Titration of 0.2342 g of pure Na,C,O, (134.0 g/mol) required 33.45 ml of KMNO, solution according to the chemical reaction: 2MNO, + 5C,0, +16 H* 2MN2+ + 10CO, +8H,0 The Molarity of KMNO, solution would be: a. 0.01609 M b. 0.04020 M c. 0.02090 M d. 0.20140 M e. 0.12450 M

Titration of 0.2342 g of pure Na,C,O, (134.0 g/mol) required 33.45 ml of KMNO, solution according to the chemical reaction: 2MNO, + 5C,0, +16 H* 2MN2+ + 10CO, +8H,0 The Molarity of KMNO, solution would be: a. 0.01609 M b. 0.04020 M c. 0.02090 M d. 0.20140 M e. 0.12450 M

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.42QAP

See similar textbooks

Related questions

Q: A student weighs out 0.9854 g of Na2CO3 unknown and dissolves it in 25.00 mL of deionized water. A…

A: Answer % of Na2CO3 in the unknown = 54.05% Formulas No.of moles = Given…

Q: odometric titration of Vitamin C with sodium thiosulfate How many moles of iodine (I2) react with…

A: Iodometric titration is a redox titration which shows the disappearance of iodine at the end point.…

Q: A 0.4755-g sample containing (NH,),C,O, and inert materials was dissolved in water and 3. strongly…

Q: Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the…

A: Density of commercial bleach solution = 1.08 g/mL

Q: Titration of a 0.7513-g sample of impure NazB,07 required 30.79 mL of 0.1129 M HCI. B40,2+ 2H3O*…

Q: The molarity of an EDTA solution is 0.0114 M. A 25.0 mL sample of water with unknown Ca+2…

A: Molarity is number of moles of solute present in 1 liter of solution. Mass of substance = molar mass…

Q: 1.963-g sample of an alloy is dissolved in HNO3 and diluted to volume in a 100-mL volumetric flask.…

Q: A student wanted to determine the percent of NaOCI in a commercial bleaching solution. He diluted…

A: Given data, Mass of bleach = 5.0g Volume of flask = 100mL=0.1L Volume of sample = 25mL=0.025L…

Q: A blank titration requires 0.65 mL to reach the same end point. Report the %w/w KBr in the sample.

A: The reaction will be: KBr(aq) + AgNO₃(aq) → KNO₃(aq) + AgBr(s) From the reaction- 1 mole of KBr…

Q: A 1.9300 g impure sample of Fe(NH4)2(SO4)2 (FW = 392.14) was dissolved in 75 mL 0.75 M H2SO4 and was…

Q: A 300.0-mg sample containing H3PO4 and inert material was diluted with water and titrated with…

A: Answer: Since, 2 water molecules are forming as a product, therefore balanced reaction between…

Q: A 0.8357 -g sample of a wheat flour was analyzed by the Kjeldahl procedure. The ammonia formed was…

A: Here we have to determine the mass percentage of protein present in 0.8357 g of wheat sample if the…

Q: Titration of 0.2342 g of pure Na,C,0, (134.0 g/mol) required 13.45 ml of KMNO, solution according to…

A: 1- Calculate the moles of C2O42- ion : moles = [ mass / Molar mass ] moles = [ 0.2342mol /…

Q: A 60.00 ml of a sample of river water was titrated with 0.0016 M of sodium dichromate and required…

A: given: volume of the sample of river water is 60.00 ml concentration of sodium dichromate is 0.0016…

Q: A 0.7120 g of iron ore was brought into solution and passed through a Jones reductor. Titration of…

A: The balanced redox reaction given is 5 Fe+2 + MnO4- + 8H+ → 5 Fe+3 + Mn+2 + 4 H2O Volume of KMnO4 =…

Q: 0.00247

A: Molarity of KMnO4 = 0.0010 M Volume of KMnO4 = 4.94 mL At equivalent point, Geq. of KMnO4 = Geq. of…

Q: 0.178 L of aqueous HCl solution of unknown concentration was titrated with 0.825 M KOH (aq). 68.4 mL…

A: here the question:- one unknown M we have to calculate using the ' MVHCl=MVKOH volume of HCl =0.178L…

Q: 12. A 0.5000-g sample that contains KCl and KI gives a precipitate of Aga and AgI that weighs 0.2818…

Q: A 0.1510 g KHP (MW = 204.22 g/mol) sample required a volume of 57.04 mL of NaOH solution to reach a…

Q: Molarity of Na2S2O3 (stock solution). 0.100 M Volume of diluted bleach titrated (taken from the…

A: Solution: For a given titration reaction the stoichiometric relation plays important role, as from…

Q: 23 The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.12 M…

A: The titration of 25.0 mL of an unknown concentration sulfuric acid solution requires 83.6 mL of 0.12…

Q: A 0.4755-g sample containing (NH,),C,O, and inert materials was dissolved in water and strongly…

Q: A solution of potassium permanganate is standardized using pure As2O3as the primary standard (upon…

A: we are required to find the molarity of the potassium permanganate.

