A 7mL triprotic acid was analyzed and found to contain 0.2572 grams of acid, evidence of phosphate group. Find the molecular weight of the acid, and identify acid.
Thank you.
To find the molecular weight of the acid and identify it, we need to use the given information about the amount of acid present and its volume.
1. Start by calculating the molarity of the acid:
Molarity (M) = moles/volume
Since the volume is given in mL, we need to convert it to L:
Volume = 7 mL = 7/1000 L = 0.007 L
Therefore, the molarity (M) = moles/0.007 L
2. Convert the mass of the acid to moles:
Given that the mass of the acid is 0.2572 grams, we need to convert it to moles.
Moles = mass/molar mass
3. Rearrange the molarity formula to solve for the moles:
Moles = Molarity x volume
Plug in the values:
Moles = M x 0.007 L
4. Substitute the moles value in the mass to moles conversion equation:
Moles = mass/molar mass
Rearrange the equation to solve for the molar mass:
Molar mass = mass/Moles
Plug in the values:
Molar mass = 0.2572 g / Moles
5. Use the calculated molar mass to identify the acid:
To determine the identity of the acid, you can compare its molar mass to the molar masses of known compounds and identify a match.
Once you have the calculated molar mass, you can search for known acids with a similar molar mass or use chemical databases to compare the molar mass and identify the acid in question.