Question 1

What are the spectator ions in the reaction of barium hydroxide and nitric acid? A)H₃O^- and NO₃^- B)Ba²⁺ and OH^- C)H₃O⁺ and OH^- D)Ba²⁺ and NO₃^- E)Ba²⁺, NO₃^-, H₃O⁺, and OH^-

Accepted Answer

Spectator ions are ions that do not participate in the chemical reaction and remain in solution unchanged. In the reaction between barium hydroxide and nitric acid, the barium ($Ba^{2+}$) and nitrate ($NO_3^-$) ions are the spectator ions, as the reaction primarily involves the hydrogen ions ($H^+$) from the acid reacting with the hydroxide ions ($OH^-$) from the base to form water.

Question 2

Identify a spectator ion in the following acid-base reaction. Ca(CO₃)(s) 2HCl(aq) CaCl₂(aq) 2H₂O(l ) CO₂(g) A)H⁺ B)Ca²⁺ C)Cl^- D)CO₃^2- E)H₃O⁺

Accepted Answer

The spectator ion is the Cl- ion, which does not participate in the chemical reaction and remains unchanged. In this reaction, Ca2+ and Cl- ions combine to form CaCl2, while the other ions (HSO4-, CO32-, and H+) participate in forming the other products.

Question 3

If the molar concentration of sodium sulfate (Na₂SO₄) is 0.10 M, what is the concentration of sodium ion? A)0.10 M B)0.050 M C)0.20 M D)0.30 M E)0.40 M

Accepted Answer

Sodium sulfate (Na2SO4) dissociates in water to form 2 sodium ions (Na+) and 1 sulfate ion (SO4^2-). Therefore, a 0.10 M solution of sodium sulfate will produce a 0.20 M concentration of sodium ions because each formula unit of sodium sulfate produces two sodium ions upon dissociation.

Question 4

Which one of the following statements regarding a weak base is not correct?
A)A weak base ionizes only to a small extent in water.
B)A weak base ionizes in water to produce hydroxide ions.
C)A weak base neutralizes acids.
D)Sodium hydroxide is an example of a weak base.
E)A weak base can also be a weak electrolyte.

Accepted Answer

Sodium hydroxide is actually a strong base, not a weak base.

Question 5

Which picture best represents an atomic-level view of hydrochloric acid, which is a strong acid, in aqueous solution (water molecules not shown)?
A) 
B) 
C) 
D)

Accepted Answer

Choice C shows an atomic-level view of hydrochloric acid, with the hydrogen ion (H+) dissociated from the chloride ion (Cl-) in aqueous solution. This represents the strong acidity of hydrochloric acid. Choices A and B show individual atoms without any indication of dissociation, and choice D shows a covalent bond between atoms rather than the ionic bond present in hydrochloric acid.

Question 6

What is the molar concentration of sodium ions in a 0.3 M sodium phosphate (Na₃PO₄, 164 g/mol) solution? Sodium phosphate is used as a cleaning agent, food additive, and stain remover. A)0.1 M B)0.3 M C)0.6 M D)0.9 M E)1.0 M

Accepted Answer

Sodium phosphate (Na3PO4) dissociates in water to form three sodium ions (Na+) and one phosphate ion (PO4^3-). Therefore, for every 1 mole of sodium phosphate that dissolves, 3 moles of sodium ions are produced. Given a 0.3 M solution of sodium phosphate, the concentration of sodium ions will be 0.3 M * 3 = 0.9 M.

Question 7

Hartmann's solution is used in intravenous therapy to replace lost body fluid and mineral salts. Hartmann's solution contains 5.00 mM potassium chloride, 2.00 mM calcium chloride, and 102 mM sodium chloride. What is the total chloride ion concentration in Hartmann's solution?
A)109 mM
B)107 mM
C)111 mM
D)104 mM
E)218 mM

Accepted Answer

The total chloride ion concentration is the sum of chloride ions from all sources: 5.00 mM from potassium chloride, 2.00 mM from calcium chloride, and 102 mM from sodium chloride, totaling 109 mM.

Question 8

In a demonstration of strong electrolytes, weak electrolytes, and nonelectrolytes, Professor Popsnorkle used a lightbulb apparatus that showed how much a solution conducted electricity by the brightness of the lightbulb. When pure water was tested, the bulb did not light. When some acetic acid was added to the water, the bulb burned dimly. When more acetic acid was added to the solution, the bulb burned a little more brightly. In his frustration to make the bulb shine brightly with acetic acid, Professor Popsnorkle started over by testing the beaker of the pure acetic acid. What was the result?
A)The bulb did not light.
B)The bulb burned dimly.
C)The bulb burned more than any of the others but still not brightly.
D)The bulb burned brightly.
E)Professor Popsnorkle was electrocuted.

