Suppose you are titrating a solution of sodium oxalate, which has a molar mass of 134 g/mol, with a potassium permanganate solutionaccording to the equation2 MnO4 + 16 H +5 C2O4²- → 2 Mn²+ + 10 CO2 + 8 H2OIf you require 13.9 mL of 0.0372 M KMNO4 solution to titrate the Na,C,0, solution, what is the mass of Na, C2O4 present in thesolution?Type answer:

Number of moles of potassium permanganate should be equal to sodium oxalate at the equivalence…

Suppose you are titrating a solution of sodium oxalate, which has a molar mass of 134 g/mol, with a potassium permanganate solution according to the equation 2 MnO4 + 16H +5 C,O,²- 2 Mn2+ + 10 CO, + 8 H2O If you require 13.9 mL of 0.0372 M KMNO4 solution to titrate the Na C,0, solution, what is the mass of Na,C2O4 present in the solution? Type answer:

Suppose you are titrating a solution of sodium oxalate, which has a molar mass of 134 g/mol, with a potassium permanganate solution according to the equation 2 MnO4 + 16H +5 C,O,²- 2 Mn2+ + 10 CO, + 8 H2O If you require 13.9 mL of 0.0372 M KMNO4 solution to titrate the Na C,0, solution, what is the mass of Na,C2O4 present in the solution? Type answer:

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

Mark and John, two vinegar enthusiasts, are each tasked to determine the acetic acid content of their respective vinegar concoctions by titration. First, a 1 M-labeled KOH solution was standardized against the KHP (MW = 204.22 g/mol) standard that is 99.4% pure. In the process, 0.540 g KHP was found to require 2.80 mL of the KOH solution to completely react up to the phenolphthalein endpoint. Then, Mark and John both prepared their samples by taking 10.0-mL aliquots of each vinegar and diluting them to 25.0 mL. Using the same titrant and indicator, Mark’s vinegar required 18.60 mL of the standardized titrant to reach the endpoint, while John’s vinegar required 16.50 mL of the same titrant to reach the same endpoint. Question: What is the acetic acid concentration of Mark’s and John’s vinegar in molarity given that the Concentration of KOH is 9386 M?
to 70 ml of 0.2M Pb solution (NO3) 2 add 30 ml of 0.7 M KIO3 solution. a) Write the equation of the chemical reaction and calculate the number of moles of Pb2 + and IO3- ions before mixing b) count the number of moles of Pb2 + and IO3- ions after mixing, knowing that Ksp of Pb (IO3) 2 = 2.5 × 10-¹³
OCHEMICAL REACTIONS Determining the volume of base needed to titrate a given mass... chemistry student weighs out 0.0570 g of chloroacetic acid (HCH₂CICO2) into a 250. mL volumetric flask and dilutes to the mark with distilled water. He lans to titrate the acid with 0.2000M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the equivalence point. Be sure your answer has the correct number of significant digits. mL Explanation Check AUG 2 0.0 X e S tv W 3/5 X MacBook Air Hu © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center A
Please give complete answer with explanation
Please help
Jack determines the concentration of NaOH by titrating it with 4.0 g KHP (a monoprotic acid). It takes 21.2 mL of NaOH to reach the equivalence point. What is the concentration of the NaOH? molar mass of KHP 204.2 g/mol [NaOH] = [?] M [NaOH], M Enter
solution after precipitation is complete. 68. The drawings below represent aqueous solutions. Solution A is 2.00 L of a 2.00-M aqueous solution of copper(II) nitrate. Solution B is 2.00 L of a 3.00-M aqueous solution of potas- sium hydroxide. (0) suiro Cu²+ ebro NO3 БО K+ OH™ A B a. Draw a picture of the solution made by mixing solutions A and B together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions A and B, and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in M) of all ions left in solution (from part a) and the mass of solid formed.
10- A solution with a volume of 100 ml is prepared by weighing 2.50 g from the mixture of Kl and KBr. When 10 ml of this solution is titrated with 0.015 M AgNO3 solution, there is a consumption of 105. Accordingly, calculate the percentage of Kl in the mixture A)88,4 B)43,7 C)56,3 D)11,6
if 100 mL of 0.100 M Cu(NO3)2 is reacted with 50 ml of .20 M NaOH, according to the following reaction how many moles of Cu(OH)2 will be formed? Cu(NO3)2 + 2NaOH > Cu(OH)2 + 2NaNO3
Questions 5-10 refer to the same weak acid/strong base (WA/SB) titration. The K₂ of hypobromous acid is 2.8 x 10-⁹. A 30.00 mL solution of 0.300 M hypobromous acid (HBrO) is being titrated with a solution that is 0.600 M in lithium hydroxide (LiOH). What is the total solution volume (in mL) at the equivalence point? (Nearest whole number) Type your answer...
Suppose you are titrating a sulfuric acid solution of unknown concentration with a sodium hydroxide solution according to the equation H2SO4+2NaOH⟶2H2O+Na2SO4HX2SOX4+2NaOH⟶2HX2O+NaX2SOX4 If you require 26.63 mL of 0.910 M NaOH solution to titrate 180.9 mL of H2SO4 solution, what is the concentration of the H2SO4 solution?
A 24.8mL sample of vegetable juice is titrated with 15.65mL of NaOH solution. The molar concentration of the NaOH is .106 M. The molar mass of citric acid is 192.12 g-mol-1. Express all with three significant figures. A) Determine the molar concentration of citric acid in the vegetable juice sample B) Determine the number of moles of citric acid per 240 mL of the vegetable juice. C) Determine the mass of citric acid per 240 mL of the vegetable juice. D) If the label on the bottle lists the citric acid contest as 1g per serving with a serving size of 240 mL determine the percent error in the rotation results. Express in 2 sig figs.