Question 4 Titration video step 3 question: NaOH flush out H2O True or False, before you do the titration, you need to get the air bubble out of the glass tubing below the glass bead. A True B False Question 5 Questions Filter (10)

Question 4 Titration video step 3 question: NaOH flush out H2O True or False, before you do the titration, you need to get the air bubble out of the glass tubing below the glass bead. A True B False Question 5 Questions Filter (10)

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter5: Errors In Chemical Analyses

Section: Chapter Questions

Problem 5.10QAP

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Hello! Could you please answer this with one long dimentional analysis like I am supposed to do it? Thank you!
2A student used a pipette to add 25 cm³ of sodium hydroxide of unknown concentration to a conical flask. The student carried out a titration to find out the volume of 0.1 mol/dm3 sulfuric acid needed to neutralise the sodium hydroxide. The following is the table of results obtained. Titration Volume of sulfuric acid used/cm³ 1 27.85 27.30 27.25 27.10 27.30 a. Write down a balanced equation for the reaction between sodium hydroxide and sulfuric acid. b. Describe the titration experimental procedure (details of washings are expected) c. Determine the average titre value and explain your choice of titre values in calculating the average. d. Determine the concentration of sodium hydroxide. e. If instead of sulfuric acid, hydrochloric acid of the same concentration was used what would you expect the average titre value to be and why?
Review the list of common titration errors. Determine whether each error would cause the calculation for moles of analyte to be too high, too low, or have no effect. ANSWER BANK: Too low, No effect OR Too high adding titrant past the color change of the analyte solutionrecording the molarity of titrant as 0.1 M rather than its actual value of 0.01 Mspilling some analyte out of the flask during the titrationstarting the titration with air bubbles in the buretfilling the buret above the 0.0 mL volume mark
Calculate final concentration
Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 2.29 1.41 1.95 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 50.37 49.39 49.84 Expected color at end point Volume of NaOH used (mL) 48.08 47.98 47.89 Compute for the ff: a. Average moles of acetic acid (mol)? b. Average molarity of acetic acid (M)? c. Average molarity of acetic acid (M)?
What is the molarity of the three solutions ?
Table 2. Titration data Trial 1 Trial 2 Trial 3 Initial burette reading (mL) 1.19 2.26 2.39 Molarity of NaOH (M) 0.100 0.100 0.100 Volume of vinegar sample (mL) 5.00 5.00 5.00 Final burette reading (mL) 48.55 49.43 49.99 Expected color at end point Volume of NaOH used (mL) Average Volume of NaOH used in liters Average moles of NaOH used (mol) Average moles of acetic acid (mol) Average molarity of acetic acid (M) Average mass of acetic acid (g) Average mass of vinegar (g) (assume the density of vinegar is 1.00 g/mL) Average mass % of acetic acid in vinegar Known mass % of acetic acid in vinegar is 5.45% Percent Error
Students measured the concentration of HCl in a solution by titrating with different indicators to find the end point. (Use the table to find critical F values.) Mean HCl concentration (M) (+ standard deviation) Indicator Number of measurements 1. Bromothymol blue 0.09565 + 0.00170 28 2. Methyl red 0.08681 ± 0.00098 18 3. Bromocresol green 0.08641 + 0.00106 29 Is the difference between Indicators 1 and 2 significant at the 95% confidence level? O Yes O No Fenlculated clegrees of freedom Ecalculated Is the difference between indicators 2 and 3 significant at the 95% confidence level? O Yes O No Fealculated Spooled tcalculated
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Volume vinegar used (mL)= 5.00 mL % from labe= l5 % Molarity of NaOH = 0.0976 M Titration volume measurements Trial 1 Trial 2 Trial 3 Inital volume NaOH (mL) 0.69 0.86 0.16 Final volume NaOH (mL) 43.47 43.36 43.03 Volume NaOH used (mL) Average volume NaOH used (mL) Average volume NaOH used (L) Moles NaOH used (from avg volume) Moles CH3COOH Molarity CH3COOH (mol/L) Mass CH3COOH (g) % (m/v) CH3COOH in vinegar
In chemistry class, a student conducted an investigation about factors affecting the solubility of copper (II) sulfate (CuSO4) in water. The data was recorded in the table below. Factors Trial 1 Trial 2 Trial 3 Stirring Yes No Yes Temperature 25°C 25°C 60°C Finely Crushed Powder Surface Area Large crystals Large crystals Q1)Which trial should dissolve the fastest? Q2) How are the collisions between the CuSO4 and water affected? Format BIU