Question

You want to determine the concentration of acid in a particular solution. To this end, you decide to titrate the acid with a standardized sodium hydroxide solution. You quickly throw together an approximately 0.1 M NaOH solution, and then you realize you need to know the exact concentration of this solution before you can use it for anything meaningful. 1. Using an acid-base titration, 30.65 mL of your NaOH solution were needed to neutralize 0.6923 g of KHP (potassium hydrogen phthalate, KHC8H4O4). What is the actual molarity of the NaOH solution? (HINT: moles acid = moles base) 2. Now that you have standardized your NaOH solution, determine the mass of acetic acid (CH3COOH) dissolved in a 49.77 mL of water if it takes 62.30 mL of your NaOH solution to neutralize it.

          You want to determine the concentration of acid in a particular
solution. To this end, you decide to titrate the acid with a
standardized sodium hydroxide solution. You quickly throw together
an approximately 0.1 M NaOH solution, and then you realize you need
to know the exact concentration of this solution before you can use
it for anything meaningful.
1. Using an acid-base titration, 30.65 mL of your NaOH solution
were needed to neutralize 0.6923 g of KHP (potassium hydrogen
phthalate, KHC8H4O4). What is the actual molarity of the NaOH
solution? (HINT: moles acid = moles base)
2. Now that you have standardized your NaOH solution, determine
the mass of acetic acid (CH3COOH) dissolved in a 49.77 mL of water
if it takes 62.30 mL of your NaOH solution to neutralize it.

Added by Lauren S.

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