Accepted Answer

Pure acetic acid is a weak electrolyte because it does not dissociate completely in water. However, in its pure form, without water to facilitate the ionization process, it hardly conducts electricity at all, hence the bulb would not light.

Question 9

What is the molar concentration of sodium in a 200.0 mL solution prepared from 1.223 g of sodium phosphate (Na₃PO₄, 163.9 g/mol), which is a cleaning agent, food additive, and stain remover? A)0.03731 M B)0.2486 M C)0.7338 M D)0.1119 M E)0.1243 M

Accepted Answer

The answer of What is the molar concentration of sodium...

Question 10

If 50.0 mL of a 0.10 M solution of sodium chloride is mixed with 50.0 mL of 0.10 M magnesium chloride, what is the molar concentration of chloride in the resulting solution?
A)0.10 M
B)0.20 M
C)0.05 M
D)0.15 M
E)0.25 M

Accepted Answer

The answer of If 50.0 mL of a 0.10 M...

Question 11

In its reaction with water, ammonia (NH₃) ________ A)acts as an acid. B)acts as a base. C)acts neither as an acid nor as a base. D)serves as both an acid and as a base. E)causes a precipitate to form.

Accepted Answer

Ammonia acts as a base when it reacts with water, producing NH4+ and OH- ions.

Question 12

Identify the base in the following acid-base reaction. NaNO₂(aq) HI(aq) NaI(aq) HNO₂(aq) A)Na⁺ B)NO₂^- C)I^- D)HI E)HNO₂

Accepted Answer

The answer of Identify the base in the following acid-base...

Question 13

Which of the following compounds is a nonelectrolyte? A)sulfuric acid, H₂SO₄ B)acetic acid, CH₃COOH C)hexane, C₆H₁₄ D)nitrous acid, HNO₂ E)potassium hydroxide, KOH

Accepted Answer

Hexane is a nonpolar compound, therefore it does not dissociate into ions and does not conduct electricity in solution. All of the other compounds listed are either strong or weak electrolytes, meaning they dissociate into ions in solution and can conduct electricity.

Question 14

In the following reaction, H₂O ________ CH₃COOH(aq) H₂O(l) CH₃COO^-(aq) H₃O⁺(aq) A)acts as an acid. B)acts as a base. C)acts neither as an acid nor as a base. D)serves as both an acid and as a base. E)causes a precipitate to form.

Accepted Answer

The answer of In the following reaction, H₂O ________ CH₃COOH(aq)...

Question 15

Which one of the following is the molecular equation for the reaction of hydrobromic acid with potassium hydroxide? All species are in aqueous solution. A)H⁺ Br ^- K⁺ OH^- KBr H₂O B)H⁺ Br ^- K⁺ OH^- K⁺ Br ^- H₂O C)HBr KOH KBr H₂O D)K⁺ Br^- KBr E)H⁺ OH^- H₂O

Accepted Answer

The molecular equation is the balanced chemical equation for the reaction in which the reactants and products are written as undissociated molecules. The balanced molecular equation for the reaction of hydrobromic acid with potassium hydroxide is:

HBr(aq) + KOH(aq) → KBr(aq) + H2O(l)

Option C is the only choice that represents the correct balanced molecular equation for the reaction. Option A, B, D, and E do not represent the balanced molecular equation for the given reaction.

Question 16

In a demonstration of strong electrolytes, weak electrolytes, and nonelectrolytes, Professor Popsnorkle used a lightbulb apparatus that showed how much a solution conducted electricity by the brightness of the lightbulb. When pure water was tested, the bulb did not light. Then Professor Popsnorkle tested the following aqueous solutions. Which one caused the bulb to burn the brightest? A)table salt, NaCl B)ethanol, CH₃CH₂OH C)table sugar, C₁₂H₂₂O₁₁ D)acetic acid, CH₃COOH E)methanol, CH₃OH

Accepted Answer

Table salt (NaCl) is a strong electrolyte, meaning that when it is dissolved in water, it completely dissociates into ions that can conduct electricity. This results in a very bright lightbulb, indicating a high conductivity of electricity. Ethanol (B) and table sugar (C) are both nonelectrolytes, meaning they do not produce ions in solution and thus cannot conduct electricity. Acetic acid (D) is a weak electrolyte, meaning it partially dissociates into ions in solution and can conduct some electricity, but not to the extent of a strong electrolyte like NaCl. Methanol (E) is also a weak electrolyte.

