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.
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.
FeCl3 + H2O4-2 +Zn
The molar mass of FeCl3 is 162.20 g/mol. First, convert 40.0 g to moles by dividing by the molar mass. Then, calculate the concentration in mol/L by dividing the moles of FeCl3 by the volume of the solution in liters (0.275 L).
The amount of FeCl3 needed depends on the concentration of the FeCl3 solution required for the test. Typically, a 2-5% solution of FeCl3 is used. To make a 100mL of 2-5% FeCl3 solution, you would need to dissolve 2-5 grams of FeCl3 in distilled water. The exact amount can be calculated using the formula: (desired % concentration/100) x volume of solution needed x molar mass of FeCl3.
When ferric chloride (FeCl3) is mixed with iron (Fe), the iron displaces the chloride ion to form ferrous chloride (FeCl2) and iron chloride (FeCl3). The chemical equation is: FeCl3 + Fe -> FeCl2 + FeCl3.
The optimum pH range for FeCl3 as a coagulant is typically between 4.0 and 6.0. At this pH range, the effectiveness of FeCl3 in coagulation and flocculation processes is maximized, leading to improved removal of impurities in water treatment applications. It is essential to optimize the pH to ensure the best performance of FeCl3 as a coagulant.
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.
The optimum pH for alum is typically around 6.5-7.5, as this allows for effective coagulation and flocculation of suspended particles in water treatment processes. For FeCl3, the optimum pH is usually lower, around 5.0-6.0, to ensure the formation of positively charged iron hydroxide flocs for efficient removal of contaminants in water treatment applications.
34h 05m
FeCl3 + H2O4-2 +Zn
To find the number of moles in 1.1 grams of FeCl3, you'll first determine the molar mass of FeCl3 (55.85 + 35.45*3) = 162.31 g/mol. Then, divide the given mass (1.1g) by the molar mass to get the number of moles (1.1g / 162.31g/mol ≈ 0.007 moles of FeCl3).
The molar mass of FeCl3 is 162.20 g/mol. First, convert 40.0 g to moles by dividing by the molar mass. Then, calculate the concentration in mol/L by dividing the moles of FeCl3 by the volume of the solution in liters (0.275 L).
The amount of FeCl3 needed depends on the concentration of the FeCl3 solution required for the test. Typically, a 2-5% solution of FeCl3 is used. To make a 100mL of 2-5% FeCl3 solution, you would need to dissolve 2-5 grams of FeCl3 in distilled water. The exact amount can be calculated using the formula: (desired % concentration/100) x volume of solution needed x molar mass of FeCl3.
When ferric chloride (FeCl3) is mixed with iron (Fe), the iron displaces the chloride ion to form ferrous chloride (FeCl2) and iron chloride (FeCl3). The chemical equation is: FeCl3 + Fe -> FeCl2 + FeCl3.
Yes, FeCl3 is soluble in water. It forms a greenish-brown solution when dissolved in water.
To prepare a 0.5M glutaraldehyde solution, you would need to dilute a concentrated glutaraldehyde stock solution with the appropriate volume of water or buffer solution. Calculate the volume of stock solution needed based on the desired final volume and concentration, then dilute with the solvent. Finally, mix the solution thoroughly to ensure uniform distribution. Remember to follow safety protocols when working with glutaraldehyde, as it is a hazardous chemical.
Iron (III) Cloride