How do I find the molarity of Fe(SCN)2+?
I know the molarity of SCN=0.1 and the molarity of Fe is 0.0001. The volume of SCN is 5 mL and the volume of the Fe is also 5mL. I also think that I use M1V1=M2V2.
You have diluted each by a factor of 2 (that is, from 5 to 10); therefore, (Fe^+3) = (1/2)*0.0001 and (SCN^-) = (1/2)*0.1.
M1V1 = M2V2 works but this one is so easy you don't need an equation.
Thanks. Would it matter which molarity I use if I used M1V1 = M2V2
To find the molarity of Fe(SCN)2+, you can use the formula M1V1 = M2V2, where M1 is the initial molarity, V1 is the initial volume, M2 is the final molarity, and V2 is the final volume.
In this case, the initial molarity of SCN^- is 0.1 M, and the initial volume is 5 mL. The initial molarity of Fe is 0.0001 M, and the initial volume is also 5 mL.
Let's use M1V1 = M2V2 to calculate the final molarity:
(0.1 M)(5 mL) = M2(5 mL)
Dividing both sides of the equation by 5 mL:
0.1 M = M2
Therefore, the molarity of Fe(SCN)2+ is 0.1 M.
To find the molarity of Fe(SCN)2+, you can use the formula M1V1 = M2V2, where M1 and V1 represent the initial molarity and volume, and M2 and V2 represent the final molarity and volume.
Since you know the molarity of SCN- (0.1 M) and the molarity of Fe (0.0001 M), you can plug these values into the formula:
M1V1 = M2V2
(0.0001 M)(5 mL) = M2(5 mL)
Now, you need to solve for M2, which represents the molarity of Fe(SCN)2+. Rearranging the formula, we get:
M2 = (0.0001 M)(5 mL) / 5 mL
M2 = 0.0001 M
Therefore, the molarity of Fe(SCN)2+ is 0.0001 M.
Explanation: In order to find the molarity of Fe(SCN)2+, you need to use the equation M1V1 = M2V2, also known as the dilution formula. This equation allows you to relate the initial molarity and volume of a solution to the final molarity and volume.
In this case, you are given the initial molarities of SCN- and Fe, along with their respective volumes. By plugging these values into the equation, you can solve for the final molarity of Fe(SCN)2+.