Problem: Complete this table of values for four aqueous solutions at 25  °C.

FREE Expert Solution

The pH and pOH of a compound determine its acidity and basicity.

• pH

▪ pH stands for the negative logarithmic function of hydronium ion concentration
can be calculated using the following equation:


pH=-log H+

Take note that:         [H+] = [H3O+]


• pOH

▪ pOH stands for the negative logarithmic function of hydroxide concentration
can be calculated using the following equation:

pOH=-log OH-


The relationship between pH and pOH is connected by the following equation:

pH+pOH=14


On the other hand, if the pH and pOH are given:

The H+ or H3O+ concentration can be calculated using the following equation:

H+=10-pH

The OH- concentration can be calculated using the following equation:

OH-=10-pOH

The relationship between [H+] and [OH-] is connected by the following equation:

Kw=H+OH-

Kw = autoionization constant of water

Kw = 1.0x10-14 at T = 25°C

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Problem Details

Complete this table of values for four aqueous solutions at 25  °C.

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