Q: Titration of 0.2121 g of primary standard Na C,0, (133.999 g/mol) required 21.66 mL of KMnO,…

A: Given that: Mass of Na2C2O4 = 0.2121g Molar mass of Na2C2O4 = 133.999g/mol Moles of Na2C2O4 =…

Q: 2.4414 g sample containing KCl, K2SO4and inert materials was dissolved in sufficient water to give…

A: Given: Mass of sample = 2.4414 g. This sample contains KCl, K2SO4 and inert materials. The volume of…

Q: Titration of 0.2342 g of pure Na,C,0, (134.0 g/mol) required 33.45 ml of KMNO, solution according to…

Q: The titration of 20.0 mL of a H2SO4 solution requires 42.6 mL of 0.16 M LIOH solution. What is the…

A: The technique in which a solution of Known concentration is used to determine the concentration of…

Q: 1. A 1.000 g sample.containing Na,C,0, (MM=134 mg/mmol) is titrated with 40.00 mL of 0.0200 M KMNO,…

A: Given,

Q: Consider the titrimetric determination of acetic acid (60.05 g/mol) in vinegar. Titration of a 5.00…

A: Given: Concentration of NaOH = 0.250 M And volume of NaOH solution used = 16.15 mL = 0.01615 L…

Q: Mass of NaOCl in commercial bleach titrated. ?

A: Moles help to calculate mass

Q: 12. A 0.3284-g sample of brass (containing lead, zinc, copper, and tin) was dissolved in nitric…

A: First of all, the titration reaction with EDTA forms complexes that have 1:1 ratios of EDTA:Analyte.…

Q: 2.4414 g sample containing KCl, K2SO4and inert materials was dissolved in sufficient water to give…

A: Mohr method is the method to determine the chloride ion concentration of a solution. This is done by…

Q: The DO of a water sample used in a steel industry was tested by Winkler’s method. The following…

A: A question based on introduction to chemistry that is to be accomplished.

Q: The Zn in a 260-g sample of foot powder was titrated with 2 L of 0.5 M EDTA. Calculate the percent…

A: Given that - Mass of Sample of Zn = 260 g Volume of EDTA Solution = 2 L Molarity of EDTA Solution…

Q: Titration of 0.2342 g of pure Na,C,0, (134.0 g/mol) required 33.45 ml of KMNO, solution according to…

Q: The standardization of a KSCN solution against 0.3341 g of primary standard grade AgNO3 (M.M.…

A: standardization of KSCN by AgNO3 an aliqout of the sample of KSCN is taken and titrated against…

Q: A 25.0025.00 mL solution of 0.088300.08830 M NaINaI is titrated with 0.051500.05150 M AgNO3AgNO3.…

A: Consider dissolution of AgI as AgI (s) Ag+(aq) + I -(aq) For the above reaction, Ksp =[ Ag+ ][I-]…

Q: A 50.0 mL solution of Ca(OH)2 with an unknown concentration was titrated with 0.340 M HNO3. To reach…

A: Calcium hydroxide reacts with nitric acid to form calcium nitrate. In this reaction, calcium…

Q: Moles of OCl– in the diluted bleach titrated. ?

A: Iodine and hypochlorite play role in titration Moles of iodine play role in hypochlorite ions

Q: A sample of primary standard grade K2Cr2O7 (MM = 294.20) weighing 0.2153 g is dissolved, the…

Q: 0.753-g sample of a chlorocarbon compound was analyzed by burning it in oxygen and collecting the…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: 1. How many ml of 0.30M solution of H2SO4 will react with 20ml of a 0.30M solution of NaOH?…

A: Given values: n1 = 2 M1= 0.30M V1 = ? n2= 1 V2= 20ml M2= 0.30M n1, M1 and V1 are the…

Q: A 20.00 ml sample of H2SO4 solution of unknown concentration is titrated with 0.1203 M NaOH and…

A: Given that, Volume of H2SO4 solution V1= 20 mL Molarity of H2SO4 solution M1 = to be calculated…

Q: The Zn in a 0.7556-g sample of foot powder was titrated with 21.27 mL of 0.01645 M EDTA. Calculate…

A: Since you have posted multiple questions, we will solve only first question for you. If you want any…

Q: A 492-mg sample containing KH2PO4 (136.09 g/mol) is titrated with 0.112 M NaOH requiring 25.60 mL.…

A: Number of moles of NaOH should be calculated to determine the moles of KH2PO4 . Number of moles =…

Q: An EDTA solution is standardized against 0.3982 g of 99.99% CaCO3 (100.09 g/mol) dissolved in HCl…

A: given data mass of CaCO3 is 0.3982g the volume of EDTA Is 38.00Ml pH is 10.0

Q: A titration of 50.00 mL of 0.1100 M Fe3+ with 0.07750 M Sn2+ is carried out. The analytical reaction…

A: Equivalance point is the point where all moles of one reactant is neutralized by another compound.…

Q: A 0.5131-g sample containing KBr is dissolved in 50 mL of distilled water. Titrating with 0.04473 M…

