The pH of 40 cm3 a 0,05 mol∙dm–3 solution of H2SO4 is?
To find the pH of the solution, we first need to determine the concentration of H+ ions in the solution.
H2SO4 is a strong acid that dissociates completely in water, so for every 1 mole of H2SO4, we get 2 moles of H+ ions.
The volume of the solution is given as 40 cm3, which can be converted to liters by dividing by 1000:
40 cm3 = 40/1000 = 0.04 L
The concentration of H2SO4 is given as 0.05 mol∙dm–3, which means there are 0.05 moles of H2SO4 in 1 dm3 (or 1 liter) of solution.
To find the concentration of H+ ions in the solution, we multiply the concentration of H2SO4 by the number of H+ ions produced per mole of H2SO4:
0.05 mol∙dm–3 x 2 = 0.1 mol∙dm–3
Now that we have the concentration of H+ ions, we can find the pH using the formula:
pH = -log[H+]
pH = -log(0.1) = -(-1) = 1
Therefore, the pH of the 0.05 mol∙dm–3 solution of H2SO4 is 1.