**A pKa to KA calculator is a useful tool in chemistry that helps convert between two important measures of acid strength: pKa and Ka. **

**pKa**, or the **negative logarithm of the acid dissociation constant**, is a measure of how easily an acid gives up a proton. On the other hand, **Ka**, or the **acid dissociation constant**, directly represents the extent to which an acid dissociates in an aqueous solution.

## Convert pKa to KA Calculator

This calculator converts between pKa and Ka.

pKa | Ka |
---|---|

4.76 | 1.74 × 10^(-5) |

3.00 | 1.00 × 10^(-3) |

7.50 | 3.16 × 10^(-8) |

9.25 | 5.62 × 10^(-10) |

2.15 | 7.08 × 10^(-3) |

To calculate these values, we used the formula:

**Ka = 10^(-pKa)**

For example, for the first row: Ka = 10^(-4.76) = 1.74 × 10^(-5)

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## pKa to KA Conversion Formula

The relationship between pKa and Ka is defined by a simple logarithmic equation:

**pKa = -log₁₀(Ka)**

Conversely, to calculate Ka from pKa, we use the inverse logarithmic function:

**Ka = 10^(-pKa)**

These formulas form the basis of any pKa to KA calculator, allowing for quick and accurate conversions between the two values.

## How do you convert pKa to KA?

Converting pKa to Ka involves a few simple steps:

**Start with the pKa value**you want to convert.**Recognize the relationship**: pKa = -log₁₀(Ka)**Rearrange the equation**to solve for Ka: Ka = 10^(-pKa)**Use a calculator**to compute 10 raised to the power of the negative pKa value.

For example, if you have a pKa of 4.5: Ka = 10^(-4.5) = 3.16 × 10^(-5)

This process can be easily automated using a KA to pKa calculator, which performs these calculations instantly.

## What is the pKa of 4.76 to Ka?

Let’s apply the conversion process to a specific example:

Given pKa = 4.76, we need to find Ka.

Using the formula Ka = 10^(-pKa):

Ka = 10^(-4.76) Ka = 1.74 × 10^(-5)

Therefore, a pKa of 4.76 corresponds to a Ka of 1.74 × 10^(-5).

This value indicates that the acid is relatively weak, as it has a small Ka value (much less than 1), meaning it doesn’t dissociate extensively in solution.

## How is pKa different to Ka?

pKa and Ka both describe acid strength, they differ in several key aspects:

**Scale**: Ka is a direct measure of the acid dissociation constant, while pKa is a logarithmic scale.**Range**: Ka values can span many orders of magnitude (e.g., 10^(-15) to 10^(15)), while pKa values typically range from about -2 to 16 for common acids.**Interpretation**: A**higher Ka**indicates a**stronger acid**, whereas a**lower pKa**indicates a**stronger acid**.**Ease of use**: pKa values are often easier to work with due to their more manageable range.**Logarithmic nature**: pKa represents the negative logarithm of Ka, similar to how pH represents the negative logarithm of hydrogen ion concentration.

## Is Ka directly proportional to pKa?

No, Ka is **not directly proportional** to pKa. Instead, they have an **inverse logarithmic relationship**.

As pKa increases:

- Ka decreases exponentially
- The acid becomes weaker

As pKa decreases:

- Ka increases exponentially
- The acid becomes stronger

## How to Calculate Ka and pKa from pH and Concentration

Let’s focus on weak acids for this explanation.

- pH = 4.5
- Initial concentration (C₀) = 0.1 M
**Calculate [H⁺]:**[H⁺] = 10^(-4.5) = 3.16 × 10^(-5) M**Calculate [A⁻]:**[A⁻] = [H⁺] = 3.16 × 10^(-5) M**Calculate [HA]:**[HA] = 0.1 – (3.16 × 10^(-5)) ≈ 0.1 M**Calculate Ka:**Ka = (3.16 × 10^(-5))² / 0.1 = 1.00 × 10^(-8)**Calculate pKa:**pKa = -log₁₀(1.00 × 10^(-8)) = 8.00

Therefore, for this weak acid solution:

**Ka = 1.00 × 10^(-8)****pKa = 8.00**