Perform the necessary calculations to determine the concentration of sodium hydroxide solution given the data below. Round off your answer to 4 decimal places. No need to include the unit. Weight of primary standard, g 0.2415 Molar mass of primary standard, g/mol 204.22 For the titrant Initial buret reading, mL 0.12 Final buret reading, mL 23.79 Add your answer

Perform the necessary calculations to determine the concentration of sodium hydroxide solution given the data below. Round off your answer to 4 decimal places. No need to include the unit. Weight of primary standard, g 0.2415 Molar mass of primary standard, g/mol 204.22 For the titrant Initial buret reading, mL 0.12 Final buret reading, mL 23.79 Add your answer

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter79: Solubility

Section: Chapter Questions

Problem 1P

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Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
Please answer this NEATLY, COMPLETELY, and CORRECTLY for an UPVOTE. From the stock solution (0.020 M), pipet 4.00 mL and dilute to 100.00 mL. From the diluted solution, pipet 0.00, 1.00, 1.50, 2.00, 2.50, 5.00 and 7.50 mL aliquots into 100 mL volumetric flasks. Dilute to mark. Determine the concentration of each standard solution and tabulate.
In which situation(s) is it necessary to use a volumetric flask for maximum accuracy? to prepare a 0.150M solution of sodium chloride to measure ~25mL of water to prepare 0.1M HCI from 36-38% HCI a and c all of the above (Please type answer no write by hend)
A 1.458 g primary-standard grade Na2CO3 (MW = 105.99 g/mol) was used to standardize an HCl solution. Solve for the molarity of HCl if 24.81 mL of HCl was used to reach the endpoint.
-The density of aluminum is 2.70 g/cm'. Calculate the thickness of a rectangular sheetof aluminum foil with a width of 11.5 cm, a length of 14.0 cm, and a mass of 2.04 g. -Examine your results from your data table in Part 3. Do you have any values for thedensity of the salt solution that lie OUTSIDE the range (& 2s)? If so, list them here: Recalculate & by omitting values that lie OUTSIDE the range. This is the density valueyou should use to determine your experimental % NaCl. part 3 data table included
Normality is same as Molarity for sodium hydroxide and normal = molar (for NaOH) Normality of sodium hydroxide = 0.10395N (normal) or Molarity of NaOH = 0.10395M (molar) Volume of NaOH consumed during the titration = 21.87 mL Mol wt of Naproxen = 230.26 g/mol Weight of Naproxen ds (i.e., sample) = 0.534g Calculate the % Purity (dried-basis) of Naproxen ds, given that the LOD results for Naproxen = 1.0% a 97.0 b 98.0 c 98.5 d 99.0 e 99.5 f none of the other answers.
. A student was given a solution of unknown molarity of Potassium Hydroxide (KOH). On the lab bench the following chemicals are kept Distilled water, Potassium Hydrogen Phthalate (KHP), HNO3, phenolphthalein and methyl or ange All required glassware is available in the lab. (a). What should be chosen as the standard solution? Justify and explain your answer by giving two properties of substances used to make standard solution. (b). What should be chosen as the indicator for the titration of nitric acid and ammonium hydroxide? Justify your answer
Please answer subparts d-e. Show solutions. Thanks
Write in your own words the steps and precautions involved in using a pipette to measure out the standard solution. Explain the justifications for each step.
PS. Further values required for the solvings are give in the various situations below. (ANSWER) Situation: A community in a mountainous area of Bohol uses water collected from a nearby natural spring. A sample was submitted to a laboratory for the analysis of its total hardness. Required: SHOW YOUR COMPLETE CALCULATIONS. BASED ON THE IMAGE PROVIDED BELOW FOR THIS QUESTION: Calculate the amount of titrant used in each trial to reach endpoint. Report total hardness of the sample as mean ±sd. a. 250.0 mL of 500.0 ppm of CaCO3 solution from a primary standard (assume solvent is distilled water only). Answer : Mass of CaCO3 = 0.125 g b, The EDTA solution was standardized by titrating it with a 25.0 mL aliquot of the CaCO3 solution. How much of the titrant was consumed. Answer: Volume of EDTA consumed = 12.405 g c. Calculate the average titer (mg CaCO3/mL EDTA). Mass of CaCO3 in 25 mL CaCO3 solution: 0.0125 g Answer: 1.008 mg CaCO3/ mL EDTA
A titrant solution of KMnO was standardized with 0.2000 grams of Na2C2O4 and consumed 27.75 mL to reach end point. Calculate the standardized NORMAL concentration of the titrant.
In standardizing a solution of NaOH against 1.431g of KHC8H4O4, the analyst uses 35.50 mL of the alkali and has to run back with 5.12 mL of acid (1mL = 0.0031g Na20) What is the normality of NaOH? Additional instructions: Make it handwritten Include up to 4 decimal places Please include explanations of the process Thank you so much!