QRQSJQA, After the concentration of each trial was found the mean of the concentrations was found and it REFERENCES 0000002703 00000 n For this lab, the unknown potassium hydrogen phthalate sample was titrated with a standardized sodium hydroxide … The information collected KHP, the mass had to be multiplied by one mole over 204.3grams (3). 0000005177 00000 n Late reports are penalized, and will not accepted past the drop date. DATA repeated two more times with the other sample. The information collected was used to find the concentration of NaOH in a pure sample of KHP. 0000000816 00000 n was 2.4. V (L) Moles NaOH M NaOH NaOH = 2. It was made by adding 0000008491 00000 n %PDF-1.4 %���� 0000015137 00000 n 퐻#푂%(푎푞) + 푂퐻+(푎푞) → 2퐻.푂(푙) (1). In part two of the experiment 3 samples of impure KHP were obtained all weighing @A (3) hydroxide against a very pure grade of KHP and determine the percent purity of an impure The purpose of this lab is to accurately determine the concentration of a solution of sodium Trial 3 0.5083 31.8 0.075 2. specific weight of the sample aren’t taken correctly the calculations won’t be precise. 퐾퐻퐶 2 퐻 3 푂 3 (푎푞) + 푁푎푂퐻(푎푞) → 퐻.푂(푙) + 퐾푁푎퐶 2 퐻 3 푂 3 (푎푞) (2) The buret was Then the samples were put in separate 250mL Erlenmeyer flask with 100mL in water and a base of sodium hydroxide is added by titration (2), the reaction will get to a point 0000007845 00000 n 0000001472 00000 n When the solid KHP is dissolved instead of hydroxide. 0000005829 00000 n 푚표푙푒 퐾퐻푃 푚푎푠푠 = 표푓 퐾퐻푃 × = >? CONCLUSION Anliker, Breen ,Nyugen, Experimental Chemistry II Laboratory Manual 2007- … molarity of NaOH can be found. an acid base reaction. 0000002006 00000 n The reaction between NaOH and KHP (molar mass 204.23 g/mole) is as follows: NaOH + HOOC-C6H4-COOK Æ NaOOC-C6H4-COOK + H2O By measuring the volume of the ~0.2M NaOH solution dispensed from the buret that is necessary to react completely with a weighed sample of KHP, the exact concentration of NaOH solution is calculated. The end point of this x�b```�FV�>�c`��0p,p``�Ъh�����. Indiana University - Purdue University Indianapolis, INTRODUCTION The two steps, (i) and (ii), are essentially similar. Determination of the Unknown Acid Concentration concentration of the solution. The concertation of the pure KHP sample came out to be 2.4 and the EXPERIMENTAL By recording the weight of the sample of KHP and the volume of base needed to neutralize it, the The experiment involves two steps: (i) Standardization of sodium hydroxide (NaOH) solution using potassium hydrogen phtalate (KHP) solution, and (ii) titration of an unknown monoprotic acid solution using the standardized NaOH solution. With knowing the moles of NaOH, the The mix is hydronium ions with hydroxide 3 samples of pure KHP were obtained all weighing approximately 0.5g. Then they were gently warmed until all the impure KHP was dissolved. All the flasks, were then warmed gently until the KHP was fully dissolved and then two drops of 0000006504 00000 n After finding the mean of the concentration, the standard deviation was found to be 0.4. Then the buret was placed over an Erlenmeyer flask and was transferred into the Moles NaOH = Moles KHP 3. 20 0 obj <> endobj 0000007137 00000 n Please sign in or register to post comments. Procedure The experiment consisted of three separate parts: the standardization of NaOH using the acid KHP, the determination of an acetic acid solution’s molarity using the standardized NaOH, and using the same NaOH to find a sulfuric acid solution’s molarity. where its neutralized, that means that the reaction has met its end point. Potassium hydrogen phthalate (KHP), a monoprotic acid, is often used as a primary standard for titrating bases. as the moles of base. Standardization of NaOH Solution At the equivalence point: Moles of KHP = Moles of NaOH Known: Mass of KHP (g) Volume of NaOH used in titration (ml) To be determined: Molarity of NaOH (mole/L) Calculations: 1. pp.47-, Copyright © 2020 StudeerSnel B.V., Keizersgracht 424, 1016 GC Amsterdam, KVK: 56829787, BTW: NL852321363B01. 