I am assuming that this FeCl3 is going to be aqueous, as it usually is. Therefore, Fe+3 forms complexes in water in the following manner:
B FeCl3(aq) +6H2O → [Fe(H2O)6]3+
Now, because the Fe has a positive charge, it will pull the negative electron cloud towards itself, making the bond holding the H on the OH weaker, which leads to an easier release of protons (H+). Therefore,
[Fe(H2O)6]3+ → [Fe(H2O)5]+2 + H+
As you can see, Fe is in the "net reaction" acting as an acid, as it makes the H2O's bound to it release H+ ions into the water. Therefore, FeCl3 is assigned a Ka value, which = 2.0 x 10-3.
Now, we need to set up our table:
FeCl3 →
Fe(H2O)5]+2
+
H+
Initial concentration
0.5 M
0.0 M
0.0 M
Change
(-) x
x
x
Final Concentration
0.5-x
x
x
So, we can set up our equilibrium constant expression:
Ka= [H+][ [Fe(H2O)5]+2]/[[Fe(H2O)6]3+]
we know Ka therefore:
2.0 x 10-3= x2/0.5-x
Solve for x, must use quadratic:
0.001-2.0 x 10-3x-x2=0
Solving the quadratic gives us:
x= -0.032639, 0.030639
The negative result is unphysical, because we cannot have a negative concentration, therefore, x= 0.030639, which from our graph tells us that the concentration of H+ = 0.030639M, so to find the pH:
-log( 0.030639)= pH = 1.51, so therefore, the pH of 0.5 M FeCl3 is 1.51.
Hope that helps, don't know if you needed to know all the details.
Praise God!
Eugene.
Wiki User
∙ 12y agohow to prepare .05M glutaraldhyde solution molecular weight is 100.12
Look up or calculate the molecular weight/molar mass of FeCl3. Then... 40.0 g FeCl3/MW FeCl3/0.275 L = M (concentration of FeCl3 in solution)
FeCl3 has the name iron III chloride
FeCl3 + H2O4-2 +Zn
Take 1 ml FeCl3 solution. add ammonia solution drop wise till brown precipitate just form. Now again add FeCl3 solution till brown precipitate just dissolve. This is your Neutral FeCl3 solution.
how to prepare .05M glutaraldhyde solution molecular weight is 100.12
34h 05m
FeCl3 ? 1.1 grams FeCl3 (1 mole FeCl3/162.2 grams) = 0.0068 moles of FeCl3 ------------------------------------
Look up or calculate the molecular weight/molar mass of FeCl3. Then... 40.0 g FeCl3/MW FeCl3/0.275 L = M (concentration of FeCl3 in solution)
FeCl3 has the name iron III chloride
FeCl3 +KSCN + AgNO3
FeCl3 + H2O4-2 +Zn
No, pure FeCl3 is not aqueous.
Take 1 ml FeCl3 solution. add ammonia solution drop wise till brown precipitate just form. Now again add FeCl3 solution till brown precipitate just dissolve. This is your Neutral FeCl3 solution.
why does salicylic acid give a positive test with FeCl3
.2M x V FeCl3=moles FeCl3 x 1mole Fe2S3/2mole FeCl3=moles of Fe2S3 x mm of Fe2S3/1 mole Fe2S3= g Fe2S3 x .65% yield. 2.75g Fe2S3/ .65= 4.23g Fe2S3/ 207.91= .02035 x 2mole FeCl3=.0407 moles FeCl3/ .2M FeCl3= .2035 L x 1000= 203.5 ml
what would be seen if you analyzed salicylic acid in FeCl3?