How we can prepare sulfuric acid solution containing 6.10gperdm3 of sulfuric acid?
Usually the problem is to prepare H2SO4 solution of 6.10 g/dm^3 BUT we are given a solution of some different concentration initially. I will assume we have a sample of H2SO4 that contains 12.2 g H2SO4/dm^3 and you want to prepare 100 mL of the solution containing 6.10 g/dm^3.
Pipet 50 mL of the 12.2 g/dm^3 solution into a 100 mL volumetric flask, add deionized water to the mark on the volumetric flask, stopper, mix thoroughly, label.
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thank you so much sir.
To prepare a sulfuric acid solution containing 6.10 g/dm3 of sulfuric acid, you need to follow these steps:
1. Determine the molar mass of sulfuric acid (H2SO4). The molar mass of hydrogen (H) is 1 g/mol, sulfur (S) is 32 g/mol, and oxygen (O) is 16 g/mol. So, the molar mass of sulfuric acid is (2 * 1) + 32 + (4 * 16) = 98 g/mol.
2. Use the equation Molarity (M) = moles of solute/volume of solution in liters (L). Rearrange the equation to solve for the moles of solute, which gives the formula: Moles of solute = Molarity * Volume (in L).
3. Convert the given concentration of sulfuric acid from g/dm3 to grams per liter (g/L). Since 1 dm3 is equal to 1 L, the concentration remains the same.
4. Substitute the given values into the formula. We have the concentration in g/L (6.10 g/L) and the molar mass of sulfuric acid from step 1 (98 g/mol). Now we can calculate the number of moles of sulfuric acid.
Moles of solute = (6.10 g/L) / (98 g/mol) = 0.062 mol/L
5. Decide on the volume of solution you want to prepare. Let's say you want to prepare 500 mL (0.5 L) of the sulfuric acid solution.
6. Use the moles of solute and desired volume of solution to calculate the required amount of sulfuric acid.
Mass of sulfuric acid = Moles of solute * Molar mass
= (0.062 mol/L) * (98 g/mol) * (0.5 L)
= 3.03 g
Therefore, to prepare a sulfuric acid solution with a concentration of 6.10 g/dm3, you would need to dissolve 3.03 grams of sulfuric acid in 500 mL of water or solution (0.5 L).