For question 5 could you find the best value and explain how you arrive to the best value pleasethank you! 08上LO%23B. Standardization of the NaOH solution3.25Moles of KHp in 20.00 mL of KHp solution used for titration_5.Volumes of your NaOH solution used to titrate this 20.00 mL of acid. Best two trials for each student:Your ResultsPartner's Results16.3514.30Trial 113.3319.47Trial 2Best Value6.Explain how you arrived at your best value.0.227.Molarity of your NAOH solution:MacBook Air00000002F4DDF5F6DAF7F8%24&3.4.9-7.

A question based on quantitative analysis, which is to be accomplished.

Answered: For question 5 could you find the best…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.28QAP

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Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSeO4, 0.0118 g/100 mL. (b) Ba(BrO3)2H2O, 0.30 g/100 mL. (c) NH4MgAsO46H2O, 0.033 g/100 mL. (d) La2(MoO4)3, 0.00179 g/100 mL
Consider the following two acids: pKa1 = 2.98; pKa2 = 13.40 HO2CCH2CH2CH2CH2CO2H Adipic acid pKa1 = 4.41; pKa2 = 5.28 In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results.
Determine the Concentration of Ethanoic Acid in Vinegar Equipment / Apparatus:  250-mL conical flasks  Clamp  Burette  Graduated cylinder  Pipette Reagents / Materials:  Vinegar  Phenolphthalein indicator  0.2 M NaOH (standardized) Calculation: Molarity (M) of ethanoic acid  The average measured volume of the NaOH from titration: Average volume of NaOH used = (21.5ml + 21.5ml + 21.6ml) / 3 =21.5ml No of mole of NaOH = Concentration of NaOH (0.2M) × Average volume of NaOH used When an acid is completely neutralized: No of moles of CH3COOH = No of moles of NaOH Using the moles of CH3COOH, the molarity of ethanoic acid in the 5.0-mL sample of vinegar is calculated: Molarity (M) CH3COOH = moles CH3COOH / volume of vinegar (0.005 dm3). Calculation: Mass / Volume Percent (m/v) of ethanoic acid To calculate the percent (m/v) of CH3COOH in vinegar, we convert the moles of ethanoic acid to grams using the molar mass of ethanoic acid, 60.1 g/mole. Mass of CH3COOH =…
A sample of vinegar weighing 10.52 g is titrated with NaOH. The end point is overstepped, and the solution is titrated back with HCl. From the following data, calculate the acidity of the vinegar in terms of percentage of acetic acid, CH3COOH Standardization Data:1.050 mL HCl ≡ 1.000 mL NaOH1.000 mL NaOH ≡ 0.06050 g benzoic acid, C6H5COOH (122.12 g/mol) Analysis Data:Volume NaOH used = 19.03 mLVolume HCl used for back titration = 1.50 mL
What mass of Ba(OH)2 is present in a sample if it is titrated to its equivalence point with 44.20 mL of 0.1000 N H2SO4? Note: Present complete solutions for the following problem. Express your final answers up to two (2) decimal places.
Calculate the percentage CH3COOH in a sample of vinegar from the following data. Sample = 15.00 g, NaOH used = 43.00 ml ; 0.600 N H2SO4 used for back titration =0.250 ml ; 1.00 ml NaOH is equivalent to 0.0315 g H2C2O4. 2H2O.
Calculate the percentage CH3COOH in a sample of vinegar from the following data.Sample = 15.00 g, NaOH used = 43.00 ml ; 0.600 N H2SO4 used for back titration =0.250 ml ; 1.00ml NaOH is equivalent to 0.0315 g H2C2O4. 2H2O.
Na2CO3 served as the primary standard in a titration experiment. Find the molarity of the titrant given the following data in 3 decimal places. Show solutions Primary Standard Used: Na2CO3Formula Mass of 1º standard: 105.99 g/mol% purity of 1º standard: 95% Trial 1 2 3 1º Standard weight, g 0.1005 0.1001 0.0997 Net volume of HCl, mL 9.30 9.00 8.90 Molarity of HCl X1 X2 X3
What is the molarity of a commercial phosphoric acid solution, H3PO4 (MW= 98.0 g/mol) that is 85.0% (w/w) and has a specific gravity of 1.689? Also Make a graph of pH versus VHCl for the titration
If a 0.3 M solution of NaOH was used to titrate 100 mL of 0.3 M solution of CH3COOH (Ka =1.8 x 10 -5) and the following volumes of NaOH were recorded: 102, 97, 99, 98, 101, 106 mL. The pH Value is………………when added 99.0 mL of 0.3 M NaOH The pH of the solution at the equivalence point more than 7 Because................................... Calculate the 99% confidence limits of the mean? And use them to decide whether there is any evidence of systematic error? [ hints: For N=6 and the 99 % confidence interval, the value of t is 4.03].
Calculate the volume in mL of 0.311 M KOH necessary to titrate 23.38mL of 0.342 M diprotic sulfuric acid, H2SO4 to a phenolphthalein end-point. Report your answer to a precision of 2 decimal places.

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For question 5 could you find the best value and explain how you arrive to the best value please thank you!