Assuming that the concentration of EDTA for the experiment was 0.01 M in 20 ml tap water and the readings for Determination of total Mg2+ and Ca2+ is given below Observation Vol of EDTA (ml) 1st Titration (ml) 2nd Titration (ml) 3rd Titration (ml) Initial reading 0.00 3.00 6.00 Final reading 3.00 5.10 3.00 Vol. addede xxxxxxxx xxxxxxxx xxxxxx Determination of Ca2+ only is given below Vol of EDTA (ml) 1st Titration (ml) 2nd Titration (ml) 3rd Titration (ml) Initial reading 0.00 2.75 6.00 Final reading 2.75 5.00 3.20 Vol. addede xxxxxxxx xxxxxxxx xxxxxx Calculate: Concentration of Ca2+ in ppm = Concentration of Mg2+ in ppm =

Assuming that the concentration of EDTA for the experiment was 0.01 M in 20 ml tap water and the readings for Determination of total Mg2+ and Ca2+ is given below Observation Vol of EDTA (ml) 1st Titration (ml) 2nd Titration (ml) 3rd Titration (ml) Initial reading 0.00 3.00 6.00 Final reading 3.00 5.10 3.00 Vol. addede xxxxxxxx xxxxxxxx xxxxxx Determination of Ca2+ only is given below Vol of EDTA (ml) 1st Titration (ml) 2nd Titration (ml) 3rd Titration (ml) Initial reading 0.00 2.75 6.00 Final reading 2.75 5.00 3.20 Vol. addede xxxxxxxx xxxxxxxx xxxxxx Calculate: Concentration of Ca2+ in ppm = Concentration of Mg2+ in ppm =

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.19QAP

See similar textbooks

Similar questions

2,5 ml volume has taken from an “hypothetic” solution which includes (3+) Sb and (3+) Fe and at the titration with 0.1004 N KMnO4, the wasted amount has found as 16,4 mL. The other 2,5 mL that has taken, has reduced with Zn after that, this 2,5 mL solution has titrates with the same KMnO4 solution solution and the wasted amount is 26,5mL. With these datas find the %concentrations of the ions at the solution.
Data Table 1: Complexometric Titration of Hard Water 6ml of water used (5ml of hard water and 1ml of buffer) Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 0.55ml .50ml .33ml Volume of EDTA Consumed (mL) 0.45ml .50ml .77ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L): photo shows equation that needs to be used to solve
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…
For the complexiometric titration of Ca2 + ions in the shell of the egg sample weighing 62,576 g, the necessary procedures were applied to the egg shells and 100 mL sample was prepared. 1 mL of the prepared sample was taken and diluted to 100 mL, the pH was adjusted, and two drops of EBT indicator were dropped on it. The prepared solution was titrated with 23.6 mL of 0.0095 M EDTA solution. What is the value of the amount of calcium in the sample in terms of% CaCO3? (Ca: 40, C: 12, O: 16 g / mol)
The water hardness of tap water has been determined to be 120 (= 120 mg CaCO3 per 1 L of water). After the tap water has run through the ion exchange column, titration of a 20.00 mL sample used only 0.70 mL of 0.0100 M EDTA, to reach the endpoint. Calculate the effectiveness of the ion exchange column: what is the % of the calcium, removed by the ion exchange column? Provide your answer in % and without decimal. ( Please type answer note write by hend)
Calculate for titer: (in mgCaCO3/mL EDTA) Molarity of Trials: Trial #1: .01083 M EDTA #2: .01069 M EDTA #3: .01077 M EDTA
Data Table 3: Complexometric Titration of Soft Water 5 ml of water 1ml of buffer Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 77ml 79ml 75ml Volume of EDTA Consumed (mL) .23ml .21ml .25ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L):
Sources of Error Determine the relationship between the observed/apparent value (EX) VERSUS that of the true value (ET) for the quantity being sought by writing either <, >, or = on the space provided TOPIC: Measured mass of the precipitate 1. Filter paper was dried prior to filtration. EX _____ ET TOPIC: Standardization of Titrant 2. Distilled water was not equilibrated to room temperature before the preparation of NaOH titrant. EX ______ ET TOPIC: Determination of Molar Concentration of each component (Double Indicator Titration) 3. No blank correction EX ______ ET
100 mL water sample was subjected to DO analysis using the Winkler method. The initial reading of the titrant (0.025 M Na2SO3) in the buret was 2.51 mL. The endpoint was obtained and the final reading was 7.07 mL. A blank was also titrated and 0.75 mL of the titrant was consumed. Compute for the amount of DO (mg/L) in the sample.
Data Table 3: Complexometric Titration of Soft Water 6ml of water used (1ml of buffer and 5ml of soft water) Hard Water Trial 1 Hard Water Trial 2 Hard Water Trial 3 Initial Syringe Reading (mL) 1ml 1ml 1ml Final Syringe Reading (mL) 77ml 79ml 75ml Volume of EDTA Consumed (mL) .23ml .21ml .25ml Water Hardness ppm CaCO3 (mg/L) Average ppm CaCO3 (mg/L):
a 20 ml portion of a deep well water sample was diluted to 250 ml solution. a 50 ml aliquot of this diluted sample water was buffered at ph 10 and required 8. 50 ml of a standard EDTA.the titrant was standardized using 100ml containing 0.8622 mg primary standard calcium carbonate , which required 15.45 ml for titration.(a) identify a possible indicator and its endpoint color (b) calculate the molarity of the EDTA solution. (c) calculate the total hardness of the water as ppm CaCO3 (d) identify the quality of the water sample in terms of hardness
A RbOH solution is titrated four (4) times against potassium hydrogen phthalate (KHP; FW=204.224) samples to the Phenolphthalein endpoint. Using the data below, determine the concentration of the RbOH solution? g of KHP Volume of Base Required 0.5373 g 42.49 mL 0.5856 g 43.88 mL 0.5790 g 48.56 mL 0.5856 g 44.60 mL (Report your answer as "mean +/- std dev") M What is the percent relative standard deviation? % What is the 99% Confidence Interval for the concentration of the solution (population mean)?

SEE MORE QUESTIONS

Recommended textbooks for you

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

SEE MORE TEXTBOOKS

GET THE APP

About FAQ Academic Integrity Sitemap Document Sitemap

Contact Bartleby Contact Research (Essays)High School Textbooks Literature Guides Concept Explainers by Subject Essay Help Mobile App

GET THE APP

Privacy

Your CA Privacy Rights

Your NV Privacy Rights

About Ads

Manage My Data

bartleby, a Learneo, Inc. business

Vol of EDTA (ml)	1^st Titration (ml)	2^nd Titration (ml)	3^rd Titration (ml)
Initial reading	0.00	3.00	6.00
Final reading	3.00	5.10	3.00
Vol. addede	xxxxxxxx	xxxxxxxx	xxxxxx