Question 1

Determine the oxidation state of nitrogen in RbNO₂.

Accepted Answer

In RbNO2, rubidium (Rb) has an oxidation state of +1, and oxygen (O) has an oxidation state of -2. Let the oxidation state of nitrogen (N) be x. The sum of oxidation states in the compound is zero: +1 + x + 2(-2) = 0, solving gives x = +3.

Question 2

A solution is prepared by adding 1.50 g of solid NaCl to 50.0 mL of 0.100 M  .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

Accepted Answer

First, we need to calculate the number of moles of NaCl added to the solution: 
mass of NaCl = 1.50 g 
molar mass of NaCl = 58.44 g/mol 
moles of NaCl = (1.50 g) / (58.44 g/mol) = 0.0257 mol

Next, we need to calculate the number of moles of chloride ion (Cl-) in the original solution: 
Molarity of NaCl solution = 0.100 M 
Volume of NaCl solution = 50.0 mL = 0.0500 L 
moles of NaCl in solution = (0.100 mol/L) x (0.0500 L) = 0.00500 mol 
moles of Cl- in solution = 0.00500 mol

Now we can calculate the total number of moles of Cl- in the final solution: 
moles of Cl- in final solution = moles of Cl- from NaCl + moles of Cl- from original solution 
moles of Cl- in final solution = 0.0257 mol + 0.00500 mol = 0.0307 mol

Finally, we can calculate the molarity of Cl- in the final solution: 
Molarity of Cl- in final solution = moles of Cl- / volume of final solution 
volume of final solution = 50.0 mL = 0.0500 L 
Molarity of Cl- in final solution = 0.0307 mol / 0.0500 L = 0.613 M 
Therefore, the answer is A) 0.713.

Question 3

When 220.mL of 1.50 × 10^-4M hydrochloric acid is added to 135 mL of 1.75 × 10^-4 M Mg(OH)₂,the resulting solution will be

Accepted Answer

The reaction between hydrochloric acid and magnesium hydroxide produces magnesium chloride and water. The balanced chemical equation is:
2HCl + Mg(OH)2 → MgCl2 + 2H2O
Given the concentrations and volumes of the two solutions, we can calculate the moles of each compound present:
moles HCl = (0.00000150 mol/mL) x 0.220 L = 0.00033 mol
moles Mg(OH)2 = (0.00000175 mol/mL) x 0.135 L = 0.00024 mol
Because there are more moles of HCl than Mg(OH)2, the excess acid will react completely with the hydroxide ions from magnesium hydroxide to form water, leaving magnesium chloride in solution. Since the reaction consumes hydroxide ions, the resulting solution will be acidic. Therefore, the correct answer is B) basic.

Question 4

A solution is prepared by mixing 20.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl.What is the molarity of chloride ion in this solution?

Accepted Answer

The answer of A solution is prepared by mixing 20.0...

Question 5

Determine the oxidation state of Ti in Ti(SO₄)₂.

Accepted Answer

In this compound, the overall charge is 0. Oxygen always has an oxidation state of -2. Sulfur is usually -2, but since there are different types of sulfurs (SOS, ₄, ₂) we cannot assume all sulfurs have an oxidation state of -2. Therefore, we need to look at the oxidation state of Ti. Let x be the oxidation state of Ti. The compound can be written as Ti(SO₄)₂. Using the fact that the overall charge is 0, we can write: x + (oxidation state of SO₄) + (oxidation state of ₂) = 0 Now, we need to determine the oxidation states of each of the sulfur molecules in order to solve for x. In SO₄, the oxygen has an oxidation state of -2, and there are 4 oxygens. Therefore, the total oxidation state of the oxygens is -8. The overall oxidation state of the molecule is 0, so the sum of the oxidation states of sulfur must be +8. Since there are 2 sulfur atoms, each sulfur has an oxidation state of +4. In ₂, there is only one sulfur atom. Since the overall oxidation state of the molecule is 0, and oxygen has an oxidation state of -2, the sulfur must have an oxidation state of +2. Using these values, we can solve for x: x + (+8) + (+2) = 0 x = -10 However, oxidation states must be integers. Therefore, the closest integer to -10 is -4. This means that Ti has an oxidation state of +4. The answer is B) +4.

Question 6

What is the oxidation number of the oxygen atom in O₂^2-?

Accepted Answer

In most compounds, the oxidation number of oxygen is -2. However, there are some exceptions such as peroxides where its oxidation number is -1. In this compound, we can identify the peroxide group by the O-O bond. Therefore, the oxidation number of each oxygen atom is -1.

