The formula to calculate K_{a} from the pK_{a} value is –

∴ K_{a} = 10^{-pKa}

pKa to Ka calculator

pK_{a} to K_{a} Calculator

[K_{a}] =

Step by Step Solution:

To determine [K_{a}], you can use the formula given below:

⇒ [K_{a}] = 10^{-pKa}

Given that,

⇒ pK_{a} =

Substitute the pK_{a} value into the formula:

∴ [K_{a}] = 10^{-()}

∴ [K_{a}] =

How to use pK_{a} to K_{a} calculator?

Using the above calculator you can easily convert the pK_{a} value to K_{a}.

Enter a pK_{a} value in the input field labeled “pK_{a} value =”.

Click the “Calculate” button.

The result [K_{a}] will be displayed in the “result” section with Step by Step solution.

How to calculate K_{a} from pK_{a}?

pK_{a} is the negative logarithm of K_{a} to the base 10 as shown in the formula given below:

∴ pK_{a} = -log_{10}(K_{a})

Above equation can be transferred by taking antilog –

∴ K_{a} = 10^{-pKa}

Example of calculating K_{a} value using “pK_{a} to K_{a} calculator”

Let’s say we have given the value of pK_{a} and we need to calculate the K_{a} value.

For example – If the pK_{a} value = 3.14, what is the [K_{a}] value?

As we know, the formula to convert pK_{a} to K_{a} is –

∴ K_{a} = 10^{-pKa}

So, just put the value of pK_{a} in the respective field and then press calculate button.

∴ So, The acid dissociation constant (K_{a}) for the given pK_{a} value is 0.000724 or 7.24 x 10^{-4}.

Numericals based on “Converting pK_{a} value to K_{a}“

What is the value of the acid dissociation constant (K_{a}) for the acidic solution, given its pK_{a} value of 11.62?

To find the value of the acid dissociation constant (K_{a}) for the acidic solution, we can use the equation given below –

⇒ K_{a} = 10^{-pKa}

We have given, the pK_{a} value which is 11.62

∴ [K_{a}] = 10^{-11.62}

= 2.40 x 10^{-12}

So, the acid dissociation constant (K_{a}) for the given pK_{a} value is 2.40 x 10^{-12}

The pK_{a} for acetic acid is 4.80. What is the K_{a} value for acetic acid?

As the pK_{a} value for acetic acid is given in the question statement. So we can substitute it into the equation given below to find K_{a} as follows.

∴ K_{a} = 10^{-pKa}

∴ K_{a} = 10^{-4.80} = 1.58 x 10^{-5}.

So, the acid dissociation constant (K_{a}) value for the given pK_{a} of acetic acid is 1.58 x 10^{-5}.

Vishal Goyal is the founder of Topblogtenz, a comprehensive resource for students seeking guidance and support in their chemistry studies. He holds a degree in B.Tech (Chemical Engineering) and has four years of experience as a chemistry tutor. The team at Topblogtenz includes experts like experienced researchers, professors, and educators, with the goal of making complex subjects like chemistry accessible and understandable for all. A passion for sharing knowledge and a love for chemistry and science drives the team behind the website. Let's connect through LinkedIn: https://www.linkedin.com/in/vishal-goyal-2926a122b/

Topblogtenz is a website dedicated to providing informative and engaging content related to the field of chemistry and science. We aim to make complex subjects, like chemistry, approachable and enjoyable for everyone.