4.000 g is after all 0.1000 mole of NaOH, so dissolving it in one litre of water should produce a one litre solution. Standardizing NaOH(aq) Potassium hydrogen phthalate (KHP, KC 8 H 5 O 4) is a solid, monoprotic acid. or. The reaction between solutions of HCl and NaOH is illustrated by Equation 1. 3. 37 - 24,4 = 12,4 into the acid HCL From the above experiment it was evident that sodium hydroxide can be effectively standardized by using oxalic acid. In this experiment, standardization of a NaOH solution will be carried out either using KHP as the primary standard or by using a standard HCl solution of known concentration. THIS IS THE VALUE THAT YOU WILL USE IN EXPERIMENT 12B. Transfer 10 mL of the NaOH solution into a 125 mL conical flask with the aid of a pipette, add 1-2 drops of phenolphthalein indicator and titrate with the standard oxalic acid. been standardized. This sample calculation uses the … 2. Calculate the average molar concentration of the sodium hydroxide solution. The volumetric analysis allows for the calculation of the unknown amount or concentration by a reaction with a known amount of reagent. By: Juno Kim Introduction In this experiment the concentration of potassium hydrogen phthalate (KHP) in an unknown sample was determined through volumetric analysis. 49 - 12 cm3 = 37 cm3 of NaOH. You might think that you could just weigh 4.000g of solid NaOH and dissolve it in enough water to make 1.000 L of solution. Calculation N 1 V 1 = N 2 V 2 N 2 =Normality of oxalic acid N 1 =Normality of NaOH V 2 =Volume of Oxalic acid V 1 =Volume of NaOH N 1 =N 2 V 2 /V 1. Equipment/Materials: Try it risk-free for 30 days Try it risk-free Ask a question. E. CALCULATION 1. 3.3.2 Standardization of NaOH solution using diprotic acid (oxalic acid) or (Succinic acid) Place the standard oxalic acid solution 0.025 M in the burette. Average NaOH molarity calculated to be 0.09515 M. Titrations performed by Yu-Ting Tseng and taken for comparison The standard deviation for both data sets was calculated by the method shown below using Equation 1. (2) Again fill the burette with the standardized NaOH solution to the zero mark. Weight out 0.4g of KHP STOPPER AND SAVE YOUR NaOH SOLUTION FOR USE IN EXPERIMENT 12B !!!!! CONCLUSION. Become a member and unlock all Study Answers. Calculations : 24,4 ml - 12 ml = 12,4 ml ⇒ Neutral. NaOH of unknow concentration. We ended with 24,4 ml of NaOH. Therefore, the equivalent weight of crystalline oxalic acid = 63. Suppose that you needed a 0.1000 M solution of NaOH to do a titration. Before you can use the NaOH(aq) to standardize your HCl(aq), you will have to standardize the NaOH(aq) using the primary solid acid standard, potassium hydrogen phthalate. Top it up to the mark. Calculate the molar concentration of the sodium hydroxide solution using your data for each run. 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