Question 7

How many milliliters of 0.188 M  solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

Accepted Answer

The answer of How many milliliters of 0.188 M ...

Question 8

What is the molarity of a NaOH solution if 39.1 mL of a 0.112 M   solution is required to neutralize a 25.0-mL sample of the NaOH solution?

Accepted Answer

The answer of What is the molarity of a NaOH...

Question 9

Identify the oxidation state of H in H₂(g). Mg(s)+ 2H Br(aq)→ Mg Br₂(aq)+ H₂(g)

Accepted Answer

The answer of Identify the oxidation state of H in...

Question 10

What is the oxidation number of the chromium atom in Na₂CrO₄?

Accepted Answer

In the given compound, the oxidation numbers of S, O, and P are constant (-2, -2, and +5, respectively). Therefore, by applying the compound's charge and oxidation numbers of other elements, we can determine that the oxidation number of Chromium must be +6.

Question 11

Which of the following is an oxidation-reduction reaction?

Accepted Answer

In reaction D, magnesium (Mg) is oxidized to Mg²⁺, and hydrogen ions (H⁺) are reduced to H₂ gas, indicating an oxidation-reduction reaction.

Question 12

What is the oxidation number change for the manganese atom in the following unbalanced reduction half reaction?

Accepted Answer

The answer of What is the oxidation number change for...

Question 13

Identify the oxidation state of H in H F(aq). Ca(s)+ 2H F(aq)→ Ca F₂(aq)+ H₂(g)

Accepted Answer

In HF, hydrogen is bonded to fluorine, which is more electronegative. Therefore, hydrogen has an oxidation state of +1.

Question 14

In an acid-base neutralization reaction 23.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H₂SO₄ solution?

Accepted Answer

The answer of In an acid-base neutralization reaction 23.74 mL...

Question 15

Identify the oxidation state of Ca in Ca(s). Ca(s)+ 2H F(aq)→ Ca F₂(aq)+ H₂(g)

Accepted Answer

In its elemental form, calcium (Ca) has an oxidation state of 0.

Question 16

Determine the oxidation state of fluorine in F₂.

Accepted Answer

In F₂, fluorine is in its elemental form, and elements in their natural state have an oxidation state of 0.

Question 17

Determine the oxidation state of S in K₂SO₄.

Accepted Answer

The oxidation state of K is +1 and that of O is -2. Taking this into consideration, we can assign the oxidation state of S in the given compound as follows:
(+1) + S + (+1) + (-2) + (+1) + (+4) + S + (+1) + (+4) + (+1) + (-2) + S + (+1) + (+4) + (+1) + (-2) + 0 = 0
Solving this equation, we get the oxidation state of S to be +6. Therefore, the correct option is D.

Question 18

Determine the oxidation state of nitrogen in NaNO₃.

Accepted Answer

In NaNO3, sodium (Na) has an oxidation state of +1, and each oxygen (O) has an oxidation state of -2. The sum of oxidation states in a neutral compound is zero. Therefore, for nitrogen (N) in NaNO3: +1 (Na) + x (N) + 3(-2) (O) = 0, solving gives x = +5.

Question 19

What is the oxidation number of the sulfur atom in Li₂SO₄?

Accepted Answer

The oxidation number of sulfur in SO4^2- is +6 and sulfur is present in SO4 ion, therefore, the oxidation number of sulfur would be +6.

Question 20

Identify the oxidation state of Ca in Ca Br₂(aq). Ca(s)+ 2H Br(aq)→ Ca Br₂(aq)+ H₂(g)

Accepted Answer

The oxidation state of Br, S, and H is -1, -2, and +1, respectively. Therefore, the sum of the oxidation states in Ca Br₂(aq) is -1 + (-2) + 2(+1) = 0. Since the compound is neutral, the oxidation state of Ca must be the negative sum of the other oxidation states, which is +2. Therefore, the correct answer is B.

Quiz 9: Introduction to Solutions and Aqueous Reactions

Determine the oxidation state of nitrogen in RbNO₂.

A solution is prepared by adding 1.50 g of solid NaCl to 50.0 mL of 0.100 M .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

When 220.mL of 1.50 × 10^-4M hydrochloric acid is added to 135 mL of 1.75 × 10^-4 M Mg(OH) ₂,the resulting solution will be

A solution is prepared by mixing 20.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl.What is the molarity of chloride ion in this solution?

Determine the oxidation state of Ti in Ti(SO₄) ₂.

What is the oxidation number of the oxygen atom in O₂^2-?

How many milliliters of 0.188 M solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

What is the molarity of a NaOH solution if 39.1 mL of a 0.112 M solution is required to neutralize a 25.0-mL sample of the NaOH solution?

