3.25ml of H2SO4 dissolve in 68.0 ml water
This statement describes the process of dissolving 3.25 milliliters of sulfuric acid (H2SO4) in 68.0 milliliters of water. The resulting solution will contain both the H2SO4 and the water, and the two substances will be mixed together.
To calculate the concentration of the H2SO4 solution, we can use the formula:
Concentration = Amount of solute / Volume of solution
In this case, the amount of solute is given as 3.25 ml of H2SO4 and the volume of the solution is the sum of the H2SO4 and water, which is 3.25 ml + 68.0 ml = 71.25 ml.
Now we can plug these values into the formula:
Concentration = 3.25 ml / 71.25 ml
Concentration = 0.0455 or 4.55% (rounding to two decimal places)
Therefore, the concentration of the H2SO4 solution is 4.55%.
To find the concentration of the H2SO4 solution, you need to divide the volume of the solute (3.25 mL) by the total volume of the solution (3.25 mL + 68.0 mL).
First, add the volumes of the solute and the solvent together:
3.25 mL + 68.0 mL = 71.25 mL
Next, divide the volume of the solute by the total volume of the solution and multiply the result by 100 to express it as a percentage:
(3.25 mL / 71.25 mL) * 100 = 4.56140350877 %
Therefore, the concentration of the H2SO4 solution is approximately 4.56%.