Calculate Moles of CH3NH2 Needed for pH 9.55: Buffer Solution

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SUMMARY

To achieve a pH of 9.55 in a buffer solution, 319 grams of CH3NH3ClO4 must be added to 800 ml of 0.258 M CH3NH2. The calculation utilizes the Henderson-Hasselbalch equation and considers the Kb value of methylamine, which is 4.2 x 10^-4. The volume of the solution is assumed to remain constant during the process.

PREREQUISITES
  • Understanding of the Henderson-Hasselbalch equation
  • Knowledge of buffer solutions and their components
  • Familiarity with Kb values and their significance in pH calculations
  • Basic skills in stoichiometry for calculating moles and grams
NEXT STEPS
  • Study the Henderson-Hasselbalch equation in detail
  • Learn about buffer capacity and how to calculate it
  • Explore the properties of methylamine and its applications in buffer solutions
  • Investigate the effects of temperature on buffer pH stability
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Chemistry students, laboratory technicians, and anyone preparing for exams on buffer solutions and pH calculations.

alingy2
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You want to have a ph of 9.55 with a buffer. How many grames of CH3NH3ClO4 would you add to 800 ml of 0.258 M CH3NH2 to do this. Assume volume remains constant. Kb for methylamine is 4.2x10^-4.

My answer is 320g. Can anyone check this please? I have an exam on buffers very fast. You would do me a great favor.
I used Henderson to find concentration of methylamine required. Then the number of moles and grams.
 
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I got 319 g, close enough.
 

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