If we mix a weak acid (HA) with its conjugate base (A-), both the acid and base components remain present in the solution. If a strong base is added to a buffer, the weak acid will give up its H+ in order to transform the base (OH-) into water (H2O) and the conjugate base: HA + OH- → A- + H2O.

A weak acid will react with a strong base to form a basic (pH > 7) solution.

The procedure for calculating the pH of a solution of a weak base is similar to that of the weak acid in the example. However, the variable x will represent the concentration of the hydroxide ion. The pH is found by taking the negative logarithm to get the pOH, followed by subtracting from 14 to get the pH.

Sodium hydroxide, a chemical compound with the formula NaOH, is known to be a strong base. This is because sodium hydroxide undergoes almost complete ionization when it is dissolved in water. Weak bases are the basic substances that do not completely ionize in water. An example of a weak base is ammonia.

The 7 common strong acids are: HCl, HBr, HI, HNO3, HClO3, HClO4 and H2SO4 (1st proton only).

any acid that is not one of the seven strong is a weak acid (e.g. H3PO4, HNO2, H2SO3, HClO, HClO2, HF, H2S, HC2H3O2 etc.) 2. solutions of weak acids have a low concentration of H+. the molecular form of the weak acid does exist in solution.

HClO3 and HClO4 are strong acids due to the multiple oxygens bonded to the central atom. HClO2, however, is a weak acid.

Solubility of Ba(OH)2 is much higher than Sr(OH)2. So more OH- amount can be given by Ba(OH)2 to the aqueous solution. Therefore, Ba(OH)2 is a strong base than Sr(OH)2.

Classifying Electrolytes