You are titrating a 1.033 g sample of white vinegar solution (5.0% acetic acid) with a 1.00 M NaOH titrant. At the endpoint of titration, 0.89 mL of NaOH was used. What is the mass % of acetic acid based on your experimental results? CH3COOH = 60.052 g/mol
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You are titrating a 1.033 g sample of white vinegar solution (5.0% acetic acid) with a 1.00 M NaOH titrant. At the endpoint of titration, 0.89 mL of NaOH was used. What is the mass % of acetic acid based on your experimental results? CH3COOH = 60.052 g/mol
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- Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balance chemical equation is given below. If the student used 21.21 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balanced chemical equation is given below. If the student used 25.71 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)1. An acid solution is prepared by dissolving 19.264 grams of pure KHC2O4.H2C2O4.2H2O in water and diluting to exactly 900 ml. Fifty milliliters (50.00 mL) of this solution are neutralized by 35.00 ml. of KOH solution. What is the normality of each solution? 2. What mass of Ca(OH)2 is present in a sample if it is titrated to its equivalence point with 44.02 mL of 0.0885 M HNO3? The balanced chemical equation is as follows: 2HNO3 + Ca(OH)2 → Ca(NO3)2 + 2H2O ; Balanced.
- 10 ml of commercial vinegar was diluted to 100 ml with distilled water, when we titrate 10 ml of this solution with 0.15 M standardized sodium hydroxide solution, we found that we need 12 ml of basic solution to reach the end point, if the atomic weight of c = 12 0 = 16 H=1 calculate : 1- Number of grams of acetic acid in commercial vinegar. 2- The percentage of acetic acid in commercial vinegar. 3- Write the chemical equation between acetic acid and sodium hydroxide.A pharmacist is identifying the saponification value of corn oil in the lab. She weighs 1.8 g of corn oil and saponified with 25 mL of 0.4 N KOH which require 9 mL of 0.5N HCl to titrate the excess KOH. She performs blank determination, 20 mL of 0.5 N HCl was required to titrate the corn oil. What is the saponification value of the corn oil? Does the sample comply with the USP requirement? Use this formula to work your result Saponification Value = (Vblank - Vsample)N of HCl56.11/Sample weight (g)This question is about acid base titration: Osama a student, performed an acid base titration involving a standard solution of Sodium hydroxide (NaOH) (RMM = 40) against unknown HCl solution and obtained the following results. Mass of Sodium hydroxide (NaOH) dissolved in 250 ml volumetric flask = 3.6 g 2.Volume of Sodium hydroxide used in the titration = 23 ml 3.The mean volume of HCl titrated with 25 ml Sodium…
- A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 50.mg of oxalic acid H2C2O4 , a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 26.2mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Be sure your answer has the correct number of significant digits.In Part A of this experiment, you will be standardizing a solution of sodium hydroxide (NaOH) against a sample of oxalic acid dihydrate (H2C2O4⋅2H2O, 126 g/mol). Calculate the number of grams of H2C2O4⋅2H2O required to completely neutralize 25.0 mL of 0.120M NaOH.A titration of 25.00 mL of an unknown HCl solution with 0.1550 M NaOH starts at a buret reading of NaOH of 0.33 mL. The phenolphthalein indicator turns light pink in the acid solution over 30 seconds at a buret reading of 24.19 mL. Write the balanced equation for the neutralization reaction. What is the molarity of the HCl solution?
- A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 51 mg of oxalic acid (H2C2O4), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250 mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 19.2 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution.A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 13.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 11.9mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.1. A solution of HCl is prepared by an unknown dilution of concentrated HCl. It is standardized by titrating 0.2897 grams of dried primary standard Na2CO3 with 54.76 mL acid, 0.2475 g Na2CO3 with 53.46 mL acid, and 0.2279 g Na2CO3 with 55.12 mL acid. Calculate the mean molar concentration of the HCl solution. 2. a) What is the uncertainty in the molarity in the previous problem determined by the propagation of typical uncertainties: emass = ±0.0002 g and evolume = ±0.02 mL? (You may use any one trial from Problem 2 to illustrate the propagation). b) What is the uncertainty in molarity in the previous problem if we take the uncertainty to be the standard deviation? c) For what reason(s) are the answers to B and A different? What is the cause of the difference?
