Question 1

What is true when the following equation is balanced in basic solution? P(s)+ PO₄^3-(aq)→ HPO₃^2-(aq)

Accepted Answer

The answer of What is true when the following equation...

Question 2

What are the coefficients in front of Fe(s)and O₃(g)when the following equation is balanced in a basic solution? _____ Fe(s)+ _____ O₃(g)→ _____ Fe₂O₃(s)+ _____ O₂(g)

Accepted Answer

The answer of What are the coefficients in front of...

Question 3

What is the reduction half reaction for the following chemical reaction in a basic solution? Mn²⁺(aq)+ 2 ClO₃^-(aq)+ OH^-(aq)→ MnO₂(s)+ 2 ClO₂(aq)+ H₂O(l)

Accepted Answer

The answer of What is the reduction half reaction for...

Question 4

Determine the number of water molecules necessary to balance the reduction half reaction of ____ MnO₄^-(aq)→ ____ MnO₂(s)that occurs in a basic solution.

Accepted Answer

The answer of Determine the number of water molecules necessary...

Question 5

Determine the number of water molecules necessary to balance the reduction half reaction of ____ MnO₄^-(aq)→ ____ Mn²⁺(aq)that occurs in an acidic solution.

Accepted Answer

The answer of Determine the number of water molecules necessary...

Question 6

What are the coefficients in front of NO₃^-(aq)and Cu(s)when the following redox equation is balanced in an acidic solution: _____ NO₃^-(aq)+ _____ Cu(s)→ _____ NO(g)+ _____ Cu²⁺(aq)?

Accepted Answer

First, we write out the half-reactions: NO₃^-(aq) -> NO(g) Cu(s) -> Cu²⁺(aq) Next, we balance the atoms that are not hydrogen or oxygen. For the reduction half-reaction: N: 1 on both sides O: 13 on the left, 1 on the right (add H2O to balance) S: 1 on both sides P: 1 on both sides For the oxidation half-reaction: Cu: 1 on both sides S: 1 on both sides P: 12 on the left, 1 on the right (add H+ and e- to balance) Now we balance the hydrogen and oxygen atoms by adding H+ and H2O as needed: Reduction: 13 H2O + 13 e- + NO₃^-(aq) -> 13 H+ + 13 NO(g) Oxidation: Cu(s) -> Cu²⁺(aq) + 2 H+ + 2 e- Finally, we multiply the two half-reactions by coefficients so that the number of electrons lost in the oxidation half-reaction is equal to the number of electrons gained in the reduction half-reaction: Reduction: 13 H2O + 13 e- + NO₃^-(aq) -> 13 H+ + 13 NO(g) Oxidation: 2 Cu(s) -> 2 Cu²⁺(aq) + 24 H+ + 24 e- Now we can add the two half-reactions together and cancel out common species: 13 H2O + NO₃^-(aq) + 2 Cu(s) -> 13 H+ + 13 NO(g) + 2 Cu²⁺(aq) The coefficients in front of NO₃^-(aq) and Cu(s) are therefore 2 and 3, respectively. The correct answer is A.

Question 7

In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent? C₂O₄2- (aq)+ MnO₄^-(aq)→ CO₂(aq)+ Mn²⁺(aq)

Accepted Answer

In the balanced equation, you can see that 2 moles of electrons are transferred per mole of reducing agent (CS2O2-). This is because the coefficient in front of CS2O2- is 2, indicating that 2 moles of CS2O2- are needed to react with 1 mole of MnO4-. During the reaction, each CS2O2- molecule loses 2 electrons to form CO2, while each MnO4- molecule gains 5 electrons to form Mn2+. Therefore, the ratio of mole of electrons to mole of CS2O2- is 2:1, or 2 moles of electrons per mole of CS2O2-.

