Hypothesis: A prediction of what you think the results of the project will be. Calculate the molarity of the NaOH solution. The resultant Acidic solution was transparent, with a small amount of undissolved granules of KHP. Hypothesis: A prediction of what you think the results of the project will be. This way, we avoid excess NaOH from being added. both moles and grams. Hint: You must write a balanced equation for the reaction. Cite this article as: William Anderson (Schoolworkhelper Editorial Team), "Titration Lab: NaOH with Standardized solution of KHP," in. Where [c]KHP is the concentration of KHP Acid. The percent error that has resulted is: 9.03% is by far a significant error that has resulted from a small error in the volume. Calculate the molarity of the NaOH solution. The molar mass of NaOH is 39.997 g/mol. How many mL of water were used to prepare the NaOH solution? Overall, the data obtained, although not completely inaccurate, have not been as accurate as it could have been. Standardization of a Sodium Hydroxide (NaOH) Solution with Unknown Concentration. Number of moles of KHP in 2.00 grams = (m/M) = (2/204.22) mol = 0.00979 mol, Number of moles of KHP in 0.01 dm3 of solution in conical flask = [c] x V. From mole ratio, number of moles of NaOH = 0.00979 mol. This preview shows page 1 - 2 out of 3 pages. The volumes of NaOH used up shows significant fluctuations. Let us do your homework! What I know is due to various errors which tend to happen when conducting an experiment such as contamination of the sample used (impurities) also external factor like temperature and humidity which results the sample to react with the atmosphere (air). The molar mass of NaOH is 39.997 g/mol..800g X 1mole/39.997= .200mole/ .200L= .1M NaOH … For example, in trial 1, I used 11.0 cm3 of NaOH, which is 1.50 cm3 off 9.50 cm3, and in my rough trial, the volume used was 9.9 cm3 and in trial 2, the amount used up was 10.4 cm3. Short Answer Standardization of an NaOH Solution Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare the NaOH Solution Lab Results 1. How many mL of water were used to prepare the NaOH solution? However, this, being only 0.01 grams of the expected value, could have only constituted a very small portion of the error. Also, the % uncertainty of the volume of NaOH was ±1.05%, taking the value of 9.50 cm3. How many mL of water were used to prepare the NaOH solution? However, there has been a deviation of 0.9 cm3, which is significant, but not high. These errors were avoidable. It only takes seconds! (b) Place the Erlenmeyer flask on the lower half of the burette — this will connect them. Fill the burette with 50 mL of the prepared sodium hydroxide solution. Help Please If you assume that the NaOH which you will prepare for the standardization is approximately .12M, calculate the number of moles and the number of grams of H2C2O2 x 2H20 required to neutralize 25 ml of this NaOH solution? Standardization of an NaOH Solution-Help.docx, Wytheville Community College • CHEMISTRY 112, Pennsylvania State University, Berks • CHEM 113, Liberty University Online Academy • CHEM 101, Georgia Military College Valdosta Campus • CHE 122, Copyright © 2020. The molar mass of benzoic acid is 122.12 g/mol. To standardize a sodium hydroxide (NaOH) solution against a primary standard acid [Potassium Hydrogen Phthalate (KHP)] using phenolphthalein as indicator. Your online site for school work help and homework help. Calculate the molarity of the NaOH solution. For a substance to be a primary standard, the following criteria should be met: • It must be available in very pure form. Taking the value of 9.50 cm3 and mass of 2 grams, the concentration of NaOH should have been 0.103 mol, but the value I obtained due to the excessive deviation gave me 0.0937 mol. Calculate the molarity of the NaOH solution. 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. To standardize a sodium hydroxide (NaOH) solution against a primary standard acid [Potassium Hydrogen Phthalate (KHP)] using phenolphthalein as indicator. 2.00 grams was the amount expected to be taken, but the experimental amount was 1.99 grams. Calculate the amount of benzoic acid to be neutralized by 20.00 mL NaOH solution, in. EXPERIMENT 7: ACID-BASE TITRATION: STANDARDIZATION 91 Standardizing the NaOH Solution In the lab notebook, set up a data table similar to the one given at the end of this exercise. The theoretical value of the Sodium Hydroxide that was expected to be used was 9.50 cm3. These fluctuations caused the 0.95% error. (if available) magnetic stir plate. Standardization of an NaOH Solution Experiment 1: Standardize an NaOH Solution Using Benzoic Acid as Primary Standard Part 1: Prepare the NaOH Solution Lab Results 1. The molar mass of NaOH is 39.997 g/mol. Calculate the molar concentration of the NaOH solution. The molar mass of NaOH is 39.997 g/mol. 18th May 2020 Chemistry Reference this V (L) Moles NaOH M NaOH NaOH = 2. ATTENTION: Please help us feed and educate children by uploading your old homework! A standard solution 4. The expected % uncertainty that was expected was 0.500%, and the uncertainty I obtained was 0.503%. The resulting percentage error out of this deviation is: There is almost a 1% deviation. The difference between these sets of data indicates that the systematic error of allowing the KHP solution to become too pale resulted in strange fluctuations. Moles NaOH = Moles KHP 3. MW (KHP) g of KHP Moles KHP = 2. To do this, you will titrate an accurately measured mass of dry benzoic acid with a prepared NaOH solution of approximate concentration. The crystals required intense stirring before it could dissolved in water. Therefore, due to flaws in raw data values taken from systematic errors, there has been a deviation in uncertainty too, indicating the impact of methodical flaws. The uncertainty of 2.57% indicates that my values were accurate up to within ±2.57%. However, the amount I added on an average was 10.4 cm3, which suggests why the solution became unusually dark pink as supposed to light pink. Transfer 10 mL of the NaOH solution into a 125 mL conical flask with the aid of a pipette, add 1-2 drops of Chem- Pre Lab Standardization of a Solution of Sodium Hydroxide? Free proofreading and copy-editing included. 200mL Data Analysis 2. A primary standard substance b. Standardization of NaOH. As the transparent NaOH solution came into contact with transparent phenolphthalein in the KHP solution, it turned pink which on shaking became transparent. 1 Digital Balance (upto 2 decimal places accuracy), % Uncertainty of (aq) KHP in Volumetric Flask = (0.1/100) x 100, % Uncertainty of (aq) KHP in Pipette = (0.1/10) x 100. Standardization of NaOH Solution? 200 mL Data Analysis 2. II. The deviation in the volume, however, is not the only indicator of noticeable systematic errors. One experimental flaw which resulted in readings inconsistent with the literature value was due to human error. Allowing the KHP solution to become too pink. During the standardization of the NaOH solution used in the lab, suppose that a student accidentally “overshot” the standardization titrations (added too much titrant). Article last reviewed: 2019 | St. Rosemary Institution © 2010-2020 | Creative Commons 4.0.

standardization of an naoh solution lab answers

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standardization of an naoh solution lab answers 2020