Calculate [H3O ], [ClO4–], and [OH–] in an aqueous solution that is 0.170 M in HClO4(aq) at 25 °C.

Well, let's dive into the world of chemistry! To calculate the concentrations of different ions in the solution, we'll need to use some equations and a touch of math.

First, HClO4(aq) is a strong acid that completely dissociates in water. This means that it breaks apart into ions when it dissolves. In this case, HClO4(aq) fully dissociates into H3O+(aq) and ClO4–(aq).

Since the concentration of HClO4(aq) is given as 0.170 M, the concentration of H3O+(aq) will also be 0.170 M. So, [H3O+] = 0.170 M.

Now, let's talk about the hydroxide ion (OH–). In pure water at 25 °C, the concentration of OH– is 1.0 x 10^-7 M. However, in this case, we have a strong acid (HClO4) present, which also has the potential to generate H3O+ ions.

Since we're dealing with a strong acid, it will dominate the solution by adding H3O+ ions. As a result, the concentration of OH– will be negligible. So, [OH–] ≈ 0.

Lastly, let's talk about ClO4–. Since HClO4(aq) fully dissociates, the concentration of ClO4– will also be equal to the initial concentration of HClO4(aq), which is 0.170 M. So, [ClO4–] = 0.170 M.

I hope that chemistry humor didn't make your brain explode! Let me know if you have any more questions.

To calculate the concentrations of H3O+, ClO4-, and OH- in the given aqueous solution, we need to consider the dissociation of HClO4.

HClO4(aq) → H+(aq) + ClO4-(aq)

In this case, HClO4 is a strong acid, which means it dissociates completely in water.

Step 1: Determine the concentration of H+ ions

Since HClO4 dissociates completely, the concentration of H+ ions is the same as the concentration of HClO4.
[H+] = 0.170 M

Step 2: Determine the concentration of ClO4- ions

Since HClO4 dissociates completely, the concentration of ClO4- ions is also the same as the concentration of HClO4.
[ClO4-] = 0.170 M

Step 3: Determine the concentration of OH- ions

To find the concentration of OH- ions, we need to use the Kw expression at 25 °C, which is the product of the concentrations of H+ and OH- ions.

Kw = [H+][OH-]

Since the solution is acidic due to the presence of HClO4, the concentration of OH- ions is expected to be very low.
Assuming x M is the concentration of OH-, we can ignore the x value compared to 0.170 M for H+, which means we can approximate [H+] as 0.170 M.

Kw = (0.170)(x)
1.0 x 10^-14 = 0.170x
x = (1.0 x 10^-14) / 0.170
x ≈ 5.88 x 10^-14 M

Thus, [OH-] ≈ 5.88 x 10^-14 M

To summarize the results:
[H3O+] = [H+] = 0.170 M
[ClO4-] = 0.170 M
[OH-] ≈ 5.88 x 10^-14 M

To calculate the concentrations of H3O+, ClO4-, and OH- in the given aqueous solution, you'll need to consider the dissociation of HClO4.

HClO4 is a strong acid that completely dissociates in water, which means that it dissociates into H3O+ and ClO4-. The balanced chemical equation for this dissociation is:

HClO4(aq) + H2O(l) -> H3O+(aq) + ClO4-(aq)

Since the solution is 0.170 M in HClO4, the concentration of H3O+ will also be 0.170 M.

However, ClO4- is not included in the initial solution but is produced through the dissociation of HClO4. So, the concentration of ClO4- is also 0.170 M.

Since HClO4 is an acid, it donates a proton (H+) in water, resulting in an increase in the concentration of H3O+, but a decrease in the concentration of OH-. To calculate the concentration of OH-, we can use the concept of the autoionization of water.

In water, a small fraction of water molecules self-ionize, leading to the formation of H3O+ and OH-. The balanced chemical equation for this autoionization is:

2H2O(l) -> H3O+(aq) + OH-(aq)

At 25 °C, the concentration of H3O+ and OH- in pure water is 1.0 x 10^(-7) M. However, in this case, the concentration of H3O+ is higher due to the presence of the strong acid HClO4.

To calculate the concentration of OH- in the solution, we can use the Kw expression, which represents the equilibrium constant for the autoionization of water:

Kw = [H3O+][OH-] = 1.0 x 10^(-14) M^2

We already know that the concentration of H3O+ is 0.170 M. By rearranging the equation, we can solve for the concentration of OH-:

[OH-] = Kw / [H3O+]

[OH-] = (1.0 x 10^(-14) M^2) / (0.170 M)

Calculating the value, the concentration of OH- in the given aqueous solution is approximately 5.88 x 10^(-14) M.

HClO4 is a strong acid meaning that it ionizes 100%; therefore,

HClO4 ==> H^+ + ClO4^-
0.170.....0.......0
-0.170...0.170..0.170
...0.....0.170...0.170
This gives the (H^+) [which is the same as H3O^+].
You can obtain OH by
(H^+)(OH^-) = Kw = 1E-14.