Question 8

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃₍_aq₎ is needed to completely react with 12.44 mL of 0.125 M KI₃(aq)? 2 S₂O₃^2-(aq)+ I₃^-(aq)→ S₄O₆^2-(aq)+ 3 I^-(aq)

Accepted Answer

First, use the balanced chemical equation to determine the mole ratio between KI and Na2S2O3:

1 mol KI reacts with 2 mol Na2S2O3

Then, use the concentration and volume of KI to calculate the number of moles present:

moles KI = concentration x volume = 0.125 M x 12.44 mL x (1 L / 1000 mL) = 0.001555 mol

Finally, use the mole ratio to determine the volume of Na2S2O3 needed:

moles Na2S2O3 = (0.001555 mol KI) x (2 mol Na2S2O3 / 1 mol KI) = 0.00311 mol

volume Na2S2O3 = moles / concentration = 0.00311 mol / 0.250 M = 0.0124 L = 12.4 mL

Therefore, the best choice is C, 12.4 mL.

Question 9

What is the oxidation half reaction in the following chemical reaction? Cr₂O₇^2-(aq)+ 6 Cl^-(aq)+ 14 H⁺(aq)→ 2 Cr³⁺(aq)+ 3 Cl₂(aq)+ 7 H₂O(l)

Accepted Answer

The answer of What is the oxidation half reaction in...

Question 10

Determine the number of water molecules necessary to balance the reduction half reaction of ____ ClO₃^-(aq)→ ____ Cl^- (aq)that occurs in an acidic solution.

Accepted Answer

In order to balance the reduction half reaction, we need to add 3 electrons to the reactant side to form Cl^- (aq). Each oxygen atom in ClO₃^-(aq) gains two electrons and two hydrogen ions to become two water molecules. Therefore, we need a total of 3 water molecules to balance the reduction half reaction.

Question 11

Determine the number of water molecules necessary to balance the following chemical equation. Cr₂O₇^2-(aq)+ Cl^-(aq)+ H⁺(aq)→ Cr³⁺(aq)+ Cl₂(g)+ _____ H₂O(l)

Accepted Answer

Looking at the balanced equation: Cr₂O₇^2-(aq)+ Cl^-(aq)+ H⁺(aq)→ Cr³⁺(aq)+ Cl₂(g)+ _____ H₂O(l) We can see that there is only one oxygen molecule on the reactant side, compared to two on the product side. Therefore, we need to balance this with a water molecule. Also, we can see that there are 17 sulfur atoms on the reactant side, but only 12 on the product side. We can balance this by adding 5 water molecules, which also balances the hydrogen atoms. Therefore, the answer is C) 7.

Question 12

According to the balanced equation shown below,1.00 mole of oxalic acid,H₂C₂O₄,reacts with ________ moles of permanganate ion,MnO₄^-. 5 H₂C₂O₄(aq)+ 2 MnO₄^-(aq)+ 6 H⁺(aq)→ 10 CO₂(g)+ 2 Mn²⁺(aq)+ 8 H₂O(l)

Accepted Answer

The answer of According to the balanced equation shown below,1.00...

Question 13

According to the balanced chemical equation 5 H₂C₂O₄(aq)+ 2 MnO₄^-(aq)+ 6 H⁺(aq)→ 10 CO₂(g)+ 2 Mn²⁺(aq)+ 8 H₂O(l) 0)3500 grams of oxalic acid,H₂C₂O₄ will react with ________ mL of 0.100 M potassium permanganate,KMnO₄ solution.

Accepted Answer

The answer of According to the balanced chemical equation 5 H₂C₂O₄(aq)+...

Question 14

What are the coefficients in front of NO₃^-(aq)and Zn(s)when the following equation is balanced in a basic solution? _____ NO₃^-(aq)+ _____ Zn(s)→ _____ Zn²⁺(aq)+ _____ NO(g)

Accepted Answer

The coefficients in front of NO₃^-(aq) and Zn(s) are 2 and 3, respectively, when the equation is balanced in a basic solution.

