What is the relationship between pKa pKb and pKw?

If we take (–log) of both sides, we will get: pKa + pKb = pKw =14 Page 3 A very important conclusion can be drawn from the above equation. If pKa of an acid is lower then its conjugate base must have higher pKb and vise versa, which means strong acid has a weak conjugate base.

What is the relationship between pKa pKb and pKw for a conjugate acid-base pair?

The smaller pKa, the stronger the acid. The smaller pKb, the stronger the base. Usually pKa is reported for acids and bases – for bases it refers to the conjugate pair.

Why does pKa pKb pKw?

The lower the pKa of the acid, the higher the pKb of its conjugate base. So, when we make sure to use an acid/conjugate pair in this equation, it makes perfect sense that the sum of the pKa of the acid and the pKb of the conjugate base would always be the same quantity (pKw).

What is pKw equal to?

pKw = pH + pOH. As [H3O+] equals [OH-], then pH must equal pOH because these are just the negative logs of the respective concentrations, which are equal. Therefore, the equation becomes pKw = pH + pH = 2 x pH.

What is the relationship between pKa and pKb values where Ka KB represent ionization constants of the acid and its conjugate base respectively?

pKa+pKb=pKw=14. Was this answer helpful?

How are Ka KB and KW related?

To summarize: Ka * Kb is equivalent to adding the acid and base reactions together, which results in a net equation of the autoionization of water. It’s not a neutralization/acid-base reaction, but I think the Kw = Ka * Kb is a mathematical relation made to expedite calculations.

How do you find pKw?

pKw = pH + pOH. As [H3O+] equals [OH-], then pH must equal pOH because these are just the negative logs of the respective concentrations, which are equal. Therefore, the equation becomes pKw = pH + pH = 2 x pH. Therefore, pH = pKw/2.

Is pKw always 14?

Kw is the equilibrium constant for autoprotolysis of water and represents the fact that the concentration of hydronium ions times the concentration of hydroxide ions will always equal 1.0 * 10-14. pKw is the negative log base 10 of Kw, so yes, it always equals 14, whether a solution is basic or acidic.

What is mean by pKw?

noun. automobile, a vehicle steered by a driver.

How are pKa and pKb values related to strength of acids and bases?

A large Kb value indicates the high level of dissociation of a strong base. A lower pKb value indicates a stronger base. pKa and pKb are related by the simple relation: pKa + pKb = 14.