Using the data, calculate the molarity of sodium hydroxide solution for each run. M#1M #2M #3M #4 14-8Experiment 14Name OlonseaAcid-Base TitrationsDrawer NumberDataPart I. Standardization of the Sodium Hydroxide SolutionMass of weighing bottle + sample12.5252gMass of weighing bottle - sample9432gMass of H2C20 2 H202.5320g250.00 mLVolume of H2C204 solution2341Run Number25.00 mL25.00 mL25.00 mL25.00 mLVolume of oxalic acid used42.20mL212-25mL 42-50m2NaOH buret: final reading212.10mL0.20mLD.15ML0.40mL0.55MLNaOH buret: initial reading211.90L242.05wL41.85mLVolume of NaOH usedUnknown #n=Part II. Determination of the Molar Mass of an Acid234Eun Number1Mass of test1.417578tube + sampleMass of testtube - sample1,5160g1.S13ogMass of sample0,0998g0.099390.1003g0.1001gNaOH buret:20.10ML20.50ML20.20mL20.26MLFinal readingNaOH buret:Initial reading0.10mLO. 60ml-0.10ML0.25mhVolume of20.00mL19.90ML20.10mL20.00mLNaOH vsed

Mass of oxalic acid sample is calculated as the difference in the weight between mass of weighing…

Data Drawer Number Part I. Standardization of the Sodium Hydroxide Solution Mass of weighing bottle + sample 12-5252g Mass of weighing bottle sample 99932g Mass of H2C20. 2 H20 2.5320g Volume of H2C2O4 solution 250.00 mL Run Number 1 3 Volume of oxalic acid used 25.00 mL 25.00 mL 25.00 mL 25.00 mL NaOH buret: final reading 42.10mL 42.20mL 212-25L 42.502 NAOH buret: initial reading 0.20ML D.15ML 0.40mL 0.55ML Volume of NaOH used 211.902 212.05wL 41.85mL

Data Drawer Number Part I. Standardization of the Sodium Hydroxide Solution Mass of weighing bottle + sample 12-5252g Mass of weighing bottle sample 99932g Mass of H2C20. 2 H20 2.5320g Volume of H2C2O4 solution 250.00 mL Run Number 1 3 Volume of oxalic acid used 25.00 mL 25.00 mL 25.00 mL 25.00 mL NaOH buret: final reading 42.10mL 42.20mL 212-25L 42.502 NAOH buret: initial reading 0.20ML D.15ML 0.40mL 0.55ML Volume of NaOH used 211.902 212.05wL 41.85mL

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter10: Potentiometry And Redox Titrations

Section: Chapter Questions

Problem 7P

See similar textbooks

Similar questions

Figure 15-3 outlines the classic scheme for separating a mixture of insoluble chloride salts from one another. Explain the chemistry involved in the various steps of the figure.
Titration of 50.00 mL of 0.04715 M Na2C2O4 required 39.25 mL of a potassium permanganate solution. 2MnO4- + 5C2O4-2 +16H+ -> 2Mn2+ + 10CO2(g) + 8H2O Calculate the molar concentration of the KMnO4 solution. Pls show step by step. What type of molecules will interfere in this analysis ?
What do you call the stage of the titration in which the number of moles of the titrant is stoichiometrically less than the number of moles of the analyte? pre-equivalence equivalence end stage post-equivalenc
15. A 300.00 mL solution of 0.00165 M A2B5 is added to a 230.00 mL solution of 0.00380 M C2D3. What is pQsp for A2D5?
Calculate the pH during the titration of 50.00 mL of0.0500 M NaOH with 0.100 M HCl at 25oC after theaddition of the following volumes of reagent:a. 0.00 mLb. 10.00 mLc. 15.00 mLd. 20.00 mLe. 24.5 mLf. 25.00 mLg. 25.5 mLh. 27 mL
Indicator A B C pKIndicator 3.8 9.3 5.0 Actual Transition Range (pH) 3.0 to 4.6 3.0 to 4.6 4.4 to 6.2 Consider the titration of 50.00 mL of 0.1000 mol L-1 NH4OH (Kb = 1.75 x 10-5) with 0.1000 mol L-1 HCl.Based on the table above, select the most appropriate indicator to accompany this titration. Justify your choice. What is the theoretical transition range of indicators A, B and C?
A student used 9.925 x 10-2 mol/L hydrobromic acid to standardize an aqueous solution of potassium hydroxide and obtained the following titration data using phenolphthalein as an indicator: Concentration of HBr used: 9.925 x 10-2 mol/L Volume of HBr used: 25.00 mL Indicator: phenolphthalein Endpoint colour change: colorless to pale pink Table 1: Volume of Potassium Hydroxide Required Burette reading (mL) Trial 1 Trial 2 Trial 3 Final reading 29.28 36.62 43.98 Initial reading 1.78 9.28 16.62 Volume of KOH used (mL) Average of 2 closest values to within 0.10 mL: Questions Complete Inclosed table Write the molecular equation for the reaction that occurs between potassium hydroxide and hydrobromic acid. Calculate the molar concentration, in mol/L, of the aqueous potassium hydroxide.
For Ca2+ and Mg2+ determinations in a tap water sample, two 50 mL aliquots were pipetted and placed in different Erlenmeyer flasks. The first of them had the pH adjusted to 12 (Ca2+ titration) and the second to 10 (Ca2+ +Mg2+ titration). The volumes of EDTA (5.07*10-3 mol/L) used in the first and second titrations were 2.40 and 4.80 mL, respectively. Calculate: a) The concentration of Ca2+ in mg/L in the water sampleb) The concentration of Mg2+ in mg/L in the water sample
Consider the titration of 20 mL of 0.10 M base with 0.20 M HCl. The analyte is dibasic withpKb1 = 5.00 and pKb2 = 10.00. Calculate the pH at the following volumes of HCl0 mL, 5 mL, 10 mL, 15 mL, 20 mL
Use acid-base titration to determine theconcentration of:– A strong acid: HCl 0.100 M NaOH (standardized)•0.100 M HCl0.100 M CH3COOH Phenolphthalein is used for endpoint determination– Changes from colourless to pink as a solution becomes more basic• Only need 2-3 drops per titration• pH range: 8.3-10
How many grams of potassium napthenate (KC11H7O2; MW=210.27 g/mole; Kb=85x10-10) must be added to 50.0 ml of 0.4 M Naphthenic acid (HC11H7O2; Ka=5.4x10-5) to obtain a buffer with pH 5.0?
Calculate pAg at each of the following points in the titration of 20.00 mL of 0.0500 M AgNO3 with 0.0250 M NH4SCN.Ksp AgSCN = 1.10 × 10-12 a. 0.00 mL NH4SCNb. 20.00 mL NH4SCNc. 40.00 mL NH4SCNd. 45.00 mL NH4SCNe. 50.00 mL NH4SCN