Calculating pH of a NaCN Hints & Tips

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SUMMARY

The pH of a 0.200M Sodium Cyanide (NaCN) solution can be calculated through hydrolysis, as Sodium Cyanide dissociates into CN- ions, which act as a strong conjugate base of the weak acid HCN. The hydrolysis reaction of CN- with water produces hydroxide ions (OH-), leading to an increase in pH. To find the exact pH, one must apply the formula for the base dissociation constant (Kb) of CN- and use the relationship between pH and pOH.

PREREQUISITES
  • Understanding of acid-base chemistry, specifically the Bronsted-Lowry theory.
  • Familiarity with weak acids and their conjugate bases, particularly HCN and CN-.
  • Knowledge of hydrolysis reactions and their impact on pH.
  • Ability to calculate pH and pOH using Kb values.
NEXT STEPS
  • Research the hydrolysis of sodium cyanide and its effect on pH.
  • Learn how to calculate the base dissociation constant (Kb) for CN-.
  • Study the Bronsted-Lowry definition of acids and bases in more detail.
  • Practice calculating pH for various weak acid and conjugate base pairs.
USEFUL FOR

Chemistry students, educators, and anyone preparing for exams involving acid-base equilibria and pH calculations.

kwikness
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Hi, I have the following problem:

Calculate the pH of a 0.200M Sodium Cyanide solution.

I'm confused because this salt has no H or O atoms in it. How could it affect the pH of a solution?
What formulas would I need to solve this? My final is tomorrow and I'm really worried. Thank you for any help.
 
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