Question 15

Which elements will not react with liquid water or with aqueous H⁺ ions?

Accepted Answer

The elements Ag (silver), Au (gold), Hg (mercury), and Pt (platinum) are all classified as noble metals and are known for their low reactivity. They will not react with liquid water or with aqueous H⁺ ions.

Question 16

According to the balanced chemical equation 5 H₂C₂O₄(aq)+ 2 MnO₄^-(aq)+ 6 H⁺(aq)→ 10 CO₂(g)+ 2 Mn²⁺(aq)+ 8 H₂O(l) 0)3500 grams of oxalic acid,H₂C₂O₄ will react with ________ moles of permanganate,MnO₄^-.

Accepted Answer

3500 grams of oxalic acid, H2C2O4 will react with 0.001554 moles of permanganate, MnO4-.To determine the number of moles of permanganate required, we can use the stoichiometry of the balanced chemical equation:5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l)From the equation, we can see that 5 moles of oxalic acid react with 2 moles of permanganate. Therefore, the number of moles of permanganate required to react with 3500 grams of oxalic acid can be calculated as follows:Moles of oxalic acid = 3500 g / 90.03 g/mol = 38.87 molMoles of permanganate required = (38.87 mol oxalic acid) x (2 mol permanganate / 5 mol oxalic acid) = 0.001554 molTherefore, the correct answer is A) 0.001554.

Question 17

What is the oxidation half reaction in the following chemical reaction? Zn(s)+ 2 H⁺(aq)→ Zn²⁺(aq)+ H₂(g)

Accepted Answer

The oxidation half reaction involves the loss of electrons. In this reaction, Zn(s) loses 2 electrons to form ZnS1U1P12. Therefore, the correct choice is A: Zn(s) → ZnS1U1P12 + S1S1P0(aq) + 2eS1U1P1- S1S1P0.

Question 18

What is the reduction half reaction for the following chemical reaction in a basic solution? ClO^-(aq)+ Cr(OH)₄^-(aq)→ CrO₄^2-(aq)+ Cl^-(aq)

Accepted Answer

The first step to determining the reduction half reaction is to identify which species is being reduced. In this case, we can see that chromium (Cr) is going from a +3 oxidation state to a +2 oxidation state, which means it is gaining electrons and being reduced. Therefore, the reduction half reaction should involve the Cr species.

Next, we need to balance the charges and add water molecules to balance the oxygen atoms. The balanced reduction half reaction is:

Cr(OH)4^- + 6e^- → Cr(OH)2 + 4OH^-

However, the question asks for the reduction half reaction in a basic solution, so we need to add enough hydroxide ions (OH^-) to balance out the hydrogen ions (H+) on the other side of the equation. In this case, we need to add 4 more OH^- ions to both sides of the equation:

Cr(OH)4^- + 10e^- + 4OH^- → Cr(OH)2 + 6OH^-

This final equation matches option B.

Question 19

What are the coefficients in front of BrO₃^-(aq)and Br^-(aq)when the following equation is balanced in an acidic solution? _____ BrO₃^-(aq)+ _____ Br^-(aq)→ _____ Br₂(aq)

Accepted Answer

The answer of What are the coefficients in front of...

Question 20

What is the molarity of a potassium triiodide solution,KI₃(aq),if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.200 M thiosulfate solution,Na₂S₂O₃(aq)? The chemical equation for the reaction is: 2 S₂O₃^2-(aq)+ I₃^-(aq)→ S₄O₆^2-(aq)+ 3 I^-(aq)

