Question 1

Which of the following compounds will undergo a gas-evolving reaction in an aqueous solution? A) CH₃COOH B) HF C) HCl D) H₂SO₄ E) H₂CO₃

Accepted Answer

H₂CO₃ (carbonic acid) decomposes into CO₂ (carbon dioxide) gas and H₂O (water) in aqueous solution, leading to a gas-evolving reaction.

Question 2

A beaker contains 0.50 mol of potassium bromide in 600 mL of water.An additional 600 mL of water is added.The number of moles of potassium bromide in the beaker is
A) 0.50 mol.
B) 0.83 mol.
C) 0.25 mol.
D) 1.2 mol.
E) 0.42 mol.

Accepted Answer

The number of moles of potassium bromide in the solution does not change when more water is added. Therefore, the solution still contains 0.50 mol of potassium bromide.

Question 3

Which of the following is a strong electrolyte in solution? A) CdS B) FeCl₃ C) CH₃COOH D) NiC₂O₄ E) PbMnO₄

Accepted Answer

FeCl₃ is a strong electrolyte because it completely dissociates into its ions (Fe³⁺ and Cl^-) in solution, allowing it to conduct electricity efficiently.

Question 4

If 4.89 g of ZnCl₂ is dissolved in enough water to give a total volume of 500 mL,what is the molarity of the solution? A) 0.217 M B) 0.0179 M C) 0.0717 M D) 1.33 M E) 0.849 M

Accepted Answer

We first need to calculate the number of moles of ZnCl2 in the solution:

moles of ZnCl2 = 4.89 g / (136.29 g/mol) = 0.0359 mol

Then, we can use the formula for molarity:

Molarity = moles of solute / liters of solution

Since we have 500 mL (or 0.5 L) of solution, we can calculate the molarity:

Molarity = 0.0359 mol / 0.5 L = 0.0717 M

Therefore, the best choice is C.

Question 5

6.74 g of the monoprotic acid KHP (MW = 204.2 g/mol)is dissolved into water.The sample is titrated with a 0.703 M solution of calcium hydroxide to the equivalence point.What volume of base was used?
A) 8.64 mL
B) 11.8 mL
C) 23.5 mL
D) 47.0 mL
E) 93.9 mL

Accepted Answer

The answer of 6.74 g of the monoprotic acid KHP...

Question 6

Determine the oxidation state of P in PO₃^3-. A) +3 B) +6 C) +2 D) 0 E) -3

Accepted Answer

The given formula seems to be a non-standard representation of a chemical species. However, assuming standard oxidation states for oxygen (O = -2) and sulfur (S = -2), and knowing that the sum of oxidation states in a neutral compound must equal zero, we can deduce the oxidation state of phosphorus (P). In compounds, phosphorus can exhibit various oxidation states, but +3 and +5 are common. Given the context and the options provided, +3 is the correct choice for the oxidation state of phosphorus in this compound.

Question 7

What element is undergoing reduction (if any)in the following reaction? Zn(s)+ 2 AgNO₃(aq)→ Zn(NO₃)₂(aq)+ 2 Ag(s) A) Zn B) N C) O D) Ag E) This is not an oxidation-reduction reaction.

Accepted Answer

Ag is undergoing reduction because it gains electrons, going from Ag+ in AgNO3 to Ag(s) in the products.

Question 8

Determine the reducing agent in the following reaction. 2 Li(s)+ Fe(C₂H₃O₂)₂(aq)→ 2 LiC₂H₃O₂(aq)+ Fe(s) A) O B) H C) C D) Fe E) Li

Accepted Answer

Lithium (Li) is the reducing agent because it loses electrons (is oxidized) to reduce the iron compound, resulting in lithium ions in the product.

Question 9

Determine the oxidation state of nitrogen in NO.
A) +5
B) +3
C) 0
D) +2
E) +4

Accepted Answer

In NO, oxygen has an oxidation state of -2. Since the compound is neutral, nitrogen must have an oxidation state of +2 to balance the -2 from oxygen.

Question 10

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 M KOH solution.What is the concentration of the H₃PO₄ solution (in M)? A) 1.03 M B) 0.343 M C) 0.114 M D) 0.138 M E) 0.0461 M

Accepted Answer

The answer of The titration of 80.0 mL of an...

