The autodissociation of water to H+ and OH- is endothermic. At a higher temperature more of the water molecules have sufficient energy to dissociate. So, Kw is greater.

At 25oC, Kw = 1.0 x 10-14. (standard Kw)
At 65oC, Kw = 1.0 x 10-13.

Calculate the hydrogen ion concentration, [H+], in 0.0474 M LiOH at 65oC.

LiOH = 0.0474M

(OH^-) = 0.0474M
(H^+)(OH^-) = 1E-13
Substitute the OH^- from LiOH and solve for H^+.

To calculate the hydrogen ion concentration, [H+], in 0.0474 M LiOH at 65oC, we need to consider the dissociation of water and the ionization of LiOH.

First, let's write down the balanced chemical equation for the dissociation of water:
H2O ⇌ H+ + OH-

We know that at 65oC, Kw (the equilibrium constant for the dissociation of water) is 1.0 x 10^-13.

Since LiOH is a strong base, it will fully dissociate in water:
LiOH → Li+ + OH-

Now, since the concentration of LiOH is given as 0.0474 M, we can assume that the concentration of OH- is also 0.0474 M.

Since the concentration of OH- is equal to [OH-], we can use this value to calculate [H+]:

Kw = [H+][OH-]

Substituting the given values:

1.0 x 10^-13 = [H+][0.0474]

Now we can solve for [H+]:

[H+] = (1.0 x 10^-13) / 0.0474

Calculating this value gives us:

[H+] ≈ 2.11 x 10^-12 M

Therefore, the hydrogen ion concentration, [H+], in 0.0474 M LiOH at 65oC is approximately 2.11 x 10^-12 M.

To calculate the hydrogen ion concentration ([H+]) in a solution of 0.0474 M LiOH at 65°C, we need to consider the reaction between LiOH and water.

The reaction between LiOH and water can be written as follows:
LiOH + H2O -> Li+ + OH- + H2O

Since LiOH is a strong base, it will fully dissociate in water. Therefore, we can treat LiOH as a source of OH- ions.

The concentration of OH- in the solution is equal to the concentration of LiOH since it fully dissociates:
[OH-] = 0.0474 M

Next, we need to consider the autoionization of water, which produces both H+ and OH- ions:
H2O -> H+ + OH-

At 65°C, the equilibrium constant (Kw) for the autoionization of water is given as 1.0 x 10^-13.

Since water dissociates into equal amounts of H+ and OH- ions, we can assume that the concentration of H+ ions is the same as the concentration of OH- ions.

Therefore, [H+] = [OH-] = 0.0474 M

Thus, the hydrogen ion concentration ([H+]) in a 0.0474 M solution of LiOH at 65°C is 0.0474 M.