Question 17

Which one of the following reaction equations is the net ionic equation for the reaction of hydrochloric acid with lithium hydroxide? All species are in aqueous solution. A)HCl LiOH LiCl H₂O B)H⁺ Cl^- Li⁺ OH^- Li⁺ Cl^- H₂O C)H⁺ Cl^- Li⁺ OH^- LiCl H₂O D)Li⁺ Cl^- LiCl E)H⁺ OH^- H₂O

Accepted Answer

The answer of Which one of the following reaction equations...

Question 18

Identify the acid in the following acid-base reaction. PbCO₃(s) H₂SO₄(aq) PbSO₄(s) CO₂(g) H₂O(l) A)PbCO₃(s) B)CO₂(g) C)PbSO₄(s) D)H₂O(l) E)H₂SO₄(aq)

Accepted Answer

In the given reaction, the acid is the species which donates a proton or H+ ion. Here, the aqueous solution of sulfuric acid (HSO4-) donates a proton to the aqueous solution of carbonate ion (CO32-), forming aqueous solution of hydrogen carbonate ion (HCO3-) and sulfate ion (SO42-). Therefore, the acid in the given reaction is HSO4- (or sulfuric acid). Choice E includes HSO4- in its formula.

Question 19

Which one of the following statements regarding a strong acid is not correct?
A)A strong acid ionizes completely in water.
B)A strong acid ionizes in water to produce hydronium ions.
C)A strong acid neutralizes bases.
D)HCl is an example of a strong acid.
E)Acids are only strong at a high concentration.

Accepted Answer

Acids can be strong even at low concentrations. The concentration of an acid affects its pH and acidity, but it does not determine whether it is strong or weak.

Question 20

Chalk contains calcium carbonate. What would be the best solution for cleaning a sidewalk that a preschool class covered with smiling suns, flowers, birds, rainbows, and houses using sidewalk chalk?
A)ammonia
B)plain water
C)vinegar
D)paint thinner
E)olive oil

Accepted Answer

Vinegar is acidic and can react with calcium carbonate in chalk, helping to dissolve and remove it from surfaces.

Quiz 4: Solution Chemistry: The Hydrosphere

What are the spectator ions in the reaction of barium hydroxide and nitric acid?

Identify a spectator ion in the following acid-base reaction. Ca(CO₃) (s) 2HCl(aq) CaCl₂(aq) 2H₂O(l ) CO₂(g)

If the molar concentration of sodium sulfate (Na₂SO₄) is 0.10 M, what is the concentration of sodium ion?

Which one of the following statements regarding a weak base is not correct?

Which picture best represents an atomic-level view of hydrochloric acid, which is a strong acid, in aqueous solution (water molecules not shown) ?

What is the molar concentration of sodium ions in a 0.3 M sodium phosphate (Na₃PO₄, 164 g/mol) solution? Sodium phosphate is used as a cleaning agent, food additive, and stain remover.

Hartmann's solution is used in intravenous therapy to replace lost body fluid and mineral salts. Hartmann's solution contains 5.00 mM potassium chloride, 2.00 mM calcium chloride, and 102 mM sodium chloride. What is the total chloride ion concentration in Hartmann's solution?

What is the molar concentration of sodium in a 200.0 mL solution prepared from 1.223 g of sodium phosphate (Na₃PO₄, 163.9 g/mol) , which is a cleaning agent, food additive, and stain remover?

If 50.0 mL of a 0.10 M solution of sodium chloride is mixed with 50.0 mL of 0.10 M magnesium chloride, what is the molar concentration of chloride in the resulting solution?

In its reaction with water, ammonia (NH₃) ________

Identify the base in the following acid-base reaction. NaNO₂(aq) HI(aq) NaI(aq) HNO₂(aq)

Which of the following compounds is a nonelectrolyte?

In the following reaction, H₂O ________ CH₃COOH(aq) H₂O(l) CH₃COO^-(aq) H₃O⁺(aq)

Which one of the following is the molecular equation for the reaction of hydrobromic acid with potassium hydroxide? All species are in aqueous solution.

Which one of the following reaction equations is the net ionic equation for the reaction of hydrochloric acid with lithium hydroxide? All species are in aqueous solution.

Identify the acid in the following acid-base reaction. PbCO₃(s) H₂SO₄(aq) PbSO₄(s) CO₂(g) H₂O(l)

Which one of the following statements regarding a strong acid is not correct?

Chalk contains calcium carbonate. What would be the best solution for cleaning a sidewalk that a preschool class covered with smiling suns, flowers, birds, rainbows, and houses using sidewalk chalk?