Question 11

Determine the oxidation state of nitrogen in NO₂. A) +5 B) +3 C) 0 D) +2 E) +4

Accepted Answer

In NO₂, oxygen has an oxidation state of -2. Since there are two oxygen atoms, their total contribution is -4. To balance this, nitrogen must have an oxidation state of +4.

Question 12

What element is undergoing oxidation (if any)in the following reaction? CH₄(g)+ 2 O₂(g)→ CO₂(g)+ 2 H₂O(g) A) O B) H C) C D) both C and H E) None of the elements is undergoing oxidation.

Accepted Answer

The answer of What element is undergoing oxidation (if any)in...

Question 13

Determine the oxidizing agent in the following reaction. Ni(s)+ 2 AgClO₄(aq)→ Ni(ClO₄)₂(aq)+ 2 Ag(s) A) Ag B) Ni C) Cl D) O E) This is not an oxidation-reduction reaction.

Accepted Answer

In the given reaction, silver ion (Ag+) is reduced to silver (Ag) while nickel atom (Ni) is oxidized to nickel ion (Ni2+). Therefore, silver ion (Ag+) is the oxidizing agent as it causes the oxidation of nickel atom (Ni).

Question 14

When an aqueous solution of manganese (II)nitrate is combined with an aqueous solution of ammonium sulfide,what should precipitate out? A) MnS B) Mn(SO₃)₂ C) Mn(SO₄)₂ D) Mn₂SO₃ E) Mn₂SO₄

Accepted Answer

When ammonium sulfide is added to manganese (II) nitrate, a double displacement reaction occurs where the cation from the sulfide solution combines with the anion from the nitrate solution, resulting in the formation of a precipitate. In this case, the cation from the sulfide solution is ammonium (NH4+) while the anion from the nitrate solution is Mn2+. Therefore, the most likely product is a solid manganese sulfide (MnS). Choice A is the only option that includes MnS as the potential product.

Question 15

What element is undergoing oxidation (if any)in the following reaction? 2 MnO₄^-(aq)+ 3 NO₂^-(aq)+ H₂O(l)→ 2 MnO₂(s)+ 3 NO₃^-(aq)+ 2 OH^-(aq) A) Mn B) O C) N D) H E) This is not an oxidation-reduction reaction

Accepted Answer

Nitrogen is undergoing oxidation as its oxidation state increases from +3 in NO₂⁻ to +5 in NO₃⁻.

Question 16

What is the name for an aqueous solution of HIO?
A) hydroiodic acid
B) hypoiodous acid
C) iodous acid
D) iodic acid
E) periodic acid

Accepted Answer

Hypoiodous acid is the name for an aqueous solution of HIO.

Question 17

Determine the oxidation state of C in CO₃^-2. A) +4 B) +2 C) -2 D) -4 E) +6

Accepted Answer

The answer of Determine the oxidation state of C in...

Question 18

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of 0.12 M LiOH solution.What is the concentration of the H₂SO₄ solution (in M)? A) 0.20 M B) 0.40 M C) 0.10 M D) 0.36 M E) 0.25 M

Accepted Answer

The concentration of the unknown solution can be found using the titration formula: $M_1V_1 = M_2V_2$, where $M_1$ and $M_2$ are the molarities of the two solutions, and $V_1$ and $V_2$ are their volumes. Given $M_2 = 0.12 \, M$, $V_2 = 83.6 \, mL$, and $V_1 = 25.0 \, mL$, we can solve for $M_1$: $M_1 = \frac{M_2V_2}{V_1} = \frac{0.12 \, M \times 83.6 \, mL}{25.0 \, mL} = 0.40128 \, M$, which rounds to $0.40 \, M$, making choice B correct.

Question 19

What element is undergoing oxidation (if any)in the following reaction? Zn(s)+ 2 AgNO₃(aq)→ Zn(NO₃)₂(aq)+ 2 Ag(s) A) Zn B) N C) O D) Ag E) This is not an oxidation-reduction reaction.

Accepted Answer

In this reaction, Zn goes from a neutral charge to a +2 charge in the product while Ag goes from a +1 charge to 0 in the product. This means that Zn has lost electrons, or undergone oxidation, while Ag has gained electrons, or undergone reduction. Therefore, the element undergoing oxidation is Zn.

