Titration data (5 pts) Titration 1 Titration 2 Titration 3 Volume of diluted bleach 10.0mL 100m2 Paulib) doe 10.0mL Volume of sodium thiosulfate 76.2 16.0mL 16. Ime (0.0250 M Na2S2O3) Moles of Na2S2O3 4.05x104 mol 4.0x104mol 4.02×10-40 mol Molar ratio of S2032: CIO 2:1 2.02x104 Moles of NaOCI mol 2.0x10mol 2.01×10-4 mol Molarity of diluted bleach 2.02x10-2m mul 2.0x10² mul 2.01x10-2 mul Mean molarity of diluted bleach 2.01x10-2 mul

Titration data (5 pts) Titration 1 Titration 2 Titration 3 Volume of diluted bleach 10.0mL 100m2 Paulib) doe 10.0mL Volume of sodium thiosulfate 76.2 16.0mL 16. Ime (0.0250 M Na2S2O3) Moles of Na2S2O3 4.05x104 mol 4.0x104mol 4.02×10-40 mol Molar ratio of S2032: CIO 2:1 2.02x104 Moles of NaOCI mol 2.0x10mol 2.01×10-4 mol Molarity of diluted bleach 2.02x10-2m mul 2.0x10² mul 2.01x10-2 mul Mean molarity of diluted bleach 2.01x10-2 mul

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter24: The Standardization Of A Basic Solution And The Determination Of The Molar Mass Of An Acid

Section: Chapter Questions

Problem 3ASA: A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to...

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A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
Malonic acid (HO2CCH2CO2H) is a diprotic acid. In the titration of malonic acid w ith NaOH, stoichiometric points occur at pH = 3.9 and 8.8. A 25.00-mL sample of malonic acid of unknown concentration is titrated with 0.0984 M NaOH, requiring 31.50 mL of the NaOH solution to reach the phenolphthalein end point. Calculate the concentration of the initial malonic acid solution. (Sec Exercise 113.)
Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
3. One erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HC1 (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used?
Identify which indicator will be suitable for the following titrimetric analyses: a. 0.100 M solution of HOAc (Ka = 1.78 x 10-5 ) with 0.100 M NaOH. b. 0.0527 M solution of NH4Cl (Kb = 1.80 x 10-5) with 0.100 M NaOH. c. 0.0162 M solution of piperidine hydrochloride (Kb 1.60 x 103) with 0.100 M NaOH.
What is the percentage of total acid expressed as acetic acid in a sample of vinegar if 4.0g of vinegar requires 29.5ml of 0.153N KOH for an endpoint with phenolphthalein indicator? (molar mass of acetic acid: HC2H3O2 = 60.05g/mol a. 3.995% b. 6.776% c. 8.650% d. 12.68%
A solution of HCl was titrated against sodium carbonate. What is the titer for Trial 1 in the given data? T2 0.3562 0.3479 0.3042 Weight (g) Initial V (ml) 0.80 1.60 35.20 36.70 39.80 Final V (ml) Vol HCI used (ml) 35.10 N of HC (eq/L) 0.1954 0.1870 Average N of HCl (eq/L) A
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
5. One Erlenmeyer contains 50 mL of 0.1 M Na2CO3 solution, the other Erlenmeyer contains 50 mL of 0.1 M NaHCO3 solution. Answer the following questions when both solutions are titrated with 0.1 M HCl (F=1) solution separately: a) How much mL will be consumed if the phenolphthalein indicator is used? b) How much mL will be consumed if the methyl orange indicator is used?
If a 300 mg sample of Sodium Bicarbonate (98% NaHCO3) is titrated with 0.922 N sulfuric acid, what volume of the acid should be required to produce an end point? Atomic Weights :Sodium - 22.99Oxygen - 15.999Hydrogen - 1.008Sulfur - 32.06 Enter numerical value only; round off to 4 decimal places
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