standardization of naoh with khp lab report

as the moles of base. Since it was a pure sample 0000007584 00000 n 0000002703 00000 n 0000003029 00000 n With knowing the moles of NaOH, the concentration can be found by diving the … Since it was a pure sample of KHP its number of moles is the same as NaOH. The experiment required a solution to be made to use as the base. With knowing the moles of NaOH, the %PDF-1.4 %���� was 2.4. Trail 1 0.5244 33.4 0.078 2. 0000001148 00000 n REFERENCES Potassium hydrogen phthalate (KHP), a monoprotic acid, is often used as a primary standard for titrating bases. %%EOF 75mL of sodium hydroxide and approximately 675mL of DI water into a 1L Nalgene bottle. 0000002006 00000 n Table 1: Standardization of Sodium Hydroxide Solution x�b```�FV�>�c`��0p,p``�Ъh�����. @AG ?H IJKL (4) The reaction 퐾퐻퐶 2 퐻 3 푂 3 (푎푞) + 푁푎푂퐻(푎푞) → 퐻.푂(푙) + 퐾푁푎퐶 2 퐻 3 푂 3 (푎푞) (2) water solution. used in titration concentration can be found by diving the moles of NaOH by the liters of the NaOH used in the KHP, the mass had to be multiplied by one mole over 204.3grams (3). 0000001067 00000 n The information collected 0000007137 00000 n 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. Neutralization is the process when an acid reacts with a base. repeated two more times with the other sample. For this lab, the unknown potassium hydrogen phthalate sample was titrated with a standardized sodium hydroxide … This experiment taught the skill of how to perform a proper titration, and how salts act in approximately 0.7g. KHP were put in separate 250mL Erlenmeyer flask, along with 100mL of DI water. 0000002780 00000 n Standardization is carried out through titrationsof a base against a known amount and concentration of acid, which in this case was potassiumacid phthalate (KHP). ions(1). To obtain the moles of KHP, the mass had to be multiplied by one mole over 204.3grams (3). Late reports are penalized, and will not accepted past the drop date. 퐻#푂%(푎푞) + 푂퐻+(푎푞) → 2퐻.푂(푙) (1). The procedure was repeated was then reaction it very close to the equivalence point, which means the moles or acid with be the same titration (4). Then the samples were put in separate 250mL Erlenmeyer flask with 100mL DATA MW (KHP) g of KHP Moles KHP = 2. After finding the mean of the concentration, the standard deviation was found to be 0.4. V (L) Moles NaOH M NaOH NaOH = 2. of KHP its number of moles is the same as NaOH. 0000015137 00000 n It was made by adding Then the buret was placed over an Erlenmeyer flask and was transferred into the In this experiment the concentration of potassium hydrogen phthalate (KHP) in an unknown sample was determined through volumetric analysis. 0000002425 00000 n 0000001472 00000 n The mix is hydronium ions with hydroxide in water and a base of sodium hydroxide is added by titration (2), the reaction will get to a point an acid base reaction. By recording the weight of the sample of KHP and the volume of base needed to neutralize it, the DI water. precise needed to get the concentration. molarity of NaOH can be found. solution that was made was then used as the base in both titrations. 0000000016 00000 n CONCLUSION 20 0 obj <> endobj hydroxide against a very pure grade of KHP and determine the percent purity of an impure The data from the first part of the lab can be found on table 1. QRQSJQA, After the concentration of each trial was found the mean of the concentrations was found and it flask by drops until the solution resulted in a faint pink. The information collected was used to find the concentration of NaOH in a pure sample of KHP. 0000000816 00000 n Anliker, Breen ,Nyugen, Experimental Chemistry II Laboratory Manual 2007- 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 percent purity of an unknown KHP. In part two of the experiment 3 samples of impure KHP were obtained all weighing To determine the concentration, standardization has to be used to find the In part one of the experiment, where its neutralized, that means that the reaction has met its end point. 0000007845 00000 n Trial 2 0.5433 30.8 0.077 2. The two steps, (i) and (ii), are essentially similar. Therefore, only the first step is briefly described below. To standardize a sodium hydroxide (NaOH) solution against a primary standard acid [Potassium Hydrogen Phthalate (KHP)] using phenolphthalein as indicator. pure KHP (M). 0000003740 00000 n 0000005177 00000 n instead of hydroxide. 3 samples of pure KHP were obtained all weighing approximately 0.5g. The buret cleaned and then filled with the sodium hydroxide and DI concentration of the solution. All the flasks, were then warmed gently until the KHP was fully dissolved and then two drops of (g), Amount of NaOH The volumetric analysis allows for the calculation of the unknown amount or concentration by a reaction with a known amount of reagent. 0000015377 00000 n The purpose of this lab is to accurately determine the concentration of a solution of sodium Indiana University - Purdue University Indianapolis, INTRODUCTION 0000005829 00000 n 0000002460 00000 n 푚표푙푒 퐾퐻푃 푚푎푠푠 = 표푓 퐾퐻푃 × = >? Then the samples of Please sign in or register to post comments. Standardizing the sodium hydroxide helps get an accurate and Mass of Pure EXPERIMENTAL @A (3) <<9A94FD09BBA6FA4183EA7C66912994AD>]>> Objective To make a standard solution of Potassium hydrogen phthalate C 8 H 5 KO 4 (KHP). .B3..#D (mL), Concentration pp.47-, Copyright © 2020 StudeerSnel B.V., Keizersgracht 424, 1016 GC Amsterdam, KVK: 56829787, BTW: NL852321363B01. 0000001328 00000 n 0000004535 00000 n Once the concentration of NaOH is found, it will help to find 0 The buret was To standardize a base solution such as NaOH, an acid whose amount can be determined to a high degree of accuracy (called a primary standard) is needed. xref 20 26 0000008491 00000 n placed over an Erlenmeyer flask and was transferred into the flask by drops until the solution 0000006504 00000 n for the first part of the lab could be off because the buret wasn’t cleaned correctly. If you are absent on the day, the report is expected to be submitted electronically. In this case, 2 moles of NaOH are required to titrate 1 mole of H 2 SO 4. 2ABSTRACTIn this experiment, the purpose was to prepare a solution of Sodium Hydroxide (NaOH) that hasa concentration of 0.1M and then standardize it. The results 0000011754 00000 n Trial 3 0.5083 31.8 0.075 2. specific weight of the sample aren’t taken correctly the calculations won’t be precise. phenolphthalein were added. 0000009061 00000 n 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. 0000004412 00000 n 45 0 obj <>stream cleaned and then filled with the sodium hydroxide and DI water solution. unknown KHP sample. 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. The happens instantaneously when they are mixed. When the solid KHP is dissolved For a salt like sodium hydroxide to be standardized it has to react with a very pure trailer The concertation of the pure KHP sample came out to be 2.4 and the startxref To obtain the moles of resulted in a faint pink.Then the procedure of titration was repeated three times. DATA The data from the first part of the lab can be found on table 1. M,OGAP Q? [푁푎푂퐻] = >? This lab consists of finding the concentration of the reaction, but there is a sodium hydroxide sample of potassium hydrogen phthalate, also known as KHP. KHP 1. 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. Then they were gently warmed until all the impure KHP was dissolved. percent purity of the impure KHP sample came out the be 32.96% pure. Determination of the Unknown Acid Concentration The end point of this of NaOH in was used to find the concentration of NaOH in a pure sample of KHP. … Moles NaOH = Moles KHP 3. Then the buret was

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