Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: AshleyMorgan91 on October 12, 2014, 06:36:49 PM
-
Hey guys, I'm new to this site and I've decided to join because I need some assistance with my chem work. It's a titration question and it reads:
25.0 cm3 of the aqueous solution of M requires 24.80 cm3 of 0.02 moldm -3 permangante for complete reaction. The equation for the reaction is
5 Fe 2+ (aq) + MnO4 - (aq) + 8H+ (aq) ---> 5 Fe 3+ (aq) + Mn2+ (aq) + 4 H2O
Calculate the following:
The no. of moles Fe 2+ in the 25.0 cm3 of aqueous M
The no. of moles Fe 2+ in 1.0 dm3 of M (aq)
The mass of Fe 2+ in 1 dm3 of M (aq)
The % Fe 2+ in the compound [The mass conc. of M is 40.90 g dm-3]
Please help me and explain how you arrive at the answer. Thanks in advance.
-
See forum rules, try to solve by yourself and explain what is not clear, then help will be given. Show your calculations.
1. Calculate the moles in your Permanganate
2. How does it correspond to iron (see equation)
The rest should be clear.