The concentrated H2SO4 of 155g dissolved in enough amount of water if acidic solution is 2.3L
a) what is the mole of H2SO4
b) what is the concentration H2SO4
c) what is the concentration of H+(H3O+) created in the solution
d) what is the PH value of solution
e) what is the concentration of SO4 ion
2) At 298K, what are the molarities of pure water?
a) To find the moles of H2SO4, we need to use its molar mass. The molar mass of H2SO4 is calculated by adding the atomic masses of each element:
H (1.01 g/mol) x 2 + S (32.07 g/mol) + O (16.00 g/mol) x 4 = 98.09 g/mol
Now, divide the mass of H2SO4 (155 g) by its molar mass:
155 g / 98.09 g/mol = 1.58 mol
Therefore, there are 1.58 moles of H2SO4.
b) Concentration is defined as moles of solute divided by the volume of the solution in liters. In this case, the volume of the acidic solution is given as 2.3 L.
Concentration of H2SO4 = moles of H2SO4 / volume of solution
Concentration of H2SO4 = 1.58 mol / 2.3 L ≈ 0.687 mol/L
Therefore, the concentration of H2SO4 is approximately 0.687 mol/L.
c) In aqueous solutions, H2SO4 dissociates to form H+ (H3O+) ions. According to the balanced chemical equation for the dissociation of H2SO4, one mole of H2SO4 produces two moles of H+ (H3O+) ions.
Therefore, the concentration of H+ (H3O+) ions is twice the concentration of H2SO4.
Concentration of H+ (H3O+) ions = 2 x Concentration of H2SO4
Concentration of H+ (H3O+) ions = 2 x 0.687 mol/L = 1.374 mol/L
Therefore, the concentration of H+ (H3O+) ions in the solution is 1.374 mol/L.
d) The pH value of a solution can be calculated using the formula:
pH = -log10[H+]
We know the concentration of H+ ions in the solution is 1.374 mol/L.
pH = -log10(1.374) ≈ -0.138
Therefore, the pH value of the solution is approximately -0.138. Note that pH values are typically defined on a scale of 0 to 14, so this answer seems unusual. It is possible that there was an error in the calculations or information given.
e) Since H2SO4 is a strong acid, it fully dissociates in water to form H+ (H3O+) and SO4 ions. According to the dissociation process:
H2SO4 ⟶ 2H+ + SO4
The concentration of SO4 ions is the same as the concentration of H2SO4, which is 0.687 mol/L.
Therefore, the concentration of SO4 ions in the solution is 0.687 mol/L.
2) Pure water in terms of concentration is typically described as having a molarity of 55.56 mol/L (at 25°C or 298K). This value is obtained by considering the dissociation of water molecules:
H2O ⟶ H+ + OH-
At 298K, the concentration of H+ and OH- ions in pure water is equal and each has a value of 1.00 x 10^-7 mol/L. Since each water molecule produces one H+ ion and one OH- ion, the total molarity of pure water is:
Molarity of pure water = Concentration of H+ ions = Concentration of OH- ions = 1.00 x 10^-7 mol/L