prepare 1M 100 ml H2SO4. 98% H2SO4, density 1.84
here
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 solution with a concentration of 98% and a density of 1.84 g/ml, you would need to follow these steps:
Step 1: Determine the molecular weight of sulfuric acid (H2SO4).
- H = 1 atomic mass unit (amu)
- S = 32 amu
- O = 16 amu
Total molecular weight of H2SO4 = (2 * 1) + 32 + (4 * 16) = 98 amu
Step 2: Calculate the amount of H2SO4 needed.
Since we want to prepare a 1M solution, which means 1 mole of H2SO4 in 1 liter (1000 mL) of solution, we need to calculate how many moles are needed to prepare 100 ml.
Moles = Molarity * Volume (in liters)
Moles = 1 * (100/1000) = 0.1 moles
Step 3: Calculate the mass of H2SO4 needed.
The solution's concentration is given as 98%, which means that 100 ml of the solution contains 98 grams of H2SO4. However, we want to calculate how much 0.1 moles of H2SO4 weighs.
Molar mass of H2SO4 = 98 g/mol
Mass = Moles * Molar mass
Mass = 0.1 * 98 = 9.8 grams
So, you would need 9.8 grams of H2SO4 to prepare 1M 100 ml of the solution.
It's important to note that sulfuric acid is highly corrosive and caution should be exercised when handling it. Protective equipment including gloves and goggles should be worn, and it should be handled in a well-ventilated area.