AgI and CdCO3) or have very low solubility due to their strong ionic bonds and low solubility product constants (Ksp), calcium fluoride (CaF2), despite also being sparingly soluble, tends to have a slightly higher solubility than the other compounds mentioned. This is a relative comparison, as all the compounds are generally considered to have low solubility in water, but among them, CaF2 is expected to dissolve more than the others under the same conditions.

Question 15

For which salt should the aqueous solubility be most sensitive to pH? A)Ca(NO₃)₂ B)CaF₂ C)CaCl₂ D)CaBr₂ E)CaI₂

Accepted Answer

The answer of For which salt should the aqueous solubility...

Question 16

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility? A)pure water B)0.020 M BaCl₂ C)0.015 NaCl D)0.020 AgNO₃ E)0.020 KCl

Accepted Answer

The answer of In which of the following aqueous solutions...

Question 17

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about __________ mol/L.
A)25.0
B)0.0600
C)0.240
D)0.120
E)0.100

Accepted Answer

The answer of A 25.0 mL sample of a solution...

Question 18

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. Which of the following indicators would be best for this titration?
A)methyl red
B)bromthymol blue
C)thymol blue
D)phenolpthalein
E)bromocresol purple

Accepted Answer

The answer of A 25.0 mL sample of a solution...

Question 19

In which of the following aqueous solutions would you expect AgBr to have the highest solubility? A)0.10 M LiBr B)0.10 M AgNO₃ C)0.20 M NaBr D)0.15 M KBr E)pure water

Accepted Answer

AgBr is insoluble in water, but it has a solubility product constant (Ksp). When the concentration of the ions in the solution is less than the Ksp for AgBr, the solution becomes saturated and AgBr precipitates out of the solution. Since pure water has the lowest ion concentration among the options, AgBr is expected to have the highest solubility in pure water.

Question 20

In which one of the following solutions is silver chloride the most soluble? A)0.181 M HCl B)0.0176 M NH₃ C)0.744 M LiNO₃ D)pure water E)0.181 M NaCl

Accepted Answer

The answer of In which one of the following solutions...

Quiz 17: Additional Aspects of Aqueous Equilibria

In which of the following aqueous solutions would you expect PbCl₂to have the lowest solubility?

A 25.0 mL sample of a solution of an unknown compound is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The unknown compound is __________.

What are the principal organs that regulate the pH of the carbonic acid-bicarbonate buffer system in the blood?

In which of the following aqueous solutions would you expect CuBr to have the highest solubility?

Which below best describe(s) the behavior of an amphoteric hydroxide in water?

The primary buffer system that controls the pH of the blood is the __________ buffer system.

Which compound listed below has the smallest molar solubility in water?

The molar solubility of __________ is not affected by the pH of the solution.

Which one of the following will cause hemoglobin to release oxygen?

In which of the following aqueous solutions would you expect AgCl to have the highest solubility?

In which of the following aqueous solutions would you expect AgBr to have the lowest solubility?

Human blood is __________.

Which one of the following is not amphoteric?

Which compound listed below has the greatest molar solubility in water?

For which salt should the aqueous solubility be most sensitive to pH?

In which of the following aqueous solutions would you expect AgCl to have the lowest solubility?

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. The concentration of the monoprotic acid is about __________ mol/L.

A 25.0 mL sample of a solution of a monoprotic acid is titrated with a 0.115 M NaOH solution. The titration curve above was obtained. Which of the following indicators would be best for this titration?

In which of the following aqueous solutions would you expect AgBr to have the highest solubility?

In which one of the following solutions is silver chloride the most soluble?