1. Write the balanced net ionic equation for the reaction between MnO4" ion and Fe2+ ion in acid solution. 2. How many moles of Fe2* ion can be oxidized by 1.2 x 10-2 moles MnO4 ion in the reaction in Question 1?
1. Write the balanced net ionic equation for the reaction between MnO4" ion and Fe2+ ion in acid solution. 2. How many moles of Fe2* ion can be oxidized by 1.2 x 10-2 moles MnO4 ion in the reaction in Question 1?
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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How many moles of Fe^2+ ion can be oxidized by 1.2 ×10^-2 moles MnO4 ion in the reaction between MnO4 ion and Fe^2+
Transcribed Image Text:lab, complete items a, b, c, and d (title, purpose, chemicals and
equipment, and summary of procedure) as described on page 10 of Exp. 1 on an
8 1/2 x 11 sheet of paper.
Answer the following questions on 8 1/2 x 11 sheet of paper or in your laboratory
notebook if one is required by your instructor:
1. Write the balanced net ionic equation for the reaction between MnO4 ion and
Fe2+ ion in acid solution.
2. How many moles of Fe2+ ion can be oxidized by 1.2 x 10-2 moles MnO4 ion in the
reaction in Question 1?
3. A solid sample containing some Fe2* ion weighs 1.923 g. It requires 36.44 mL
0.0244 M KMNO4 to titrate the Fe2* in the dissolved sample to a pink end point.
a. How many moles MnO4 ion are required?
b. How many moles Fe2* are there in the sample?
C. How many grams of iron are there in the sample?
d. What is the percentage of Fe in the sample?
Lab Activities:
Go over the sample calculations and prelab questions with your lab instructor
• Complete lab and fill in data sheet for the Standardization of Potassium
Permanganate. The next data sheet, Percent Iron in Unknown Sample will be
completed the following lab period.
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