Do the argentometric titration according to given data and fill in the blanks. Ag+ (aq) + Cl- (aq) → AgCl (s) (White) NaCl → Nat + Cl- SET 2 Measured Weight of NaCl, (gr) 2.5 g Measured Weight of Cl- , (g) Volume of Stock Solution, (mL) 200 mL Amount of Sample taken from the stock solution, (mL) 9mL Normality of AgNO3 , (N) 0.1 N Initial burette reading, (mL) O mL Final burette reading, (ml) 6.85 mL Volume of AGNO; Consumed, (mL) 6.85 mL Amount of AGNO; Consumed, (mg) Calculated Weight of NaCI in stock Solution, (g) Calculated Weight of CI- in stock Solution, (g) Error in Calculating Amount of CI--(%)

Do the argentometric titration according to given data and fill in the blanks. Ag+ (aq) + Cl- (aq) → AgCl (s) (White) NaCl → Nat + Cl- SET 2 Measured Weight of NaCl, (gr) 2.5 g Measured Weight of Cl- , (g) Volume of Stock Solution, (mL) 200 mL Amount of Sample taken from the stock solution, (mL) 9mL Normality of AgNO3 , (N) 0.1 N Initial burette reading, (mL) O mL Final burette reading, (ml) 6.85 mL Volume of AGNO; Consumed, (mL) 6.85 mL Amount of AGNO; Consumed, (mg) Calculated Weight of NaCI in stock Solution, (g) Calculated Weight of CI- in stock Solution, (g) Error in Calculating Amount of CI--(%)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Show the complete mole ratio of S2O3- and IO3- in computing for the Molarity of the titrant. Redox Titration mass IO3(g) initial volume mL final volume mL trial 1 0.1587 0.00 3.60 trial 2 0.1571 3.60 7.17 trial 3 0.1552 7.17 10.72
100.0 cm3 water is titrated with 0.0049 M ascorbic acid solution. What is the analytical concentrationof the weak acid at 12.73 cm3 added titrant volume?
A student performed titration to determine the concentration of potassium permanganate solution with oxalic acid. The net ionic equation is as follows: 2MnO4– + 16H+ + 5C2O42- → 2Mn2+ + 10CO2 + 8H2O The titration consumed 42.31 mL of 0.1001 M oxalate solution to reach the endpoint. Determine the concentration of permanganate (M) if 25 mL was used.
Please don't provide handwritten solution ......
7B-3. A 15.00 mL sample of an unknown perchloric acid solution is titrated with a 0.687 M barium hydroxide solution. It takes 29.31 mL of the base solution to reach the endpoint. а. Write a balanced chemical equation for the reaction that occurs. b. What is the molarity of the unknown acid solution?
You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?
A reg1.hu.edu.jo العربية ENGLISH Question 4/12 ميز هذا السؤال Titration of 0.2121 g of primary standard Na2C204 (133.999 g/mol) required 21.66 mL of KMNO4 (158.034 g/mol) to reach the end point. Calculate the molar concentration of KMNO4? 2 MnO4¯+ 5 C204²-+ 16 H+ → 2 Mn2+ 10 CO2 +8 H2O 1. 00.0146 2. 00.0292 3. 00.00731 4. 00.1462
A sample of antacid tablet that contains NaHCO3 is analyzed in the lab. The student dissolves 1.50g tablet in 35.0 mL of HCl solution containing 0.0300 mole of HCl. The back-titration of the excess HCl require 10.5 mL of 2.05M NaOH solution. 1) If that tablet label showed that each tablet contains 0.950 gram of NaHCO3. Determine the percent error in the student experiment. 2) Calculate the mass percent of the NaHCO3 in the tablet.
I titrate a 5.00mL aliquot of Arsenic acid with 36.09 mL 0.126M sodium hydroxide. Calculate the molarity of the arsenic acid sample.
7.7 g of citric acid (MM = 192.1 g/mol) can be titrated with NaOH according to the following balanced chemical equation. H3C6H5O7 (aq) + NaOH(aq) → H2O(l) + Na H2C6H5O7(aq) what would the curve for the titration of the neutralization of the three hydrogens of this acid with NaOH look like?
You collected the following data from a titration experiment using a 0.118M standardized NaOH solution to titrate a 26.65 mL solution with an unknown Molarity concentration (M) of sulfuric acid (H2SO4). Find molarity Initial Burette Reading (mL) Final Burette Reading (mL) Vol Delivered (mL) Molarity Trail #1 0.15 19.47 19.32 ?
A solution of malonic acid, H2C3H2O4H2C3H2O4 , was standardized by titration with 0.1000 M NaOHNaOH solution. If 21.68 mLmL of the NaOHNaOH solution were required to neutralize completely 13.00 mLmL of the malonic acid solution, what is the molarity of the malonic acid solution? H2C3H2O4+2NaOH→Na2C3H2O4+2H2OH2C3H2O4+2NaOH→Na2C3H2O4+2H2O