Question 20

All of the following compounds are soluble EXCEPT A) Ba(OH)₂. B) Pb(NO₃)₂. C) ZnCl₂. D) AgBr. E) Cu(C₂H₃O₂)₂.

Accepted Answer

AgBr (silver bromide) is insoluble in water.

Quiz 9: Introduction to Solutions and Aqueous Reactions

Which of the following compounds will undergo a gas-evolving reaction in an aqueous solution?

A beaker contains 0.50 mol of potassium bromide in 600 mL of water.An additional 600 mL of water is added.The number of moles of potassium bromide in the beaker is

Which of the following is a strong electrolyte in solution?

If 4.89 g of ZnCl₂ is dissolved in enough water to give a total volume of 500 mL,what is the molarity of the solution?

6.74 g of the monoprotic acid KHP (MW = 204.2 g/mol) is dissolved into water.The sample is titrated with a 0.703 M solution of calcium hydroxide to the equivalence point.What volume of base was used?

Determine the oxidation state of P in PO₃^3-.

What element is undergoing reduction (if any) in the following reaction? Zn(s) + 2 AgNO₃(aq) → Zn(NO₃) ₂(aq) + 2 Ag(s)

Determine the reducing agent in the following reaction. 2 Li(s) + Fe(C₂H₃O₂) ₂(aq) → 2 LiC₂H₃O₂(aq) + Fe(s)

Determine the oxidation state of nitrogen in NO.

The titration of 80.0 mL of an unknown concentration H₃PO₄ solution requires 126 mL of 0.218 M KOH solution.What is the concentration of the H₃PO₄ solution (in M) ?

Determine the oxidation state of nitrogen in NO₂.

What element is undergoing oxidation (if any) in the following reaction? CH₄(g) + 2 O₂(g) → CO₂(g) + 2 H₂O(g)

Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO₄(aq) → Ni(ClO₄) ₂(aq) + 2 Ag(s)

When an aqueous solution of manganese (II) nitrate is combined with an aqueous solution of ammonium sulfide,what should precipitate out?

What element is undergoing oxidation (if any) in the following reaction? 2 MnO₄^-(aq) + 3 NO₂^-(aq) + H₂O(l) → 2 MnO₂(s) + 3 NO₃^-(aq) + 2 OH^-(aq)

What is the name for an aqueous solution of HIO?

Determine the oxidation state of C in CO₃^-2.

The titration of 25.0 mL of an unknown concentration H₂SO₄ solution requires 83.6 mL of 0.12 M LiOH solution.What is the concentration of the H₂SO₄ solution (in M) ?

What element is undergoing oxidation (if any) in the following reaction? Zn(s) + 2 AgNO₃(aq) → Zn(NO₃) ₂(aq) + 2 Ag(s)

All of the following compounds are soluble EXCEPT

Quiz 9: Introduction to Solutions and Aqueous Reactions

Which of the following compounds will undergo a gas-evolving reaction in an aqueous solution?

A beaker contains 0.50 mol of potassium bromide in 600 mL of water.An additional 600 mL of water is added.The number of moles of potassium bromide in the beaker is

Which of the following is a strong electrolyte in solution?

If 4.89 g of ZnCl2 is dissolved in enough water to give a total volume of 500 mL,what is the molarity of the solution?

6.74 g of the monoprotic acid KHP (MW = 204.2 g/mol) is dissolved into water.The sample is titrated with a 0.703 M solution of calcium hydroxide to the equivalence point.What volume of base was used?

Determine the oxidation state of P in PO33-.

What element is undergoing reduction (if any) in the following reaction? Zn(s) + 2 AgNO3(aq) → Zn(NO3) 2(aq) + 2 Ag(s)

Determine the reducing agent in the following reaction. 2 Li(s) + Fe(C2H3O2) 2(aq) → 2 LiC2H3O2(aq) + Fe(s)

Determine the oxidation state of nitrogen in NO.

The titration of 80.0 mL of an unknown concentration H3PO4 solution requires 126 mL of 0.218 M KOH solution.What is the concentration of the H3PO4 solution (in M) ?

Determine the oxidation state of nitrogen in NO2.

What element is undergoing oxidation (if any) in the following reaction? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)

Determine the oxidizing agent in the following reaction. Ni(s) + 2 AgClO4(aq) → Ni(ClO4) 2(aq) + 2 Ag(s)