Accepted Answer

The balanced chemical equation is:2 S₂O₃^2-(aq)+ I₃^-(aq)→ S₄O₆^2-(aq)+ 3 I^-(aq)From the stoichiometry of the balanced chemical equation, we can see that 2 moles of S₂O₃^2- react with 1 mole of I₃^-. Therefore, the number of moles of I₃^- in 30.00 mL of the KI₃ solution is:$$moles\ of\ I_3^- = (25.00\ mL)(0.200\ M) imes \frac{1\ mol\ I_3^-}{2\ mol\ S_2O_3^{2-}} = 2.500 imes 10^{-3}\ mol$$The molarity of the KI₃ solution is:$$Molarity\ of\ KI_3 = \frac{moles\ of\ I_3^-}{volume\ of\ solution\ in\ liters} = \frac{2.500 imes 10^{-3}\ mol}{30.00 imes 10^{-3}\ L} = 0.0833\ M$$Therefore, the correct choice is A) 0.0833 M.

Quiz 4: Reactions in Aqueous Solutions

What is true when the following equation is balanced in basic solution? P(s) + PO₄^3-(aq) → HPO₃^2-(aq)

What are the coefficients in front of Fe(s) and O₃(g) when the following equation is balanced in a basic solution? ___ Fe(s) + _ O₃(g) → _ Fe₂O₃(s) + ___ O₂(g)

What is the reduction half reaction for the following chemical reaction in a basic solution? Mn²⁺(aq) + 2 ClO₃^-(aq) + OH^-(aq) → MnO₂(s) + 2 ClO₂(aq) + H₂O(l)

Determine the number of water molecules necessary to balance the reduction half reaction of MnO₄^-(aq) → MnO₂(s) that occurs in a basic solution.

Determine the number of water molecules necessary to balance the reduction half reaction of MnO₄^-(aq) → Mn²⁺(aq) that occurs in an acidic solution.

What are the coefficients in front of NO₃^-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution: ___ NO₃^-(aq) + _ Cu(s) → _ NO(g) + ___ Cu²⁺(aq) ?

In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent? C₂O₄2- (aq) + MnO₄^-(aq) → CO₂(aq) + Mn²⁺(aq)

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃₍_aq₎ is needed to completely react with 12.44 mL of 0.125 M KI₃(aq) ? 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)

What is the oxidation half reaction in the following chemical reaction? Cr₂O₇^2-(aq) + 6 Cl^-(aq) + 14 H⁺(aq) → 2 Cr³⁺(aq) + 3 Cl₂(aq) + 7 H₂O(l)

Determine the number of water molecules necessary to balance the reduction half reaction of ClO₃^-(aq) → Cl^- (aq) that occurs in an acidic solution.

Determine the number of water molecules necessary to balance the following chemical equation. Cr₂O₇^2-(aq) + Cl^-(aq) + H⁺(aq) → Cr³⁺(aq) + Cl₂(g) + _____ H₂O(l)

According to the balanced equation shown below,1.00 mole of oxalic acid,H₂C₂O₄,reacts with ________ moles of permanganate ion,MnO₄^-. 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l)

According to the balanced chemical equation 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l) 0) 3500 grams of oxalic acid,H₂C₂O₄ will react with ________ mL of 0.100 M potassium permanganate,KMnO₄ solution.

What are the coefficients in front of NO₃^-(aq) and Zn(s) when the following equation is balanced in a basic solution? ___ NO₃^-(aq) + _ Zn(s) → _ Zn²⁺(aq) + ___ NO(g)

Which elements will not react with liquid water or with aqueous H⁺ ions?

According to the balanced chemical equation 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l) 0) 3500 grams of oxalic acid,H₂C₂O₄ will react with ________ moles of permanganate,MnO₄^-.