A: The mass of sample containing KBr dissolved in 50 mL of distilled water is 0.5131 g. The volume of…

Question

Titration of 0.2342 g of pure Na,C,0, (134.0 g/mol) required 33.45
ml of KMNO4 solution according to the chemical reaction:
2MNO, + 5C,0, +16 H*
2MN2* + 10CO, +8H,0
The Molarity of KMNO, solution would be:
a. 0.01609 M
b. 0.04020 M
c. 0.02090 M
d. 0.20140 M
e. 0.12450 M
Please fill in the space with one of the following characters (a or b or c or d or e)

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1 given

VIEW

Step 2 Calculations

VIEW

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

You have performed an iodimetric titration using a commercial vitamin C tablet. Based on the following information below, calculate the %(w/w) of vitamin C(MM=176.16 g/mol) in the tablet: Mass of tablet dissolved in 250.0 mL: 5.422 g Aliquot volume of sample titrated: 25.00 mL Concentration of KIO3: 0.023 M Final burrette volume: 41.31 mL Initial burrette volume: 8.89 mL Blank volume: 0.14 mL
0.0585g of Na2C2O4, 10 mL of distilled water and 2 M H2SO4 were added to adjust the KMnO4 solution prepared as 0.1M. Heating process was carried out and 8.4mL of titrant was consumed as a result of titration. Calculate the true concentration of potassium permanganate accordingly.
A sample is analyzed for chloride by the Volhard method. From the following data, calculate the percentage of chloride present:Weight of sample = 6.0000 g dissolved and diluted to 200 mLAliquot used = 25.00 mL AgNO3 added = 40.00ml of 0.1234MKSCN for back titration = 13.20ml of 0.0930M
Suitable treatment of a 2.566 g soil sample converts all arsenic to AsO43-. 50.00 mL of 0.082 M Ag+ was added to form Ag3AsO4 precipitate. The excess Ag+ was back-titrated with 21.8 mL of 0.024 M SCN- to reach the equivalence point Ag+ + SCN- → AgSCN(s) Solve for the % As (MW = 74.92 g/mol) in the sample.
A 25.0025.00 mL solution of 0.088300.08830 M NaINaI is titrated with 0.051500.05150 M AgNO3AgNO3. Calculate pAg+pAg+ following the addition of the given volumes of AgNO3AgNO3. The KspKsp of AgIAgI is 8.3×10−178.3×10−17. 37.40 mLpAg+=37.40 mLpAg+= VepAg+=VepAg+= 47.30 mLpAg+=47.30 mLpAg+=
The titration of 0.5001 g of KHP with a purity of 98.5% (204.223 g/mol) required 25.10 mL of NaOH. Calculate the concentration of NaOH solution KHP reacts with NaOH in a 1:1 ratio.
1ml of 1mg/ml of diluted aspirin powder solution is titrated by 0.005M NaOH. Before titration, 5 ml ethanol, 14 ml CO2 free water, and 4 drops bromothymol blue indicator is added into diluted aspirin powder solution. Mass of 0.005M NaOH used is obtained by weight titration = 1.1384g . [Molar mass of aspirin =180.15]; for solution, 1g=1mL at 25 degree Celcius. Calculate the purity of the powder.
The SO2 present in air is mainly responsible for the phenomenon of acid rain. The concentration of SO2 can be determined by titrating against a standard permanganate solution as follows: 5SO2 + 2MnO4- + 2H2O ---> 5SO42- + 2Ms2 + 4H+ Calculate the number of grams of SO2 in a sample of air if 4.90mL of 0.00700M KMnO4 solution are required for the titration. Be sure your answer has the correct number of significant digits.
Calculate the concentration of Fe2O3 in a mineral sample after solubilization of 0.4891g and availability of Fe as Fe2+. The released Fe2+ ions were titrated with a 0.02153 mol/L K2Cr2O7 solution requiring 36.92 mL to reach the end point of the titration. Show the calculations and express the concentration in % m/m. K2Cr2O7; + 6Fe2+ + 14H+ → 2Cr+3 + 2K+ + 6Fe3+ + 7H20
The phosphate in a 3.000 g sample of industrial detergent was precipitated by the addition of 1.000 g of AgNO3. The solution was filtered and the filtrate required 18.23 mL of 0.1377 M KSCN for titration to the FeSCN2+ end point. Calculate the percentage of phosphate in the detergent.
A 0.3285 g sample containing chloride and inert material is titrated with 0.1012 M AgNO3, requiring 34.99 mL to reach the Ag,Cro. end point. Titration of a blank sample consumes 0.32 mL of the AgNO, titrant. Determine the % w/w chloride in the sample.
A salt sample was analyzed for its purity. A 0.5000g sample was dissolved in water and diluted to 250.0mL. From this solution, 25.00mL was taken for analysis. To this aliquot, 20.00mL of a 0.08735M AgNO; solution was added to precipitate the chloride. The excess AgNO required 12.45mL of a 0.09473M KSCN solution for back-titration. Calculate the purity of the salt sample as percent by mass of KCI (74.55 g/mol). (Answer: 84.63% KCI)