1. To calculate the pH of a solution of ammonia, we first need to find the concentration of hydroxide ions (OH-) in the solution.
Ammonia (NH3) can undergo a reaction with water to produce ammonium (NH4+) and hydroxide (OH-) ions according to the equation: NH3 + H2O -> NH4+ + OH-
Since ammonia is a weak base, we can assume that the concentration of hydroxide ions produced is equal to the concentration of ammonia (NH3) that reacts.
Given that the concentration of ammonia is 0.025M, the concentration of hydroxide ions is also 0.025M.
The hydroxide ion concentration can be used to calculate the pOH of the solution, using the formula: pOH = -log[OH-].
pOH = -log(0.025) = 1.60
The pH of the solution can be calculated using the formula: pH + pOH = 14.
pH + 1.60 = 14
pH = 12.40
Therefore, the pH of the 0.025M solution of ammonia is 12.40.
2. At body temperature, 37°C, the ionization constant of water (Kw) is known to be 1.00x10^-13.6.
The equation for the ionization of water is: H2O <=> H3O+ + OH-
At equilibrium, the concentration of H3O+ equals the concentration of OH-. Let x be the concentration of H3O+ (or OH-).
Using the Kw expression, we can write: Kw = [H3O+][OH-] = 1.00x10^-13.6
Since [H3O+] = [OH-] = x, we can simplify the expression to: x^2 = 1.00x10^-13.6
Taking the square root of both sides, we get: x = (1.00x10^-13.6)^(1/2)
x ≈ 1.00x10^-6.8
Therefore, at a body temperature of 37°C, the concentration of both H3O+ and OH- in water is approximately 1.00x10^-6.8 M.
1.Calculate the PH of 0.025M solution of ammonia kb=1.75x10^-5.
2.The ionization constant of water is Kw=1.00x10^-13.60 at body temperature,37°C .what are the H3O^+ and OH^- concentration at that temperature?
1 answer