calculate the initial concentration of SCN- ions and Fe3+ ions when a solution was prepared by mixing 3.00mL of 0.00280M KSCN, 6.00 mL of 0.250M Fe(NO3)3 and 16ml of 0.050M HNO3.
You can do this one of several ways. Some are longer than others but all give the same answer. The easy way I think is to just recognize that the initial concn of EACH reagent in the mixture is diluted and solve it that way.
What's the total volume? That's 3.00 + 6.00 mL + 16 mL = 25 mL.
So you diluted KSCN from 3 mL to 25 mL so the new concn is
0.0028M x (3/25) = ?
tough, eh?
Likewise you can calculate the concn of each of the other reagents in the mixture.
If you wish you may use the dilution formula of
c1v1 = c2v2
c = concn
v = volume
0.0028*3 = c2*25
Solve for c2
Describe how you could separate the components of a mixture of PbCl2 and NaSO4 and recover the two substances.
To calculate the initial concentration of SCN- ions and Fe3+ ions when the solution is prepared by mixing the given solutions, we can use the concept of moles and volumes of the solutions.
Step 1: Calculate the moles of SCN- ions
We can use the formula: Moles = Concentration (mol/L) × Volume (L)
Moles of SCN- ions = 0.00280 M × 0.00300 L = 0.0000084 mol
Step 2: Calculate the moles of Fe3+ ions
Moles of Fe3+ ions = 0.250 M × 0.00600 L = 0.00150 mol
Step 3: Calculate the total volume of the solution
Total volume = 3.00 mL + 6.00 mL + 16.00 mL = 25.00 mL = 0.0250 L
Step 4: Calculate the concentration of SCN- ions
Concentration of SCN- ions = Moles / Total volume
= 0.0000084 mol / 0.0250 L
≈ 0.000336 M
Step 5: Calculate the concentration of Fe3+ ions
Concentration of Fe3+ ions = Moles / Total volume
= 0.00150 mol / 0.0250 L
= 0.0600 M
Therefore, the initial concentration of SCN- ions is approximately 0.000336 M, and the initial concentration of Fe3+ ions is 0.0600 M.
To calculate the initial concentration of SCN- ions and Fe3+ ions in the solution, you need to consider the volumes and concentrations of the KSCN, Fe(NO3)3, and HNO3 solutions that were mixed.
First, let's calculate the total volume of the solution:
Total Volume = volume of KSCN + volume of Fe(NO3)3 + volume of HNO3
Total Volume = 3.00 mL + 6.00 mL + 16 mL
Total Volume = 25.00 mL
Next, we need to calculate the moles of SCN- ions in the KSCN solution and the moles of Fe3+ ions in the Fe(NO3)3 solution.
Moles of SCN- = volume of KSCN x concentration of KSCN
Moles of SCN- = 3.00 mL x (0.00280 mol/L)
Moles of SCN- = 0.0084 mol
Moles of Fe3+ = volume of Fe(NO3)3 x concentration of Fe(NO3)3
Moles of Fe3+ = 6.00 mL x (0.250 mol/L)
Moles of Fe3+ = 0.0015 mol
Now, let's calculate the total moles of SCN- ions and Fe3+ ions in the solution:
Total Moles of SCN- = Moles of SCN- in KSCN
Total Moles of SCN- = 0.0084 mol
Total Moles of Fe3+ = Moles of Fe3+ in Fe(NO3)3
Total Moles of Fe3+ = 0.0015 mol
Since the stoichiometry of Fe(SCN)3 complex formation is 1:1, the total moles of SCN- ions and Fe3+ ions are equal.
Therefore, the initial concentration of SCN- ions and Fe3+ ions in the solution is:
Concentration of SCN- = Total Moles of SCN- / Total Volume
Concentration of SCN- = 0.0084 mol / 25.00 mL
Concentration of SCN- = 0.336 M
Concentration of Fe3+ = Total Moles of Fe3+ / Total Volume
Concentration of Fe3+ = 0.0015 mol / 25.00 mL
Concentration of Fe3+ = 0.060 M
So, the initial concentration of SCN- ions is 0.336 M, and the initial concentration of Fe3+ ions is 0.060 M in the solution.