prepare 1M 100 ml H2SO4. 98% H2SO4, density 1.84
First of all, the density makes no sense without units. Secondly, you should only specify the amount of something present in one way. The questions gives two: (1) a molarity and a volume. (2) a percentage (by volume or by mass?) and a density. So you can't solve such a question unambiguously in general.
Suppose we go with the given molarity. That means there are 0.1 moles of sulfuric acid present (1.0 mol/L * 0.1 L). That will require adding how many grams to 100 mL of water? Molecular mass of H2SO4 = 98 g/mol, so use 98*0.1 = 0.98 grams of H2SO4.
If we go with the percent by mass, then assume the density was supposed to be 1.84 g/L, then that's 1.84g/L*0.1L = 0.184 grams all told, 98% of which is H2SO4 = 0.18032 grams.
So you see, the desired solution is impossible to obtain on the face of it. You can either have a desired molarity or a desired mass percentage and density, but not both (unless by luck the desired quantities coincide).
First of all density with no units is meaningless and makes the question impossible to solve.
Secondly the percentage without the type is meaningless.
Although can easily be find out in such question but, you should be specify that.
But to give idea about the solution lets assume
d(H2SO4) = 1.84 kg/L and 98% means
100 unit volume of stock solution contains
98 unit volume of H2SO4
so problem asks us to find the amount (mL) of H2SO4 (stock) to prepare 100 mL of 1M soluiton
x mL stock(H2SO4) =
(1mol H2SO4 / 1L solution) *
(1L solution / 1000mL solution) * (100mL solution) *
(98.04g H2SO4 / 1mol H2SO4) *
(1kg H2SO4 / 1000 g H2SO4) *
(1L H2SO4 / 1.84kg H2SO4) *
(1000mL H2SO4 / 1L H2SO4) *
(100ml stockH2SO4 / 98mL H2SO4)
----
x mL H2SO4 = 5.437 mL
to prepare 100 mL, 1M H2SO4 from stock (98% [v/v]; 1.84 [kg/L]; 98.04 [g/mol])
to 100 mL flat bottom flask add some amount of water (not much),
and pour 5.45 mL H2SO4 stock solution on it.
Dilute the solution to 100 mL
To prepare 1M 100 ml of H2SO4 using 98% H2SO4 with a density of 1.84 g/ml, you will need to follow these steps:
Step 1: Calculate the molar mass of H2SO4.
- The molar mass of hydrogen (H) is 1g/mol.
- The molar mass of sulfur (S) is 32.07g/mol.
- The molar mass of oxygen (O) is 16g/mol.
- Multiply the molar mass of hydrogen by 2, and the molar mass of oxygen by 4, then add all the masses together.
- The molar mass of H2SO4 = (2 x 1g/mol) + (32.07g/mol) + (4 x 16g/mol) = 98.09g/mol.
Step 2: Calculate the mass of pure H2SO4 needed.
- To prepare 1M 100 ml of H2SO4, 1 mole of H2SO4 would be required.
- Since the molar mass of H2SO4 is 98.09g/mol, the mass needed can be calculated as: 1 mole x 98.09g/mol = 98.09g.
Step 3: Calculate the volume of the 98% H2SO4 needed.
- The density of the 98% H2SO4 is 1.84g/ml, which means that 1 ml of H2SO4 has a mass of 1.84g.
- Divide the mass of H2SO4 needed (98.09g) by the density to find the volume: 98.09g / 1.84g/ml = 53.33 ml.
- Since we need 100 ml of H2SO4, we will need to dilute 53.33 ml of the 98% H2SO4.
Step 4: Dilute the 98% H2SO4 to prepare 1M 100 ml of H2SO4.
- Take 53.33 ml of the 98% H2SO4 and transfer it to a measuring flask or container.
- Add distilled water to the measuring flask until the total volume reaches 100 ml.
- Mix the solution thoroughly to ensure proper dilution.
Now you have prepared 1M 100 ml of H2SO4 using the 98% H2SO4 solution with a density of 1.84 g/ml.
To prepare 1M 100 ml of H2SO4 with 98% purity, we need to calculate the volume of concentrated H2SO4 required.
First, let's convert the 1M concentration to moles.
1M means 1 mole of H2SO4 per liter of solution. Since we only need 100 ml (0.1 liters) of solution, we will need 1 * 0.1 = 0.1 moles of H2SO4.
Next, let's determine the molarity of the concentrated H2SO4. Assuming it is 98% pure, we will need to use a density conversion to calculate the molarity.
Density is defined as mass/volume. Since we have the density (1.84 g/ml) and the volume (100 ml), we can calculate the mass of H2SO4 using the formula:
Mass = Density * Volume
Mass = 1.84 g/ml * 100 ml
= 184 g
Now, let's determine the molar mass of H2SO4.
H2SO4 has the following atomic masses:
H = 1 g/mol
S = 32 g/mol
O = 16 g/mol (x4 for the four oxygen atoms)
Molar Mass = 2(1 g/mol) + 32 g/mol + 16 g/mol * 4
= 98 g/mol
Finally, we can calculate the volume of concentrated H2SO4 needed using the formula:
Volume (in liters) = Moles / Molarity
Volume (in liters) = 0.1 moles / (98/1000) mol/l
= 1.02 ml
Therefore, to prepare 1M 100 ml of H2SO4 with 98% purity, you would need approximately 1.02 ml of concentrated H2SO4, assuming it is 98% pure.