Show the correct FORMULA (not name) of a compound or ion when requested. Ion for

Question

Show the correct FORMULA (not name) of a compound or ion when requested. Ion formula must have correct charge. All questions refer to the redox titration. Show ALL calculations as necessary.  

1. A sample weighing 2.066 grams is 79.00 % iron (II). How many milliliters of 0.01166 M potassium permanganate will be required to titrate this sample? Show ALL your work and CLEARLY indicate your answer.   

2. A sample weighing 1.2010 grams, and containing an unknown amount of iron (II), is titrated with a permanganate ion solution. It requires 46.20 mL of the solution to titrate the sample. The concentration of the permanganate is 0.02001 M. Answer the following questions. Show all your work and CLEARLY indicate your final answer.

a. How many moles of permanganate are consumed in the reaction?

b. How many moles of iron (II) were present in the sample?

c. How many grams of iron (II) were present in the sample?

d. What is the mass % of iron in the sample ?
3.         Show the complete, properly balanced redox reaction of Fe2+ with permanganate ion under acidic conditions, as performed in It is NOT necessary to show the individual balanced halfreactions, just the final, balanced reaction.

4. The following short questions require little or no calculation. All questions refer to the redox titration, expt. 30.

a. How many moles of permanganate would be required to react with 10 moles of Fe2+ ?     ____________________

b. In this experiment, the element which is oxidized is ________________ .

c. In this experiment, the element which is reduced is _________________.

d. A sample of iron reacts with 0.00153 moles of permanganate ion. How many moles of iron are in the sample ? _________________________ .

e. How many grams of iron are in the sample described in part d ?   _________.

f.   The charge on iron after the reaction is ________.

g. The oxidation number of manganese before the reaction is ______________.

Explanation / Answer

Answer:

Fe+2 + KMnO4 Fe(MnO4)2 + K+

Given:

1.20 grams of Fe+2 is titrated with 46.2 ml of KMnO4

Thus 2.066 grams of Fe+3 will be titrated with--

(2.066*46.2)/1.20

=79.5 ml of KMnO4 required.

a).0.0116 moles.

b) & c). 2.066/56=

d).79%

3).

Fe+2 + KMnO4 Fe(MnO4)2 + K+

Mn-is reduced in this reaction.

The oxidation number of manganese before the reaction is __+7

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