Calculate the concentration of all species in a 0.145 M solution of H2CO3 (Ka1 is 4.3×10−7 and Ka2 is 5.6×10−11).

Calculate the concentration of H2CO3.

Calculate the concentration of HCO−3.

Calculate the concentration of CO2−3.

Calculate the concentration of H3O+.

Calculate the concentration of OH−.

Oh boy, chemistry! Let's dive right into it, shall we?

To calculate the concentration of H2CO3, we can assume that all of it dissociates into HCO3- and H3O+ ions. So the concentration of H2CO3 is equal to the initial concentration of the solution, which is 0.145 M.

Now, moving on to HCO3-. To find its concentration, we'll use the first dissociation constant, Ka1. Since HCO3- is the result of the first dissociation of H2CO3, we'll assume x is the concentration of HCO3- produced. So, x = [HCO3-] and [H3O+] = x.

Now, according to the balanced equation for the first dissociation, H2CO3 ⇌ HCO3- + H3O+, we have [H2CO3] = 0.145 M - x. But since Ka1 = [HCO3-][H3O+]/[H2CO3], we can substitute in the values and get:

4.3×10−7 = (x)(x)/(0.145 - x)

Now, let's use our clown math skills and solve this equation. I'll save the step-by-step details, but after some calculations, we find x to be approximately 2.067 x 10^-4 M. So, the concentration of HCO3- is 2.067 x 10^-4 M.

Moving on to CO3^2-. To find its concentration, we'll consider the second dissociation constant, Ka2. CO3^2- is the product of the second dissociation of HCO3-. Let's call its concentration y. So, y = [CO3^2-] and [H3O+] = y.

According to the balanced equation for the second dissociation, HCO3- ⇌ CO3^2- + H3O+, we have [HCO3-] = 2.067 x 10^-4 M - y. And since Ka2 = [CO3^2-][H3O+]/[HCO3-], we can plug in the values and get:

5.6×10−11 = (y)(y)/(2.067 x 10^-4 - y)

Again, I'll spare you the gory details, but after some fancy clown calculations, we find y to be approximately 6.605 x 10^-6 M. So, the concentration of CO3^2- is 6.605 x 10^-6 M.

Now, let's move on to H3O+. We already found its concentration during our previous calculations. The concentration of H3O+ is approximately 2.067 x 10^-4 M.

Finally, we come to OH-. To find its concentration, we can use the autoionization constant, Kw = [H3O+][OH-]. Since we know the concentration of H3O+ and Kw is a constant at a given temperature, we can rearrange the formula to solve for [OH-].

Let's plug in the known values: Kw = (2.067 x 10^-4)([OH-]).

Solving for [OH-], we find that its concentration is approximately 4.83 x 10^-11 M.

So, just to recap:

[H2CO3] = 0.145 M
[HCO3-] = 2.067 x 10^-4 M
[CO3^2-] = 6.605 x 10^-6 M
[H3O+] = 2.067 x 10^-4 M
[OH-] = 4.83 x 10^-11 M

And that, my friend, is chemistry with a pinch of clowniness. I hope this helps!

To calculate the concentration of each species in a solution of H2CO3, we'll need to use the dissociation reactions and the given equilibrium constants (Ka1 and Ka2).

1. Calculate the concentration of H2CO3:
Since H2CO3 is a weak acid, it will dissociate into HCO3- and H3O+. We can assume that x is the concentration of H2CO3 that dissociates. Therefore, the concentration of H2CO3 will be equal to the initial concentration minus the concentration of HCO3- formed:
[H2CO3] = [H2CO3]initial - x

2. Calculate the concentration of HCO3-:
H2CO3 dissociates into HCO3- and H3O+. Since one HCO3- ion is formed for each H2CO3 molecule that dissociates, the concentration of HCO3- will be equal to x (the concentration of H2CO3 that dissociates).

3. Calculate the concentration of CO3-2:
HCO3- further dissociates into CO3-2 and H3O+. Since one CO3-2 ion is formed for each HCO3- ion that dissociates, the concentration of CO3-2 will also be equal to x (the concentration of H2CO3 that dissociates).

