Help Needed: Balancing pH of Acetic Acid & NaOH Mixture

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To find the pH of a mixture of 30ml 0.1M acetic acid and 30ml 0.1M NaOH, first calculate the moles of each component: 0.1M acetic acid yields 0.003 moles and 0.1M NaOH also yields 0.003 moles. When these react, they form water and sodium acetate, neutralizing each other in a 1:1 ratio. After the reaction, the resulting solution contains sodium acetate, which can affect the pH depending on its dissociation in water. The final pH can be determined by considering the equilibrium of the acetate ion in solution.
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? \[HC_2 H_3 O_3 = 1.8*10^{ - 5} \]

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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