8A : Consider the titration, 10 mL of NaCN(Ka=4.9X10^-10) with
.380M HCl. Calculate pH at 0.0mL...
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8A : Consider the titration, 10 mL of NaCN(Ka=4.9X10^-10) with.380M HCl. Calculate pH at 0.0mL HCl, 11.82mL HCl.
8B How many mL HCl is needed to reach the equivalence point andwhat is the pH at this point?
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3.7 Ratings (359 Votes)
First of all I think the concentration of the NaCN solution is missing here because we can not know the pH of this solution without knowing the amount of NaCN dissolved in 10 ml of solvent If you are using a titration to know the concentration of an unknown solution of NaCN then you will need the HCl volume reached in the equivalence point to calculate the amount of NaCN in the original solution and this is the question 8B Having said that I will assume that our
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