show how 500ml of 2M H2SO4 can be prepared from a bottle of the acid with 95% purity(H=1, S=32, O=16, specific gravity of H2SO4 is 1.82
Calculate the M or the 95% bottle of H2SO4.
1000 nK x 1,82 g/mL x 0.95 x 1 mol/98 g/mol = approx 18 that's an estimate.
Then mL x M = mL x M is the dilution formula.
500 mL x 2 M = ?mL x 18 M.
Solve for ?mL. Add that ?mL of the 95% stuff to a 500 mL volumetric flask containing about 200 or 300 mL distilled water, then fill to the mark of the flask, mix thoroughly, stopper, label.
Post your work if you get stuck.
To prepare 500ml of 2M H2SO4 solution from the given bottle of acid with 95% purity and a specific gravity of 1.82, you'll need to follow these steps:
Step 1: Calculate the desired amount of acid needed:
We know that the molarity (M) is equal to moles/volume (L).
Moles = M x L
Given:
Desired volume of acid = 500ml = 0.5L
Desired molarity of acid = 2M
Moles = 2M x 0.5L
= 1 mole
Step 2: Calculate the actual amount of pure H2SO4 present in the bottle:
Given:
Purity of H2SO4 = 95% = 0.95
Specific gravity of H2SO4 = 1.82
We know that specific gravity (S.G.) is the ratio of the density of a substance to the density of a reference substance (usually water).
Density of H2SO4 = 1.82 x Density of water
The density of water is approximately 1.0g/ml.
Density of H2SO4 = 1.82 x 1.0g/ml
= 1.82g/ml
Now, let's calculate the actual amount of pure H2SO4 in the bottle by considering the specific gravity and purity.
Actual amount of pure H2SO4 in 1ml of acid = 1.82g x 0.95
= 1.73g
Now, to get the amount of pure H2SO4 in 500ml, multiply by the volume:
Actual amount of pure H2SO4 in the bottle = 1.73g/ml x 500ml
= 865g
Step 3: Calculate the amount of the actual acid needed from the bottle:
The molar mass of H2SO4 can be calculated as follows:
(Molar mass of H) x 2 + Molar mass of S + (Molar mass of O) x 4
(1g/mol) x 2 + (32g/mol) + (16g/mol) x 4
2g + 32g + 64g
= 98g/mol
To calculate the volume of the actual acid needed from the bottle, divide the mass by the molar mass:
Volume (L) = Mass (g) / Molar mass (g/mol)
Volume (L) = 865g / 98g/mol
Volume (L) = 8.826L
Step 4: Dilute the acid:
To prepare a 2M H2SO4 solution, you need to dilute the acid to a final volume of 500ml. However, you have approximately 8.826L of the actual acid, which is much more than what you need.
Therefore, you will need to dilute the acid by adding an appropriate amount of water. The water volume can be determined by using the equation:
Final volume (L) = Initial volume (L) + Volume of water added (L)
Given:
Initial volume = 8.826L
Final volume = 0.5L
Let's calculate the volume of water to be added:
Volume of water added (L) = Final volume (L) - Initial volume (L)
Volume of water added (L) = 0.5L - 8.826L
Volume of water added (L) = -8.326L
Since the volume of water added cannot be negative (as we are diluting), it means you don't need to add any water since the amount of acid in the bottle is already more than enough.
Therefore, you can directly use the 8.826L of the actual acid from the bottle to prepare a 2M H2SO4 solution with a final volume of 500ml.
To prepare 500ml of a 2M H2SO4 solution from a bottle of acid with 95% purity, you can follow these steps:
Step 1: Calculate the molecular weight of H2SO4.
The molecular weight of H2SO4 can be calculated by adding the atomic masses of the elements:
(2 × H) + S + (4 × O) = (2 × 1) + 32 + (4 × 16) = 98 g/mol
Step 2: Determine the desired number of moles of H2SO4.
To prepare a 2M solution, you'll need to find the number of moles required for 500ml. Remember that Molarity (M) is defined as moles of solute per liter of solution. Here, you have 500ml, which is equivalent to 0.5 liters:
Moles = Molarity × Volume (in liters) = 2M × 0.5L = 1 mole
Step 3: Calculate the required mass of H2SO4.
Since you have determined the number of moles required, you can calculate the mass of H2SO4 needed using its molecular weight:
Mass = Moles × Molecular weight = 1 mole × 98 g/mol = 98 grams
Step 4: Adjust for the purity of the acid.
Since the bottle of H2SO4 has a purity of 95%, the actual amount of pure H2SO4 present will be 95% of the calculated mass:
Actual Mass = Purity × Calculated mass = 0.95 × 98 grams = 93.1 grams
Step 5: Determine the volume of H2SO4 required.
The specific gravity of H2SO4 is 1.82, which means that 1ml of H2SO4 weighs 1.82 grams. To calculate the volume required, divide the actual mass by the specific gravity:
Volume = Mass ÷ Specific gravity = 93.1g ÷ 1.82 g/mL = 51.1 mL
Therefore, to prepare 500ml of a 2M H2SO4 solution, you would need 51.1ml of the 95% purity acid to dilute with deionized or distilled water to the desired volume.