# How many grams of dry NH4Cl need to be added to 2.50 L of a 0.500 M solution of ammonia, NH3, to prepare a buffer soluti...

How many grams of dry NH4Cl need to be added to 2.50 L of a 0.500 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.74? Kb for ammonia is 1.8*10^-5.

Concepts and reason

Buffer:

A buffer is a chemical solution that contains a weak acid/base mixed with its conjugate base/acid (as in the form of salts). It can resist change when a small amount of a strong acid/base is added to it. The acidic buffer solution is made up of less than and the alkali buffer solution is made up of more than .

Fundamentals

Henderson-Hasselbalch equation is a mathematical expression which can be used to calculate the of buffer solutions.  Concentration of acid and base can be calculated as follows: Write the Henderson-Hasselbalch equation of basic buffer calculation.  Concentration of acid and base can be calculated as follows: The reaction for given buffer solution can be written as follows Given data: So, Then of given solution can be calculated as follows Henderson-Hasselbalch was used for calculating the mass of as given below, the values of were substituted in Henderson-Hasselbalch equation. Then Finally The mole of ammonium chloride was calculated as follows: The mass of ammonium chloride is calculated as follows: Ans:

The mass of is .

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