As a rule of thumb, if the [ H3O ] is less than 1% of the value of the [Acid], it does not have to be considered when figuring the concentration of the acid. Use your results in

Explanation:

In strong acids, we see how the [H3O+] comes close to be equal to the concentration of the acid. Whereas in the weak acids, the [H3O+] is appears to be far less than the concentration of the acid.

One of the ways to define and measure the relative strengths of a series of acids is to measure the pH of solutions of acids of equal concentration which is ideal: remembering that the lower the pH, the greater the concentration of hydronium ion, the stronger the acid. Let's check few more variations;

• in a strong monoprotic acid, the [H30+] in solution is equal to the original acid concentration.

• in a weak acid, the [H3O+] is lesser than the original acid concentration. Simply put that the [H3O+] is smaller than if the acid were to be a strong acid of the same concentration.

• In series of weak monoprotic acids (of the category HA) of the same concentration, here we see how the [H30+] increases (while the pH declines) as the acids become stronger.

Other concepts relevant to this discuss is thus;

• the equilibrium constant for the reaction of a weak base with water is the base ionization constant (Kb).

• for any conjugate acid–base pair, KaKb=Kw.

• smaller values of pKa relates that it gives a larger acid ionization constants and hence stronger acids.

• some acids or bases are listed as having Ka, or Kb, values that are large or very small.

• when aqueous acids are stronger than H3O+ they are completely ionized (HNO3, for example), invariably meaning that their K, values are "large."

• meaning that their conjugate bases (e.g NO3 ) do not produce meaningful concentrations of OH ions, so its Kb values is "very small."

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