Explain water and add a couple of drops of phenolphthalein

Reference no: EM13160610

Suppose in the lab you measure 0.3951 g of NaOH and dissolve it into 100.0 mL of water. You then measure 0.1985 g of KHP and place it in a clean, dry 100-mL beaker, and then dissolve the KHP in about 25 mL of water and add a couple of drops of phenolphthalein indicator. You titrate this with your NaOH(aq) solution and find that the titration requires 9.95 mL of NaOH(aq). NaOH= .1M How many moles of KHP are in your sample? How many moles of NaOH are required for the titration? What is the concentration of your NaOH(aq) solution? You then take 10.00 mL of wine, add a couple of drops of phenolphthalein, and titrate it with your NaOH(aq) solution. The titration requires 7.55 mL of NaOH(aq). How many moles of NaOH are required for the titration? Recall from the lab book that we will assume all of the acid is the diprotic acid tartaric acid (H2C4H4O6). How many moles of tartaric acid are in the 10.00 mL sample of wine? mol acid Determine the concentration of tartaric acid in the wine in terms of molarity. Determine the concentration of tartaric acid in the wine in terms of g/L.

Reference no: EM13160610

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Explain water and add a couple of drops of phenolphthalein : Suppose in the lab you measure 0.3951 g of NaOH and dissolve it into 100.0 mL of water. You then measure 0.1985 g of KHP and place it in a clean, dry 100-mL beaker, and then dissolve the KHP in about 25 mL of water and add a couple of drops of phe..

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