Question

In: Chemistry

Write the balanced equation in ACID solution for the reaction below: Fe2++MnO-4→Fe3++Mn2+

 

a. Write the balanced equation in ACID solution for the reaction below:

Fe2++MnO-4→Fe3++Mn2+

b. To standardize a potassium permanganate solution (purple in appearance), a 0.250 g sample of FAS (iron II ammonium sulfate hexahydrate; molar mass = 342 g/mol) is dissolved in 25.00 mL distilled water, then acidified with sulfuric acid. The solution is then titrated with 35.00 mL potassium permanganate solution from a buret until a pale persistent purple color is attained. Calculate the molarity of the potassium permanganate solution.

c. What would be the effect, if any, on the value of the reported standard molarity of the potassium permanganate if the following errors were made? Explain each of your 3 answers.

1.Some drops of water remained in the buret after cleaning but before the permanganate solution was added to the buret.

2.The student neglected to run some permanganate solution through the tip of the buret before taking the initial reading.

3.The student’s lab partner spilled some FAS after weighing it but before titration.

Solutions

Expert Solution

(a)

5Fe2+ + MnO4- + 8H+ ----------------->   5 Fe3+ + Mn2+ + 4H₂O

(b)

Mass of FAS = 0.250 g

Molar mass of FAS= 342 g

Volume of water =25.0 mL

Volume of potassium permanganate solution =35.00 mL

MnO4- + 5Fe2+ + 8H+ ------------> Mn2+ + 5Fe3+ + 4H2O     

By using reaction stoichiometry we find mole ratio between Fe2+ and MnO4-

And mole ratio of Fe2+ : MnO4-   is 5:1

Number of moles of FAS = Fe2+

And number of moles of KMnO4 = MnO4-

moles of FAS = Mass of FAS / Molar mass of FAS

                       = 0.250 g / 342 g per mol

                       = 0.000731 mol FAS

moles of KMnO4 = 0.000731 mol FAS * 1 mol KMnO4 / 5 mol FAS

                            = 0.0001462 mol KMnO4

Molarity of KMnO4 = moles of KMnO4 / Volume in L

The volume is total volume = Volume of water + volume of KMnO4

                                              = 25.00 mL + 35.00 mL = 60.00 mL

= 0.060 L

Molarity of KMnO4 = 0.0001462 mol KMnO4 / 0.060 L

                               = 0.00244 M

Molarity of KMnO4 = 0.00244 M

c)

1) molarity decreases. because volume of permanganate solution increases.

2) molarity decreases

3) molarity increases


Related Solutions

Derive a balanced equation for the reaction occurring in the cell: Fe(s)|Fe2+(aq)||Fe3+(aq),Fe2+(aq)|Pt(s) a.) If E?cell =...
Derive a balanced equation for the reaction occurring in the cell: Fe(s)|Fe2+(aq)||Fe3+(aq),Fe2+(aq)|Pt(s) a.) If E?cell = 1.21 V, calculate ?G? for the reaction. b.) If E?cell=1.21V, calculate the equilibrium constant for the reaction. c.) Use the Nernst equation to determine the potential for the cell: Fe(s)|Fe2+(aq,1.0�10-3M)||Fe3+(aq,1.0�10-3M),Fe2+(aq,0.10M)|Pt(s)
Write the balanced molecular equation and net ionic equation for the neutralization reaction between hydrochloric acid...
Write the balanced molecular equation and net ionic equation for the neutralization reaction between hydrochloric acid and strontium hydroxide. Include the phase of each species.
Write a balanced ionic equation for 1) the first acid-base reaction of maleic acid and sodium...
Write a balanced ionic equation for 1) the first acid-base reaction of maleic acid and sodium hydroxide, 2) the second acid-base reaction between C4H3O4-and sodium hydroxide. Finally 3) add the two equations together and cancel out spectator ions to get a net ionic reaction.
write the balanced net ionic equation for the reaction that occurs Classify as a strong acid/strong...
write the balanced net ionic equation for the reaction that occurs Classify as a strong acid/strong base weak acid/strong base strong acid/weak base weak base/weak base extent of reaction - below 50 50 percent above 50 100 percent when ammonium bromide and calcium hydroxide are combined. acetic acid and calcium hydroxide when perchloric acid and ammonia are combined.
a)Write a balanced equation for the reaction of hydrochloric acid with sodium hydrogen carbonate (aka sodium...
a)Write a balanced equation for the reaction of hydrochloric acid with sodium hydrogen carbonate (aka sodium bicarbonate). b)How many milliliters of 0.225 M sodium bicarbonate are needed to neutralize 12.0 mL of 0.20 M HCl? Refer to the equation you wrote above.
Write the balanced NET IONIC equation for the reaction that occurs when nitrous acid and potassium...
Write the balanced NET IONIC equation for the reaction that occurs when nitrous acid and potassium hydroxide are combined. The extent of this reaction is: . This reaction is classified as . A. Strong Acid + Strong Base B. Weak Acid + Strong Base C. Strong Acid + Weak Base D. Weak Acid + Weak Base A. ... Below 50% B. ... 50% C. ... Above 50% D. ... 100% Submit Answer Retry Entire Group
For each reaction write a balanced chemical equation and then below the chemical formula of each...
For each reaction write a balanced chemical equation and then below the chemical formula of each reactant and product write a brief description of the substance (color and physical state). Also, indicate whether the reaction is exothermic, endothermic, or cannot tell. 1. Combination Reaction Equation: Exothermic                  Endothermic                Cannot tell Evidence of Chemical Change: 2. Reversible Decomposition--Combination Reactions Dehydration of Blue Vitrol (Copper(II) Sulfate Pentahydrate) Equation: CuSO4·5H2O ® CuSO4 + 5H2O Exothermic                 Endothermic                Cannot tell Evidence of Chemical Change: Rehydration...
Part A Write balanced molecular equation for the reaction between nitric acid and calcium hydroxide. Part...
Part A Write balanced molecular equation for the reaction between nitric acid and calcium hydroxide. Part B Enter a net ionic equation for the reaction between nitric acid and calcium hydroxide.
write a balanced net ionic equation for the reaction between barium hydroxide and phosphoric acid (H3PO4)...
write a balanced net ionic equation for the reaction between barium hydroxide and phosphoric acid (H3PO4) in water
In a particular redox reaction, MnO2 is oxidized to MnO4– and Fe3 is reduced to Fe2...
In a particular redox reaction, MnO2 is oxidized to MnO4– and Fe3 is reduced to Fe2 . Complete and balance the equation for this reaction in acidic solution. Phases are optional.
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT