In acidic solution MnO4- oxidizes H3AsO3, a weak acid, to H3AsO4, a weak acid, and is reduced to Mn2+. Write the balanced net ionic equation for this reaction. How many H+ are there in the balanced equation

Question

In acidic solution MnO4- oxidizes H3AsO3, a weak acid, to H3AsO4, a weak acid, and is reduced to Mn2+. Write the balanced net ionic equation for this reaction. How many H+ are there in the balanced equation

Answer 1

In acidic solution MnO4- oxidizes H3AsO3, a weak acid, to H3AsO4, a weak acid, and is reduced to Mn2+. Write the balanced net ionic equation for this reaction. How many H+ are there in the balanced equation?

1
2
3
4
6

Question 2 4.2 points Save
What is the coefficient of NaCl in the balanced formula unit equation?
NaClO3 + H2O + I2 HIO3 + NaCl
1
2
3
4
5

Question 3 4.2 points Save
What is the molarity of a barium hydroxide solution if 18.62 mL of this Ba(OH)2 solution requires 35.84 mL of 0.2419 M HCl for titration to the equivalence point?
0.4656 M
0.2328 M
0.1164 M
0.3492 M
0.6984 M

Question 4 4.2 points Save
What mass of molybdenum(III) oxide, Mo2O3, will be completely oxidized to potassium molybdate, K2MoO4, by 35.0 mL of 0.200 M KMnO4?
3MnO4- + 5Mo3+ + 8H2O 3Mn2+ + 5MoO42- + 16 H+
8.40 g
4.20 g
1.40 g
2.80 g
6.40 g

Question 5 4.2 points Save
What volume of 0.230 M potassium hydroxide solution, KOH, would completely neutralize 27.4 mL of 0.205 M sulfurous acid solution, H2SO3?
61.5 mL
12.2 mL
24.4 mL
48.8 mL

Question 6 4.2 points Save
What volume of 0.50 M KOH would be required to neutralize completely 500. mL of 0.25 M HPO solution?
2.5 ´ 10 mL
1.4 ´ 10 mL
83 mL
7.5 ´ 102 mL
5.2 ´ 102 mL

Question 7 4.2 points Save
What volume of 0.0100 M KMnO4 solution is required to oxidize 42.5 mL of 0.0100 M FeSO4 sulfuric acid solution?
MnO4- + 8H+ + 5Fe2+ Mn2+ + 5Fe3+ + 4H2O
16.0 mL
8.5 mL
21.3 mL
80.0 mL
31.9 mL

Question 8 4.2 points Save
What is the oxidation number of arsenic in H2AsO4-2?
+1
+2
+3
+4
+5

Question 9 4.2 points Save
What volume of 0.0750 M Ba(OH) will completely react with 125 mL of 0.0350 M HCl?
29.2 mL
42.0 mL
230. mL
536 mL
53.6 mL

Question 10 4.2 points Save
Balance the following net ionic equation. Use H+ rather than H3O+. What is the sum of the coefficients?
H2O2 + Fe2+ Fe3+ (in acidic solution)
13
15
7
9
11

Question 11 4.2 points Save
How many mL of 0.57 M AgNO3 will completely react with 121 mL of 0.95 M NaBr?
AgNO3 + NaBr AgBr + NaNO3
72.6 mL
181 mL
202 mL
4.47 mL
0.202 mL

Question 12 4.2 points Save
Balance the following formula unit equation. What is the sum of all of the coefficients?
HNO3 + ZnS S + NO + Zn(NO3)2 + H2O
23
25
27
29
31

Question 13 4.2 points Save
Calculate the molarity of an HCl solution if 38.65 mL of this HCl solution is required to neutralize 0.2152 g of Na2CO3.
0.05251 M
0.02625 M
0.2104 M
0.05427 M
0.1050 M

Question 14 4.2 points Save
What is the molarity of a Na2Cr2O7 solution if 22.5 mL of it is required to oxidize 33.0 mL of 0.150 M Fe(NH4)2(SO4)? The reaction products include Cr3+ and Fe3+.
0.184 M
0.220 M
0.0367 M
0.0440 M
0.0660 M

Question 15 4.2 points Save
Which choice includes all of the following that are oxidation-reduction reactions and no others?

