Final answer:
The statement is false; in neutral water, the concentration of [H+] and [OH-] is 1.0 × 10^-7 M, not 0.00 M, at 25°C. The neutrality is due to the equal concentrations of H3O+ and OH- ions, giving a pH and pOH of 7.00.
Step-by-step explanation:
The statement 'In neutral water, [H+] = [OH-] = 0.00 M' is false. In a neutral aqueous solution, the concentration of hydronium ions ([H3O+], commonly referred to as [H+]) and hydroxide ions ([OH-]) is not zero. Instead, both concentrations are equal to 1.0 × 10-7 M at 25°C. This equality in concentrations results in a neutral solution because the product of the two concentrations, [H+][OH-], is always 1.0 × 10-14, reflective of the constant equilibrium for water dissociation.
Moreover, at 25°C, the pH and pOH of a neutral solution are both 7.00, because pH is calculated as -log [H3O+] and pOH as -log [OH-]. These values add up to 14.00, which is consistent with the relation pH + pOH = 14.00 for aqueous solutions at this temperature.