What is the oxidation half reaction in the following chemical reaction? Zn(s) + 2 H⁺(aq) → Zn²⁺(aq) + H₂(g)

What is the reduction half reaction for the following chemical reaction in a basic solution? ClO^-(aq) + Cr(OH) ₄^-(aq) → CrO₄^2-(aq) + Cl^-(aq)

What are the coefficients in front of BrO₃^-(aq) and Br^-(aq) when the following equation is balanced in an acidic solution? ___ BrO₃^-(aq) + _ Br^-(aq) → ___ Br₂(aq)

What is the molarity of a potassium triiodide solution,KI₃(aq) ,if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.200 M thiosulfate solution,Na₂S₂O₃(aq) ? The chemical equation for the reaction is: 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)

Quiz 4: Reactions in Aqueous Solutions

What is true when the following equation is balanced in basic solution? P(s) + PO43-(aq) → HPO32-(aq)

What are the coefficients in front of Fe(s) and O3(g) when the following equation is balanced in a basic solution? _____ Fe(s) + _____ O3(g) → _____ Fe2O3(s) + _____ O2(g)

What is the reduction half reaction for the following chemical reaction in a basic solution? Mn2+(aq) + 2 ClO3-(aq) + OH-(aq) → MnO2(s) + 2 ClO2(aq) + H2O(l)

Determine the number of water molecules necessary to balance the reduction half reaction of ____ MnO4-(aq) → ____ MnO2(s) that occurs in a basic solution.

Determine the number of water molecules necessary to balance the reduction half reaction of ____ MnO4-(aq) → ____ Mn2+(aq) that occurs in an acidic solution.

What are the coefficients in front of NO3-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution: _____ NO3-(aq) + _____ Cu(s) → _____ NO(g) + _____ Cu2+(aq) ?

In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent? C2O42- (aq) + MnO4-(aq) → CO2(aq) + Mn2+(aq)

Based on the balanced chemical equation shown below,what volume of 0.250 M K2S2O3(aq) is needed to completely react with 12.44 mL of 0.125 M KI3(aq) ? 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq)

What is the oxidation half reaction in the following chemical reaction? Cr2O72-(aq) + 6 Cl-(aq) + 14 H+(aq) → 2 Cr3+(aq) + 3 Cl2(aq) + 7 H2O(l)

Determine the number of water molecules necessary to balance the reduction half reaction of ____ ClO3-(aq) → ____ Cl- (aq) that occurs in an acidic solution.

Determine the number of water molecules necessary to balance the following chemical equation. Cr2O72-(aq) + Cl-(aq) + H+(aq) → Cr3+(aq) + Cl2(g) + _____ H2O(l)

According to the balanced equation shown below,1.00 mole of oxalic acid,H2C2O4,reacts with ________ moles of permanganate ion,MnO4-. 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l)

According to the balanced chemical equation 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l) 0) 3500 grams of oxalic acid,H2C2O4 will react with ________ mL of 0.100 M potassium permanganate,KMnO4 solution.

What are the coefficients in front of NO3-(aq) and Zn(s) when the following equation is balanced in a basic solution? _____ NO3-(aq) + _____ Zn(s) → _____ Zn2+(aq) + _____ NO(g)

Which elements will not react with liquid water or with aqueous H+ ions?

According to the balanced chemical equation 5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l) 0) 3500 grams of oxalic acid,H2C2O4 will react with ________ moles of permanganate,MnO4-.

What is the oxidation half reaction in the following chemical reaction? Zn(s) + 2 H+(aq) → Zn2+(aq) + H2(g)

What is the reduction half reaction for the following chemical reaction in a basic solution? ClO-(aq) + Cr(OH) 4-(aq) → CrO42-(aq) + Cl-(aq)

What are the coefficients in front of BrO3-(aq) and Br-(aq) when the following equation is balanced in an acidic solution? _____ BrO3-(aq) + _____ Br-(aq) → _____ Br2(aq)

What is the molarity of a potassium triiodide solution,KI3(aq) ,if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.200 M thiosulfate solution,Na2S2O3(aq) ? The chemical equation for the reaction is: 2 S2O32-(aq) + I3-(aq) → S4O62-(aq) + 3 I-(aq)

What is true when the following equation is balanced in basic solution? P(s) + PO₄^3-(aq) → HPO₃^2-(aq)

What are the coefficients in front of Fe(s) and O₃(g) when the following equation is balanced in a basic solution? ___ Fe(s) + _ O₃(g) → _ Fe₂O₃(s) + ___ O₂(g)

What is the reduction half reaction for the following chemical reaction in a basic solution? Mn²⁺(aq) + 2 ClO₃^-(aq) + OH^-(aq) → MnO₂(s) + 2 ClO₂(aq) + H₂O(l)

Determine the number of water molecules necessary to balance the reduction half reaction of MnO₄^-(aq) → MnO₂(s) that occurs in a basic solution.

