6.20 mL of tap water sample is taken in a conical flask and 1 mL ofpH 10 buffer and 3 drops of iochrome black-T indicator are addedand when titrated with 0.001 M EDTA solution, 16 mL EDTA is spent,so the hardness of the water is determined by French Hardness andGerman Hardness Calculate in terms. 5. In an experiment to quantify an unknown amount of FeS04sample, 0.1 M KMN04 solution was prepared in the first step. Then,0.216 g H2C204 acid was added to a 250 mL flask, dissolved in 50mL deionized water and 5 drops of concentrated sulfuric acid wasadded. The mixture in the flask was heated up to 70 oC and titratedwith KMN04, which was prepared as 0.1 M. The turning point wasobserved when 12 mL of KMN04 was consumed in the titrationprocess. In the second step, the sample is placed in a 250 mL flaskand dissolved in 50 mL of deionized water. Calculate the amount ofFeS04 in the sample since 25 mL of KMN04 is consumed when 5mL of sül diluted sulfuric acid is added and titrated with a regulatedKMN04 solution.

"Since you have asked multiple questions, we will solve the first question for you. If you want any…

6. 20 mL of tap water sample is taken in a conical flask and 1 mL of pH 10 buffer and 3 drops of iochrome black-T indicator are added and when titrated with 0.001 M EDTA solutien, 16 mL EDTA is spent, so the hardness of the water is determined by French Hardness and German Hardness Calculate in terms.

6. 20 mL of tap water sample is taken in a conical flask and 1 mL of pH 10 buffer and 3 drops of iochrome black-T indicator are added and when titrated with 0.001 M EDTA solutien, 16 mL EDTA is spent, so the hardness of the water is determined by French Hardness and German Hardness Calculate in terms.

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

Similar questions

A 100-mL sample of hard water is titrated with the EDTA solution in Problem 2. The same amount of Mg2 is added as previously, and the volume of EDTA required is 31.84 mL. a. What volume of EDTA is used in titrating the Ca2 in the hard water? _____________mL b. How many moles of EDTA are there in that volume? _____________ moles c. How many moles of Ca2 are there in the 100 mL of water? _____________ moles d. If the Ca2 comes from CaCO3, how many moles of CaCO3 are there in one liter of the water? How many grams of CaCO3 are present per liter of the water? _____________ mol / L _____________ g / L e. If 1 ppm CaCO3 = 1 mg per liter, what is the water hardness in ppm CaCO3? _____________ ppm CaCO3
Calculate for titer: (in mgCaCO3/mL EDTA) Molarity of Trials: Trial #1: .01083 M EDTA #2: .01069 M EDTA #3: .01077 M EDTA
In an unprecedented initiative, the professor chose you to carry out the determination of a special sample in order to verify the inherent indication system. For that, an aliquot of 25.00 mL of a solution containing Fe(III) salts was titrated with EDTA 0.00982 mol/L, using potassium thiocyanate as indicator. In this case, you have found the volume of 31.10 mL of titrant to End Point. Based on the information given in the table, choose the option that best describes/explains the process linked to the indication system of the Final Point of the degree: (a) The indication of the system will be given by the disappearance of the reddish coloration, due to the displacement reaction: Fe(III) complex with EDTA is formed in detriment of the Fe(III) complex with thiocyanate. (b) The indication of the system will be given by the appearance of a reddish color, in function of the displacement reaction: Fe(III) complex with thiocyanate is formed in detriment of the Fe(III) complex with EDTA. (c) The…
If a 25.00 ml aliquot of a solution containing sulfide ions was added to 25.00 ml of 0.0139 M Cu2+ solution. The CuS precipitate was washed and collected. The pH of the combined filtrate and washings was then adjusted by the addition of ammonia and the solution was titrated with 0.01453 M EDTA, using a suitable indicator. The endpoint volume was found to be 10.66ml. Find the molarity of the sulfide in the sample solution.
A 110.00 mL solution of 0.00195 M A3B2 is added to a 160.00 mL solution of 0.00155 M C3D4. What is pQsp for A3D2?
Data Table for Weak Acid Vol. of Titrant pH Avg. Vol. ∆pH/∆vol 0 2.881 0.25 0.622575 0.5 3.193 0.75 0.453769 1 3.420 1.25 0.32668 1.5 3.583 1.75 0.251434 2 3.709 2.25 0.20456 2.5 3.811 2.75 0.173202 3 3.897 3.25 0.150977 3.5 3.973 3.75 0.134517 4 4.040 4.25 0.12191 4.5 4.101 4.75 0.112002 5 4.157 5.25 0.104057 5.5 4.209 5.75 0.097586 6 4.258 6.25 0.092253 6.5 4.304 6.75 0.087819 7 4.348 7.25 0.084111 7.5 4.390 7.75 0.081001 8 4.431 8.25 0.078391 8.5 4.470 8.75 0.076209 9 4.508 9.25 0.074397 9.5 4.545 9.75 0.072912 10 4.582 10.25 0.071719 10.5 4.617 10.75 0.070794 11 4.653 11.25 0.070117 11.5 4.688 11.75 0.069675 12 4.723 12.25 0.06946 12.5 4.757 12.75 0.069467 13 4.792 13.25 0.069696 13.5 4.827 13.75 0.070152 14 4.862 14.25 0.070845 14.5 4.897 14.75 0.071787 15 4.933 15.25 0.072999 15.5 4.970 15.75 0.074507 16 5.007 16.25 0.076346 16.5 5.045 16.75 0.078561 17 5.085 17.25 0.081211 17.5 5.125 17.75 0.084372 18…
If the water sample used for titration was buffered with acid instead of alkali, the amount of EDTA required to reach the endpoint will: a. stay constant b. be indeterminatec. increased. decrease
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)