Question

Can someone give me a table of Factors of KMnO4, FAS, etc. to be used in Redox Titration computations? (this is Quantitative Chemistry)

Answer 1

factors? what do you mean

Answer 2

for example:
A sol'n of KMnO4 contains 2.608g of KMnO4 in 750ml. Calculate the normality.

in getting the Normality of KMnO4 sol'n:
N = (wt. of sample/milliequivalent weight)/volume of sol'n
\[=\frac{ 2.608g }{ \frac{ 158.04g/mol }{ ? }\times1000 }\ \div750ml\]

***the factor there is the one with question mark...

Answer 3

sorry i was looking stuff, i haven't used normality in a while and there was no real emphasis on it when we did it. So basically you wanna "normalize/standardize" a concentration

so from what i gathered, N =( 2.608g/158.04g/mol )/ 0.75 L

which is the same as molarity in this case, but it changes when when you're using it in a reaction, and so comparing between 2 concentrations.

Answer 4

http://faculty.chemeketa.edu/lemme/CH%20122/handouts/normality.pdf read this

Answer 5

in normality you're going to use equivalent wt.

Answer 6

do you do titrations in the lab?

Answer 7

by equivalent weight the mean the amount of mass that would equal the amount of moles when comparing one substance to another. so the mass of HCl that equals 1 N, will be equivalent to the mass oh H2SO4 that equals 0.5 N

Answer 8

not currently, but yes, i have done quite a few

Answer 9

im not using moles since it's quantitative chemistry, i use normality.. it is advisable to use moles in qualitative chemistry

Answer 10

do you have a table of solutions used in redox titration with there valence?

Answer 11

well you CAN you use moles in quantitative chemistry, i have. Normality just makes things easier in terms of weight.

I don't have a table, what do you mean by valence?

Answer 12

i think what you're looking for is into how many parts does per say KMnO4 dissociate,

KMnO4 -> K+ + MnO4-

FAS -> 2NH4+ + 2SO4- + Fe2+