I. BaSO3(s) ® BaO(s) + SO2(g)
II. 2K(s) + Br2() ® 2KBr(s)
III. H2CO3(aq) + Ca(OH)2(aq) ® CaCO3(s) + 2H2O()
IV. SnS2(s) + HCl(aq) ® H2SnCl6(s) + 2H2S(aq)
V. 3Cl2(g) + 6KOH(aq) ® 5KCl(aq) + KClO3(aq) + 3H2O()

II, III, and IV
I and III
II and V
I and IV

Question 16 4.2 points Save
Balance the following equation. How many H+ are there in the balanced equation?
(COOH)2 + MnO4- + H+ CO2 + Mn2+ + H2O
6
2
3
4
8

Question 17 4.2 points Save
Balance the following net ionic equation. What is the coefficient of H2O?
MnO4- + Bi MnO2 + Bi(OH)3 (basic solution)
1
2
3
4
5

Question 18 4.2 points Save
What is the molarity of a sulfurous acid solution if 23.7 mL of this H2SO3 solution requires 16.8 mL of 0.296 M NaOH for titration to the equivalence point?
0.210 M
0.358 M
0.105 M
0.421 M
0.0525 M

Question 19 4.2 points Save
Unlike most other carboxylic acids, oxalic acid, H2C2O4, is readily oxidized, which makes it useful as a reducing agent in photography, bleaching, and ink removal. However, a high enough concentration of its solution must be maintained. A titration with potassium permanganate, KMnO4, is used for the oxalic acid assay. The net equation is:
5H2C2O4 + 2MnO4- + 6H+ ® 10CO2 + 2Mn2+ + 8H2O()

Calculate the molarity of a H2C2O4 solution requiring 27.3 mL of 0.115 M KMnO4 for a 25.0 mL sample of the solution.
0.126 M
0.314 M
0.263 M
0.0502 M

Question 20 4.2 points Save
How many H2O are there in the balanced equation?
CuS + NO3- + H+ Cu2+ + S + NO + H2O
one
two
three
four
five

Question 21 4.2 points Save
Based on the following equation (when balanced in acidic solution), the Br- ions lose how many electrons?
MnO4- + H+ + Br- Mn2+ + Br2 + H2O
5
8
10
2
16

Question 22 4.2 points Save
If 75.0 mL of 0.250 M HNO and 75.0 mL of 0.250 M KOH are mixed, what is the molarity of the salt in the resulting solution?
0.250 M
0.500 M
0.333 M
0.125 M
0.167 M

Question 23 4.2 points Save
Chlorous acid, HClO2, oxidizes sulfur dioxide, SO2, to sulfate ions, SO42-, and is reduced to chloride ions, Cl-, in acidic solution. Use H+ rather than H3O+. Write the balanced net ionic equation for the reaction. What is the sum of the coefficients?
11
13
15
17
19

Question 24 4.2 points Save
What is the molarity of a solution of FeSO4 if 25.06 mL of it reacts with 38.19 mL of 0.1214 M KMnO4?
MnO4- + 8H+ + 5Fe2+ Mn2+ + 5Fe3+ + 4H2O
0.1854 M
0.3992 M
0.07985 M
0.4267 M
0.9250 M

Question 25 4.2 points Save
Write the balanced net ionic half-reaction for the oxidation of H2O to O2 in acidic solution. What is the sum of the coefficients (including the electrons.)
11
5
9
7
15

Answer 2

This is not a site where you can dump all of your homework. If there is something you don't understand about balancing equations, post it (or them) and we can help you through the rough spots.

Answer 3

dont get how to solve question 3. could you help me?

Answer 4

To write the balanced net ionic equation for this reaction, we need to first write the balanced chemical equation for the oxidation-reduction reaction and then eliminate any spectator ions.

The chemical equation for the reaction is:

MnO4- + H3AsO3 + H+ -> Mn2+ + H3AsO4 + H2O

To balance the equation, follow these steps:

1. Balance the As by adding a coefficient of 3 in front of H3AsO3 and H3AsO4:

MnO4- + 3H3AsO3 + H+ -> Mn2+ + 3H3AsO4 + H2O

2. Balance the oxygen atoms by adding water molecules to the appropriate side:

MnO4- + 3H3AsO3 + H+ -> Mn2+ + 3H3AsO4 + 4H2O

3. Balance the hydrogen atoms by adding H+ ions to the opposite side:

MnO4- + 3H3AsO3 + 5H+ -> Mn2+ + 3H3AsO4 + 4H2O

Now that we have the balanced equation, we can determine the number of H+ ions in the balanced equation. Looking at the equation, we can see that there are:
- 1 H+ ion on the reactant side (left side)
- 5 H+ ions on the product side (right side)

Therefore, there are a total of 5 H+ ions in the balanced equation.