A. Diluting KOH Stock Solution: I am going to make 200 mL of 0.1 Molar KOH that I will use for the titrations in this experiment. Your instructor will tell you the concentration and volume of the diluted solution that you will need to prepare. Step 1 (First day calculation, 10 pts): mL of stock KOH necessary to make the above KOH concentration. Show work here: Let's assume the stock solution that is given is 2.5 M B. Standardization of the KOH Solution Step 3 (First day calculation, 10 pts): Mass of pure H2C2O4·2H2O standard that would use about 15 mL of KOH = There is a periodic table attached. Show work here:

A. Diluting KOH Stock Solution: I am going to make _200_ mL of _0.1_ Molar KOH that I will use for the titrations in this experiment. Your instructor will tell you the concentration and volume of the diluted solution that you will need to prepare. Step 1 (First day calculation, 10 pts): ____ mL of stock KOH necessary to make the above KOH concentration. Show work here: Let's assume the stock solution that is given is 2.5 M B. Standardization of the KOH Solution Step 3 (First day calculation, 10 pts): Mass of pure $H_2C_2O_4\cdot2H_2O$ standard that would use about 15 mL of KOH = _____ There is a periodic table attached. Show work here:

Experiment: Standardization of sodium hydroxide stock solution with potassium hydrogen phthalate You prepare a solution by dissolving 4.8854 g of KHP (molar mass: 204.23 g/mol) in distilled water and making it up to 250 mL in a volumetric flask. You pipette 25 mL of the solution, add phenolphthalein indicator, and then perform 3 separate titrations using NaOH. The average volume of NaOH added is 23.97 mL. The chemical equation for the reaction between aqueous NaOH solution and potassium hydrogen phthalate is: KHP (aq) + NaOH (aq) â†’ NaKP + H2O. Calculate the following (please show detailed calculations): a) The number of moles of KHP b) The molarity of KHP solution c) The molarity of the NaOH solution

David C.

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