Help Needed: Balancing pH of Acetic Acid & NaOH Mixture

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SUMMARY

The pH of a mixture containing 30ml of 0.1M acetic acid and 30ml of 0.1M NaOH can be calculated by first determining the moles of each reactant. The reaction between acetic acid (HC₂H₃O₂) and sodium hydroxide (NaOH) produces sodium acetate (CH₃COONa) and water. Given the concentrations and volumes, the moles of acetic acid and NaOH are equal, leading to complete neutralization and the formation of a buffer solution. The resulting pH can be calculated using the Henderson-Hasselbalch equation, factoring in the dissociation constant of acetic acid, which is 1.8 x 10-5.

PREREQUISITES
  • Understanding of acid-base reactions
  • Knowledge of molarity and moles
  • Familiarity with the Henderson-Hasselbalch equation
  • Basic concepts of buffer solutions
NEXT STEPS
  • Calculate the pH of buffer solutions using the Henderson-Hasselbalch equation
  • Explore the concept of buffer capacity and its implications
  • Learn about the dissociation constants of weak acids
  • Investigate the effects of dilution on pH in acid-base mixtures
USEFUL FOR

Chemistry students, laboratory technicians, and anyone involved in acid-base chemistry or buffer solution preparation will benefit from this discussion.

Pengwuino
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I have a question here and i don't really know how to do it.

I need to know : What is the pH of a mixture of 30ml 0.1M acetic acid and 30ml of 0.1M NaOH? [tex]\[HC_2 H_3 O_3 = 1.8*10^{ - 5} \][/tex]

I'm not even sure what the equilibrium equation would be! Any help would be appreciated.
 
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Pengwuino, notice you have an acid (acetic acid) and a base (NaOH) .
  • Initially, how many moles of each are there?
  • When they react, what product will they form?
  • How many moles of acid and base react, and how many moles of product is formed?
  • So after, the reaction what happens to the product?

Figure out the answers to the above questions, and you are half way to the required answer.
 

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