what is molarity of h2so4 solution contaning 9.8g of h2so4 per 500ml?
Molarity = (9.8g x 1000) / (98 x 500) = 0.2M
mols H2SO4 = grams/molar mass = ?
M = mols/L solution = ?
Calculate the molarity of H2SO4 solution containing 9.8 g of H2SO4 per 500 mL?
9.8
To find the molarity of a solution, you need to know the amount of solute in moles (mol) and the volume of the solution in liters (L).
Given:
Mass of H2SO4 = 9.8 g
Volume of solution = 500 mL
Step 1: Convert the volume of the solution from milliliters (mL) to liters (L).
500 mL ÷ 1000 = 0.5 L
Step 2: Calculate the amount of solute (H2SO4) in moles.
To do this, you need to know the molar mass of H2SO4, which is:
(2 x atomic mass of hydrogen) + atomic mass of sulfur + (4 x atomic mass of oxygen)
(2 x 1) + 32 + (4 x 16) = 98 g/mol
Now, use the formula:
Amount of solute (in moles) = Mass of solute (in grams) / Molar mass of solute
Amount of H2SO4 (in moles) = 9.8 g / 98 g/mol = 0.1 mol
Step 3: Calculate the molarity of the solution.
Molarity (M) = Amount of solute (in moles) / Volume of solution (in liters)
Molarity of the H2SO4 solution = 0.1 mol / 0.5 L = 0.2 M
Therefore, the molarity of the H2SO4 solution containing 9.8g of H2SO4 per 500mL is 0.2 M.