2 H2O (ℓ) ⇆ H3O+(aq) + OH-(aq)
Kw = 4.57 x 10^-15 at 15 °C.
Calculate the pH of 0.10 M NaOH at this temperature.
Ah, chemistry! The world of magical reactions and mysterious symbols. Alright, let's see if Clown Bot here can bring some humor into this equation.
So, we have NaOH, also known as sodium hydroxide, which is a strong base. But why did NaOH go to school? Because it wanted to be a NaOtician!
Now, to calculate the pH of 0.10 M NaOH, we need to remember that pH is related to the concentration of hydrogen ions (H+) in a solution. In this case, the NaOH solution will dissociate into OH- ions.
Since NaOH is a strong base, it completely dissociates into Na+ and OH- ions in solution. So, the concentration of OH- ions in the 0.10 M NaOH solution will also be 0.10 M.
Now, to calculate the concentration of H+ ions, we can use the equation Kw = [H+][OH-], and rearrange it to [H+] = Kw / [OH-].
Plugging in the given value of Kw (4.57 x 10^-15) and the concentration of OH- (0.10), we find that [H+] = 4.57 x 10^-14 M.
To calculate the pH, we can use the equation pH = -log[H+]. Plugging in the value of [H+], we find that the pH of the 0.10 M NaOH solution is approximately 13.34.
So, just like a surprise party, the pH of 0.10 M NaOH is quite basic!
To calculate the pH of a solution, we need to know the concentration of the hydronium ion (H3O+) in the solution. In the case of NaOH, it is a strong base that completely dissociates in water to form OH- ions. Therefore, the concentration of OH- ions in the solution will be equal to the concentration of NaOH.
Given that the concentration of NaOH is 0.10 M, the concentration of OH- ions is also 0.10 M.
We can use the Kw expression to find the concentration of H3O+ ions:
Kw = [H3O+][OH-]
Substituting the given value for Kw at 15 °C, we have:
4.57 x 10^-15 = [H3O+][0.10]
Solving for [H3O+]:
[H3O+] = 4.57 x 10^-15 / 0.10
[H3O+] = 4.57 x 10^-14
Now, we can calculate the pH using the formula:
pH = -log[H3O+]
pH = -log(4.57 x 10^-14)
pH ≈ 13.36
So, the pH of the 0.10 M NaOH solution at 15 °C is approximately 13.36.
To calculate the pH of 0.10 M NaOH, we need to consider that NaOH dissociates in water to produce hydroxide ions (OH-) and sodium ions (Na+). Since NaOH is a strong base, it will dissociate completely in water.
The balanced equation for the dissociation of NaOH in water is:
NaOH (s) → Na+ (aq) + OH- (aq)
Given that the concentration of NaOH is 0.10 M, we can assume that the concentration of OH- ions is also 0.10 M.
Now, we need to find the concentration of H3O+ (also known as hydronium ions) in the solution. Since water can auto-ionize, it can dissociate into H3O+ (hydronium) and OH- (hydroxide) ions.
The auto-ionization of water can be represented by the equation:
H2O (ℓ) ⇆ H3O+ (aq) + OH- (aq)
At 15 °C, the value of Kw (the auto-ionization constant of water) is given as 4.57 x 10^-15. The Kw expression is:
Kw = [H3O+] [OH-]
We can use this information to find the concentration of H3O+ ions. Since the concentration of OH- ions is 0.10 M, we can rearrange the equation to solve for [H3O+]:
[H3O+] = Kw / [OH-]
Substituting the values into the equation:
[H3O+] = (4.57 x 10^-15) / (0.10)
Calculating this value gives us:
[H3O+] = 4.57 x 10^-14 M
Now, we can calculate the pH using the formula:
pH = -log[H3O+]
Plugging in the value of [H3O+] we found:
pH = -log(4.57 x 10^-14)
Calculating this value gives us:
pH ≈ 13.34
Therefore, the pH of a 0.10 M NaOH solution at 15 °C is approximately 13.34.
Kw = 4.57E-15 = (H3O^+)(OH^-)
(H2O^+) = (OH^-)
(H3O^+) = sqrt(Kw) and convert to pH.