0.1 N solurion of sodium bicarbonate has a ph value of?

Question

Answer

PH = (pKa1 + pKa2)/2. where Ka1 & Ka2 are dissociation constants of the conjugate acid of amphiprotic species.For NaHCO3, pH is (6.37 + 10.25)/2 = 8.31

Answer

pH of 0.1 N Sodium Bicarbonate Solution

A 0.1 N sodium bicarbonate (NaHCO3) solution has a pH value of approximately 8.3. This can be explained by considering the chemical properties of sodium bicarbonate and its interaction with water.

Chemical Properties of Sodium Bicarbonate

Sodium bicarbonate is a weak base that can act as a buffer in aqueous solutions.

It is an amphiprotic compound, meaning it can both accept and donate protons.

When dissolved in water, sodium bicarbonate dissociates into sodium ions (Na+) and bicarbonate ions (HCO3-).

Ionization of Sodium Bicarbonate in Water

When sodium bicarbonate is added to water, it undergoes partial ionization. The following equilibrium reaction occurs:

NaHCO3 ⇌ Na+ + HCO3-

The bicarbonate ion (HCO3-) can act as a weak base by accepting a proton from water, leading to the formation of a hydroxide ion (OH-):

HCO3- + H2O ⇌ H2CO3 + OH-

The carbonic acid (H2CO3) formed in the reaction above is unstable and readily dissociates into water and carbon dioxide (CO2):

H2CO3 ⇌ H2O + CO2

Role of Bicarbonate Ions in pH

The bicarbonate ions (HCO3-) formed through the ionization of sodium bicarbonate are responsible for the pH of the solution. Bicarbonate ions can act as a weak base and can accept protons from water, leading to the formation of hydroxide ions (OH-).

The presence of hydroxide ions increases the concentration of hydroxide ions in the solution, which in turn increases the pH. pH is a measure of the concentration of hydrogen ions (H+) in a solution, and it is calculated using the negative logarithm of the H+ concentration.

pH Calculation

The pH of a 0.1 N sodium bicarbonate solution is approximately 8.3.

Summary

In summary, a 0.1 N sodium bicarbonate solution has a pH of around 8.3. This can be attributed to the ionization of sodium bicarbonate in water, leading to the formation of bicarbonate ions, which can accept protons from water and increase the concentration of hydroxide ions. The presence of hydroxide ions raises the pH of the solution.

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