Identify the oxidation state of H in H₂(g) . Mg(s) + 2H Br(aq) → Mg Br₂(aq) + H₂(g)

What is the oxidation number of the chromium atom in Na₂CrO₄?

Which of the following is an oxidation-reduction reaction?

What is the oxidation number change for the manganese atom in the following unbalanced reduction half reaction?

Identify the oxidation state of H in H F(aq) . Ca(s) + 2H F(aq) → Ca F₂(aq) + H₂(g)

In an acid-base neutralization reaction 23.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H₂SO₄ solution?

Identify the oxidation state of Ca in Ca(s) . Ca(s) + 2H F(aq) → Ca F₂(aq) + H₂(g)

Determine the oxidation state of fluorine in F₂.

Determine the oxidation state of S in K₂SO₄.

Determine the oxidation state of nitrogen in NaNO₃.

What is the oxidation number of the sulfur atom in Li₂SO₄?

Identify the oxidation state of Ca in Ca Br₂(aq) . Ca(s) + 2H Br(aq) → Ca Br₂(aq) + H₂(g)

Quiz 9: Introduction to Solutions and Aqueous Reactions

Determine the oxidation state of nitrogen in RbNO2.

A solution is prepared by adding 1.50 g of solid NaCl to 50.0 mL of 0.100 M .What is the molarity of chloride ion in the final solution? Assume that the volume of the final solution is 50.0 mL.

When 220.mL of 1.50 × 10-4 M hydrochloric acid is added to 135 mL of 1.75 × 10-4 M Mg(OH) 2,the resulting solution will be

A solution is prepared by mixing 20.0 mL of 0.100 M HCl and 5.00 mL of 0.200 M NaCl.What is the molarity of chloride ion in this solution?

Determine the oxidation state of Ti in Ti(SO4) 2.

What is the oxidation number of the oxygen atom in O22-?

How many milliliters of 0.188 M solution are needed to neutralize 50.00 mL of 0.0789 M NaOH?

What is the molarity of a NaOH solution if 39.1 mL of a 0.112 M solution is required to neutralize a 25.0-mL sample of the NaOH solution?

Identify the oxidation state of H in H2(g) . Mg(s) + 2H Br(aq) → Mg Br2(aq) + H2(g)

What is the oxidation number of the chromium atom in Na2CrO4 ?

Which of the following is an oxidation-reduction reaction?

What is the oxidation number change for the manganese atom in the following unbalanced reduction half reaction?

Identify the oxidation state of H in H F(aq) . Ca(s) + 2H F(aq) → Ca F2(aq) + H2(g)

In an acid-base neutralization reaction 23.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H2SO4 solution?

Identify the oxidation state of Ca in Ca(s) . Ca(s) + 2H F(aq) → Ca F2(aq) + H2(g)

Determine the oxidation state of fluorine in F2.

Determine the oxidation state of S in K2SO4.

Determine the oxidation state of nitrogen in NaNO3.

What is the oxidation number of the sulfur atom in Li2SO4 ?

Identify the oxidation state of Ca in Ca Br2(aq) . Ca(s) + 2H Br(aq) → Ca Br2(aq) + H2(g)

Determine the oxidation state of nitrogen in RbNO₂.

When 220.mL of 1.50 × 10^-4M hydrochloric acid is added to 135 mL of 1.75 × 10^-4 M Mg(OH) ₂,the resulting solution will be

Determine the oxidation state of Ti in Ti(SO₄) ₂.

What is the oxidation number of the oxygen atom in O₂^2-?

Identify the oxidation state of H in H₂(g) . Mg(s) + 2H Br(aq) → Mg Br₂(aq) + H₂(g)

What is the oxidation number of the chromium atom in Na₂CrO₄?

Identify the oxidation state of H in H F(aq) . Ca(s) + 2H F(aq) → Ca F₂(aq) + H₂(g)

In an acid-base neutralization reaction 23.74 mL of 0.500 M potassium hydroxide reacts with 50.00 mL of sulfuric acid solution.What is the concentration of the H₂SO₄ solution?

Identify the oxidation state of Ca in Ca(s) . Ca(s) + 2H F(aq) → Ca F₂(aq) + H₂(g)

Determine the oxidation state of fluorine in F₂.

Determine the oxidation state of S in K₂SO₄.

Determine the oxidation state of nitrogen in NaNO₃.

What is the oxidation number of the sulfur atom in Li₂SO₄?

Identify the oxidation state of Ca in Ca Br₂(aq) . Ca(s) + 2H Br(aq) → Ca Br₂(aq) + H₂(g)