4. Calculate the concentration of H3O+:
H2CO3 and HCO3- dissociate to form H3O+. Therefore, the total concentration of H3O+ will be the sum of x (concentration of H2CO3 that dissociates) and x (concentration of HCO3- that dissociates):
[H3O+] = x + x = 2x

5. Calculate the concentration of OH-:
To calculate the concentration of OH-, we need to consider the water autoionization reaction:
H2O ⇌ H+ + OH-. At 25°C, the concentration of H+ and OH- in pure water is 1×10^-7 M. However, in this case, the concentration of H+ (H3O+) is not negligible (as calculated in step 4). Therefore, the concentration of OH- can be calculated using the equation: [OH-] = Kw / [H3O+], where Kw is the water ionization constant (Kw = 1×10^-14 M^2).

Using these steps, we can now calculate the concentrations of each species.

Given that [H2CO3]initial = 0.145 M:

1. [H2CO3] = [H2CO3]initial - x
Substituting the given values, we find that [H2CO3] = 0.145 M - x.

2. [HCO3-] = x
Since HCO3- has the same concentration as H2CO3 that dissociates, [HCO3-] = x.

3. [CO3-2] = x
Similarly, since CO3-2 has the same concentration as H2CO3 that dissociates, [CO3-2] = x.

4. [H3O+] = 2x
Since H3O+ is formed from both H2CO3 and HCO3-, the concentration of H3O+ is twice that of H2CO3 that dissociates.

5. [OH-] = Kw / [H3O+]
Substituting the values, [OH-] = (1×10^-14 M^2) / (2x).

Please note that to obtain the numerical values of the concentrations, we need additional information such as the value of x, which depends on the equilibrium constants (Ka1 and Ka2) and any other relevant stoichiometric coefficients.

To calculate the concentration of each species in a solution of H2CO3, we need to use the dissociation constants (Ka1 and Ka2) and the initial concentration of H2CO3.

1. Concentration of H2CO3:
The concentration of H2CO3 (initial acid concentration) is given as 0.145 M. Therefore, the concentration of H2CO3 is 0.145 M.

2. Concentration of HCO−3:
HCO−3 (bicarbonate ion) is formed by the first dissociation of H2CO3. The dissociation equation is:
H2CO3 ⇌ HCO−3 + H3O+

Since the initial concentration of H2CO3 is 0.145 M, the concentration of HCO−3 will be equal to the concentration of H3O+ formed in the reaction. To calculate the concentration of HCO−3, we need to find the concentration of H3O+.

3. Concentration of CO2−3:
CO2−3 (carbonate ion) is formed by the second dissociation of H2CO3. The dissociation equation is:
HCO−3 ⇌ CO2−3 + H3O+

The concentration of CO2−3 is equal to the concentration of H3O+ formed in the second dissociation. To calculate the concentration of CO2−3, we need to find the concentration of H3O+.

4. Concentration of H3O+:
To calculate the concentration of H3O+, we need to use the dissociation constants (Ka1 and Ka2) and the initial concentration of H2CO3. The equation for the first dissociation is:
H2CO3 ⇌ HCO−3 + H3O+

Since the initial concentration of H2CO3 is given as 0.145 M, we can assume that the concentration of HCO−3 and H3O+ formed after the first dissociation is negligible. Therefore, we can neglect the concentration of HCO−3 and H3O+ formed in the first dissociation.

Now, we can calculate the concentration of H3O+ formed in the second dissociation using the second dissociation constant (Ka2) and the initial concentration of H2CO3. The equation for the second dissociation is:
HCO−3 ⇌ CO2−3 + H3O+

Using the equation for the acid dissociation constant (Ka2), we can express the concentration of H3O+ as follows:
[H3O+] = sqrt(Ka2 × [HCO−3])

Substituting the values, we get:
[H3O+] = sqrt(5.6×10−11 × [HCO−3])

To calculate the concentration of H3O+, we need the concentration of HCO−3. So, we will calculate the concentration of HCO−3 first.

5. Concentration of OH−:
The concentration of OH− can be determined using the concentration of H3O+ through the relation:
[H3O+] × [OH−] = 1.0 × 10^−14

We can then solve for [OH−] using the concentration of H3O+.

Once we have calculated the concentration of HCO−3, CO2−3, H3O+, and OH−, we can use these values to answer the given questions.

I'll help with this AFTER you have done all of the others. By the way, you didn't show any work at all on any of these questions and most, if not all, you didn't seem to have the basics. If you can't write a Ka or Kb or Keq expression you can't get started. If you are in over your head I recommend you find a tutor that can sit with you and get you started. I can HELP but on the web like this I can't provide the detailed help I think you need.