how i can prepare 0.6M H3PO4(250ml).
How many mols do you want? That's M x L = mols.
Then grams = mols x molar mass = ?
To prepare a 0.6M solution of H3PO4 (phosphoric acid) with a volume of 250ml, we need to follow these steps:
Step 1: Calculate the amount of H3PO4 needed.
The formula for calculating the amount of solute (H3PO4) required is:
Amount (in moles) = concentration (in M) x volume (in L)
Given:
Concentration = 0.6 M
Volume = 250 ml = 0.25 L
Using the formula, we can calculate the amount of H3PO4 needed:
Amount (in moles) = 0.6 M x 0.25 L = 0.15 moles
Step 2: Convert the moles of H3PO4 to grams.
To convert the moles of H3PO4 to grams, we need to know the molar mass of H3PO4. The molar mass of H3PO4 is the sum of the atomic masses of each element in the compound.
Atomic mass of H = 1.0079 g/mol
Atomic mass of P = 30.9738 g/mol
Atomic mass of O = 15.9994 g/mol
Molar mass of H3PO4 = (3 x 1.0079) + 30.9738 + (4 x 15.9994) = 97.9947 g/mol
Now we can calculate the mass of H3PO4 required:
Mass (in grams) = Amount (in moles) x Molar mass (in g/mol)
Mass (in grams) = 0.15 moles x 97.9947 g/mol = 14.6992 grams
Step 3: Prepare the solution.
To prepare the solution, follow these steps:
1. Weigh out 14.6992 grams of H3PO4 using a digital balance or weighing scale.
2. Transfer it to a clean and dry 250 ml volumetric flask.
3. Add distilled water to the flask until it reaches the 250 ml mark. Gently swirl the flask to ensure complete dissolution of H3PO4.
4. Label the flask as "0.6M H3PO4" and indicate the concentration and volume.
Note: Always follow safety precautions when working with chemicals. Use protective equipment such as gloves and goggles. Additionally, handle corrosive chemicals like H3PO4 with care and dispose of waste properly.