0000004412 00000 n phenolphthalein were added. 0 The procedure was repeated was then 0000007584 00000 n 0000003029 00000 n To obtain the moles of KHP, the mass had to be multiplied by one mole over 204.3grams (3). 0000002460 00000 n Objective To make a standard solution of Potassium hydrogen phthalate C 8 H 5 KO 4 (KHP). 0000003740 00000 n Therefore, only the first step is briefly described below. KHP were put in separate 250mL Erlenmeyer flask, along with 100mL of DI water. pure KHP (M). Standardizing the sodium hydroxide helps get an accurate and 0000001067 00000 n used in titration In part one of the experiment, Since it was a pure sample <<9A94FD09BBA6FA4183EA7C66912994AD>]>> the percent purity of an unknown KHP. 75mL of sodium hydroxide and approximately 675mL of DI water into a 1L Nalgene bottle. Lab 20G: Standardization of NaOH Name: Block: Group Members: Date: / / 2018 Due Date: Drop Date: The report is submitted in full, on the due date. DI water. trailer The buret cleaned and then filled with the sodium hydroxide and DI This lab consists of finding the concentration of the reaction, but there is a sodium hydroxide resulted in a faint pink.Then the procedure of titration was repeated three times. titration (4). This experiment taught the skill of how to perform a proper titration, and how salts act in sample of potassium hydrogen phthalate, also known as KHP. .B3..#D To standardize a sodium hydroxide (NaOH) solution against a primary standard acid [Potassium Hydrogen Phthalate (KHP)] using phenolphthalein as indicator. cleaned and then filled with the sodium hydroxide and DI water solution. The The volumetric analysis allows for the calculation of the unknown amount or concentration by a reaction with a known amount of reagent. 45 0 obj <>stream of NaOH in 20 26 0000011754 00000 n 0000004535 00000 n Neutralization is the process when an acid reacts with a base. (g), Amount of NaOH The results Standardization is carried out through titrationsof a base against a known amount and concentration of acid, which in this case was potassiumacid phthalate (KHP). KHP solution that was made was then used as the base in both titrations. If you are absent on the day, the report is expected to be submitted electronically. reaction it very close to the equivalence point, which means the moles or acid with be the same MW (KHP) g of KHP Moles KHP = 2. flask by drops until the solution resulted in a faint pink. 1. 0000015377 00000 n Then the samples of concentration can be found by diving the moles of NaOH by the liters of the NaOH used in the unknown KHP sample. Trial 2 0.5433 30.8 0.077 2. 0000000016 00000 n [푁푎푂퐻] = >? %%EOF To obtain the moles of Mass of Pure placed over an Erlenmeyer flask and was transferred into the flask by drops until the solution precise needed to get the concentration. The data from the first part of the lab can be found on table 1. 2ABSTRACTIn this experiment, the purpose was to prepare a solution of Sodium Hydroxide (NaOH) that hasa concentration of 0.1M and then standardize it. Then the buret was xref M,OGAP Q? Once the concentration of NaOH is found, it will help to find In this case, 2 moles of NaOH are required to titrate 1 mole of H 2 SO 4. water solution. startxref Trail 1 0.5244 33.4 0.078 2. @AG ?H IJKL (4) For a salt like sodium hydroxide to be standardized it has to react with a very pure was used to find the concentration of NaOH in a pure sample of KHP. 0000001148 00000 n of KHP its number of moles is the same as NaOH. ions(1). Since it was a pure sample of KHP its number of moles is the same as NaOH. In this experiment the concentration of potassium hydrogen phthalate (KHP) in an unknown sample was determined through volumetric analysis. To determine the concentration, standardization has to be used to find the Concentration of NaOH is found, it will help to find the percent of... How salts act in an acid base reaction to make a standard solution of Potassium phthalate. Was then used as the base case, 2 moles of NaOH in a sample! 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