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Titration Notes

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What is a titration?

  • It is procedure that is commonly used to determine the amount of acid or base in a solution.
  • Solution of known concentration (titrant) is delivered to a solution being analyzed (analyte).
  • Acid-base indicators can be used to signal the equivalence point of a titration.
    • At this point, moles of acid = moles of base

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Acid-base Indicators

Phenolphthalein

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Acid-base Indicators

Bromothymol Blue

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Titration �set-up

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Types of Titrations PAP only �

There are three major types of titrations:

  • Strong Acid – Strong Base
    • Example – NaOH (aq) + HCl (aq)
  • Strong Base – Weak Acid
    • Example – NaOH (aq) + HC2H3O2 (aq)
  • Strong Acid – Weak Base
    • Example – HCl (aq) + NH3 (aq)

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Strong vs. Weak Acids

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  • Bond strength determines how easily an acid can ionize in solution.
  • The stronger the bond the harder it is to ionize, the weaker the bond the easier it is to ionize.

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  • Strong Acids have weak bond strengths. They have a loose hold on their protons.
  • They will break apart completely in water to make ions.

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Picture:

    • Conduct electricity well
    • Strong electrolytes
    • Give up Protons very easy

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  • Weak Acids have a strong bond strength. They have a tighter hold on their proton. Weak acids will only partially dissociate.

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  • Picture:

 

    • Partially conduct electricity (glows dimly)
    • Weak electrolyte
    • Does not give up all Protons well.

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