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9. To prepare a basic buffer of pH=10 how many grams of NH,Cl would you add to 100 ml of 0.1 M NH¸OH ? (K,(NH,OH) =1.84-10³ mol/L; molar mass of NH,Cl = 53.5 g/mol). %3D

9. To prepare a basic buffer of pH=10 how many grams of NH,Cl would you add to 100 ml of 0.1 M NH¸OH ? (K,(NH,OH) =1.84-10³ mol/L; molar mass of NH,Cl = 53.5 g/mol). %3D

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter17: Principles Of Chemical Reactivity: Other Aspects Of Aqueous Equilibria
Section17.2: Controlling Ph: Buffer Solutions
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9. To prepare a basic buffer of pH=10 how many grams of NH,Cl would you add to 100 ml of 0.1 M NH¸OH ? (K,(NH,OH) =1.84-10³ mol/L; molar mass of NH,Cl = 53.5 g/mol). %3D
Transcribed Image Text:9. To prepare a basic buffer of pH=10 how many grams of NH,Cl would you add to 100 ml of 0.1 M NH¸OH ? (K,(NH,OH) =1.84-10³ mol/L; molar mass of NH,Cl = 53.5 g/mol). %3D
Expert Solution
Step 1

 

The Henderson Hasselbalch equation for basic buffer is given as:

Chemistry homework question answer, step 1, image 1
Step 2

Given,

pH basic buffer solution = 10

Volume of solution = 100 mL = 0.1 L (1 mL = 0.001 L)

Molarity of NH4OH (base) = 0.1 M

Kb of NH4OH = 1.84 × 10-5 mol/L = 1.84 × 10-5 M

Molar mass of NH4Cl = 53.5 g/mol

The pOH of the solution and pKb can be calculated as :

Chemistry homework question answer, step 2, image 1
Step 3

The concentration of the salt (NH4Cl) can be calculated from Henderson Hasselbalch equation as :

Chemistry homework question answer, step 3, image 1
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