Calculate the concentration of each solute and each ions when 25.0 mL of 18.0 M H2SO4 is mixed with 130.0 mL water
To calculate the concentration of each solute and each ion when 25.0 mL of 18.0 M H2SO4 is mixed with 130.0 mL of water, we need to first understand the concept of molarity and dilution.
Molarity (M) is defined as the number of moles of solute divided by the volume of the solution in liters. It is usually measured in moles per liter (mol/L).
For the given problem, we have 25.0 mL (0.025 L) of 18.0 M H2SO4 and 130.0 mL (0.13 L) of water. We need to calculate the concentration of each solute (H2SO4) and each ion (H+, SO4 2-) in the resulting solution.
To calculate the new concentration of H2SO4 after dilution, we use the formula:
M1V1 = M2V2
where,
M1 = initial concentration of H2SO4 (18.0 M)
V1 = initial volume of H2SO4 (0.025 L)
M2 = final concentration of H2SO4 (unknown)
V2 = final volume of the solution (0.025 L + 0.13 L = 0.155 L)
Rearranging the formula to solve for M2:
M2 = (M1 x V1) / V2
M2 = (18.0 M x 0.025 L) / 0.155 L
M2 = 2.903 M
Thus, the concentration of H2SO4 in the resulting solution is approximately 2.903 M.
Since H2SO4 is a strong acid, it dissociates completely in water to produce H+ and SO4 2- ions in a 1:1 ratio. Therefore, the concentration of H+ ions is also 2.903 M, and the concentration of SO4 2- ions is also 2.903 M.