A buffer solution contains 0.403 M NH4Cl and 0.276 M NH3 (ammonia). Determine the pH change when 0.069 mol KOH is added to 1.00 L of the buffer.
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
A buffer solution contains 0.403 M NH4Cl and 0.276 M NH3 (ammonia). Determine the pH change when 0.069 mol KOH is added to 1.00 L of the buffer.
The pOH of the initial buffer solution of ammonia and ammonium chloride can be calculated using equation (1),
The pH can be calculated as,
One liter of the buffer solution will contain 0.403 moles of NH4Cl and 0.276 moles of NH3. Now, 0.069 moles of KOH are added in the given buffer solution, they will reaction with NH4Cl according to the reaction,
NH4Cl + KOH → KCl + NH3 + H2O
The moles of KOH will be completely consumed in the reaction and they will convert an equal number of NH4Cl into NH3. Hence, the final number of moles of both the species can be calculated as,
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