Suppose you have just added 100 ml of a solution containing 0.5 mol of acetic acid per liter to 400 ml of 0.5 m naoh. what is the final ph? (the pka of acetic acid is 4.7.)

Explanation:

Sodium hydroxide completely ionizes in water to produce sodium ions and hydroxide ions. Hydroxide ions are in excess and neutralize all acetic acid added by the following ionic equation:

The mixture would contain

if undergoes no hydrolysis; the solution is of volume after the mixing. The two species would thus be of concentration and , respectively.

Construct a RICE table for the hydrolysis of under a basic aqueous environment (with a negligible hydronium concentration.)

The question supplied the acid dissociation constant for acetic acid ; however, calculating the hydrolysis equilibrium taking place in this basic mixture requires the base dissociation constant for its conjugate base, . The following relationship relates the two quantities:

... where the water self-ionization constant under standard conditions. Thus . By the definition of :

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.

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