The pH of a .200M HBrO solution is 4.67. What is the acids Ka?

[H3O+]=10-4.67 = [BrO-]

[HBrO]=0.200-10-4.67

Ka=[H3O+][BrO-]/[HBrO]=2.286×10^(-9)

Well, it seems like HBrO has a bit of a sour attitude with a pH of 4.67! But don't worry, I'm here to help you find its Ka.

To find the acid's Ka, we first need to find the concentration of the hydrogen ions (H+). Since the pH of the solution is given, we can convert it back into a concentration using the equation pH = -log[H+].

So, by plugging in the pH value of 4.67, we find that [H+] = 10^(-4.67).

Now, since HBrO is a weak acid, we can assume that the concentration of the H+ ions formed is equal to the concentration of HBrO that ionizes:

[H+] = [HBrO]

Given that the concentration of HBrO is 0.200 M, we can now substitute this value into the expression for Ka:

Ka = [H+][BrO-] / [HBrO]

Since the concentration of H+ and HBrO are the same, we can simplify the equation to:

Ka = [H+]² / [HBrO]

Substituting the values we found earlier, the equation becomes:

Ka = (10^(-4.67))^2 / 0.200

Now, if you crunch those numbers, you'll find the value of Ka for the HBrO acid. Just remember to bring a calculator and maybe a bag of popcorn, because math can be fun!

To find the acid dissociation constant (Ka) of a weak acid, we can use the pH of the solution and the concentration of the acid. The pH gives us the concentration of H+ ions, and since HBrO is a weak acid, we can assume that it dissociates according to the following equilibrium reaction:

HBrO ⇌ H+ + BrO-

The equilibrium constant expression is:

Ka = [H+][BrO-] / [HBrO]

Given that the concentration of HBrO is 0.200 M and the pH is 4.67, we can calculate the concentration of H+ as follows:

pH = -log[H+]
10^(-pH) = [H+]
10^(-4.67) = [H+]

Now, since H+ and BrO- are produced in a 1:1 ratio, we can substitute the concentration of H+ into the equilibrium constant expression to find Ka:

Ka = [H+][BrO-] / [HBrO]
Ka = (10^-4.67)(10^-4.67) / (0.200)
Ka = 2.17 x 10^-10

Therefore, the Ka of the HBrO solution is 2.17 x 10^-10.

To find the acid's Ka (acid dissociation constant) for HBrO, we can use the given pH of the solution.

Step 1: Determine the concentration of H3O+ ions
Since the pH is given, we can convert it to [H3O+] (concentration of hydronium ions) using the formula: [H3O+] = 10^(-pH)
In this case, the pH is 4.67, so [H3O+] = 10^(-4.67).

Step 2: Determine the concentration of the undissociated acid (HBrO)
Since the initial concentration of HBrO is given as 0.200 M, we can consider it the same as the equilibrium concentration of the acid because we assume complete dissociation.

Step 3: Determine the concentration of dissociated ions (BrO-)
Again, since we assume complete dissociation, the concentration of BrO- ions will be the same as the concentration of H3O+ ions, which we determined in step 1.

Step 4: Write the balanced chemical equation for the dissociation of the acid.
HBrO ⇌ H+ + BrO-

Step 5: Set up the expression for Ka.
Ka = [H+][BrO-]/[HBrO]

Step 6: Substitute the values into the Ka expression.
Ka = ([H3O+])([BrO-])/([HBrO])
Ka = ([H3O+])([H3O+])/([HBrO])

Step 7: Substitute the concentration values into the Ka expression.
Ka = (10^(-4.67))(10^(-4.67))/(0.200)

Step 8: Calculate the value of Ka.
Using a scientific calculator or computer software, calculate the value of Ka by performing the above calculation.
Ka ≈ 1.25 x 10^(-9)

Therefore, the approximate Ka value for the HBrO acid is 1.25 x 10^(-9).