Determine the number of water molecules necessary to balance the reduction half reaction of MnO₄^-(aq) → Mn²⁺(aq) that occurs in an acidic solution.

What are the coefficients in front of NO₃^-(aq) and Cu(s) when the following redox equation is balanced in an acidic solution: ___ NO₃^-(aq) + _ Cu(s) → _ NO(g) + ___ Cu²⁺(aq) ?

In the unbalanced equation shown below how many moles of electrons are transferred per mole of reducing agent? C₂O₄2- (aq) + MnO₄^-(aq) → CO₂(aq) + Mn²⁺(aq)

Based on the balanced chemical equation shown below,what volume of 0.250 M K₂S₂O₃₍_aq₎ is needed to completely react with 12.44 mL of 0.125 M KI₃(aq) ? 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)

What is the oxidation half reaction in the following chemical reaction? Cr₂O₇^2-(aq) + 6 Cl^-(aq) + 14 H⁺(aq) → 2 Cr³⁺(aq) + 3 Cl₂(aq) + 7 H₂O(l)

Determine the number of water molecules necessary to balance the reduction half reaction of ClO₃^-(aq) → Cl^- (aq) that occurs in an acidic solution.

Determine the number of water molecules necessary to balance the following chemical equation. Cr₂O₇^2-(aq) + Cl^-(aq) + H⁺(aq) → Cr³⁺(aq) + Cl₂(g) + _____ H₂O(l)

According to the balanced equation shown below,1.00 mole of oxalic acid,H₂C₂O₄,reacts with ________ moles of permanganate ion,MnO₄^-. 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l)

According to the balanced chemical equation 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l) 0) 3500 grams of oxalic acid,H₂C₂O₄ will react with ________ mL of 0.100 M potassium permanganate,KMnO₄ solution.

What are the coefficients in front of NO₃^-(aq) and Zn(s) when the following equation is balanced in a basic solution? ___ NO₃^-(aq) + _ Zn(s) → _ Zn²⁺(aq) + ___ NO(g)

Which elements will not react with liquid water or with aqueous H⁺ ions?

According to the balanced chemical equation 5 H₂C₂O₄(aq) + 2 MnO₄^-(aq) + 6 H⁺(aq) → 10 CO₂(g) + 2 Mn²⁺(aq) + 8 H₂O(l) 0) 3500 grams of oxalic acid,H₂C₂O₄ will react with ________ moles of permanganate,MnO₄^-.

What is the oxidation half reaction in the following chemical reaction? Zn(s) + 2 H⁺(aq) → Zn²⁺(aq) + H₂(g)

What is the reduction half reaction for the following chemical reaction in a basic solution? ClO^-(aq) + Cr(OH) ₄^-(aq) → CrO₄^2-(aq) + Cl^-(aq)

What are the coefficients in front of BrO₃^-(aq) and Br^-(aq) when the following equation is balanced in an acidic solution? ___ BrO₃^-(aq) + _ Br^-(aq) → ___ Br₂(aq)

What is the molarity of a potassium triiodide solution,KI₃(aq) ,if 30.00 mL of the solution is required to completely react with 25.00 mL of a 0.200 M thiosulfate solution,Na₂S₂O₃(aq) ? The chemical equation for the reaction is: 2 S₂O₃^2-(aq) + I₃^-(aq) → S₄O₆^2-(aq) + 3 I^-(aq)