ou weigh out Potassium Permanganate,
Mass of KMnO4 (MW=158.034).......... 0.1569 g
You dissolve it completely in water.......... 46.00 mL
(a) Molarity of MnO4- solution........................... ________________ M
You pipet out your UNKNOWN............. 0.90 mL
You acidify and titrate it with your KMnO4 solution until the permanganate color persists.
Volume of permanganate solution.......... 14.61 mL
(b) Molarity of the HOOH in the UNKNOWN...................................._____________ M
I answered this below at your first post.
Dr. Bob222 already answered this is your previous post.
lmmlm
To find the molarity of the MnO4- solution (part a), we need to use the following equation:
M1V1 = M2V2
Where:
M1 is the molarity of the KMnO4 solution (unknown)
V1 is the volume of the KMnO4 solution used for titration (14.61 mL)
M2 is the molarity of the MnO4- solution (unknown)
V2 is the volume of the unknown solution used for titration (0.9 mL)
To find M2, we can rearrange the equation as follows:
M2 = (M1V1)/V2
The volume of KMnO4 solution used for titration (V1) is given as 14.61 mL. The volume of the unknown solution used for titration (V2) is given as 0.9 mL.
Now, let's substitute the values we have:
M2 = (M1 * 14.61 mL) / 0.9 mL
The molarity of the KMnO4 solution (M1) is not given in the question, so we need more information to determine this value. If we have the molar mass of the substance, we can calculate the molarity using the formula:
Molarity (M) = Mass (g) / Molar Mass (g/mol)
In this case, the molar mass of KMnO4 is given as 158.034 g/mol. The mass of KMnO4 weighed out is given as 0.1569 g. Using these values, we can calculate M1 and then substitute it into our equation.
M1 = 0.1569 g / 158.034 g/mol
Now, we can calculate M2:
M2 = (M1 * 14.61 mL) / 0.9 mL
To find the molarity of the HOOH in the unknown solution (part b), we need to use a similar equation:
M1V1 = M2V2
Where:
M1 is the molarity of the KMnO4 solution
V1 is the volume of the KMnO4 solution used for titration (46.00 mL)
M2 is the molarity of the HOOH (unknown)
V2 is the volume of the unknown solution used for titration (0.9 mL)
Since M1 is now known (calculated in part a), we can rearrange the equation to solve for M2:
M2 = (M1 * V1) / V2
Substituting the values:
M2 = (M1 * 46.00 mL) / 0.9 mL
Thus, to find the molarity of the HOOH in the unknown solution, you need to calculate M1 in part a (using the molar mass and mass of KMnO4) and then substitute it into the equation for part b.