Tables of Ka and and Kb values
From ChemPRIME
The Acid Constants for Some Acids at 25°C.
Above is a table of Ka values which define the extent to which an acid will donate its proton to water. The values of the constant is defined by the equation:
![K_{c}\text{ }\times \text{ 55}\text{.5 mol dm}^{-\text{3}}=K_{a}=\frac{\text{ }\!\![\!\!\text{ H}_{\text{3}}\text{O}^{\text{+}}\text{ }\!\!]\!\!\text{ }\!\![\!\!\text{ A}^{-}\text{ }\!\!]\!\!\text{ }}{\text{ }\!\![\!\!\text{ HA }\!\!]\!\!\text{ }}](../../../../../math/6/9/0/69001b3ab17fd5ed65108a7dc89f4a6e.png)
The Base Constants for Some Bases at 25°C.
Above is a table of Kb values which define the extent to which an base will accept a proton from water. The value of the constant, similar to above, is defined as:
![K_{c}\text{ }\times \text{ 55}\text{.5 mol dm}^{-\text{3}}=K_{b}=\frac{\text{ }\!\![\!\!\text{ BH}^{\text{+}}\text{ }\!\!]\!\!\text{ }\!\![\!\!\text{ OH}^{-}\text{ }\!\!]\!\!\text{ }}{\text{ }\!\![\!\!\text{ B }\!\!]\!\!\text{ }}](../../../../../math/b/5/8/b588e18f10995f206db8fd5e3215883c.png)
