C1. A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible. What is the molar concentration of the standardized EDTA solution? (use C1 as reference)* 0.08m 0.8M 0.08N 0.08M How many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?* 0.1825 0.1852 1.825 1.1852

C1. A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible. What is the molar concentration of the standardized EDTA solution? (use C1 as reference)* 0.08m 0.8M 0.08N 0.08M How many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?* 0.1825 0.1852 1.825 1.1852

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.29QAP

See similar textbooks

Similar questions

DATA AND RESULTS: Titration Data (Standardization of EDTA) Example II Mass, g Caco, 0.0250 0.0251 0.0246 0.0254 Final reading, mL 25.00 24.91 24.87 25.31 Initial Reading, mL 0.00 0.02 0.02 0.02 Volume, mL EDTA 25.00 Molarity of EDTA, M 0.009992 B. Analysis Data Example II Volume of Sample, mL 25.00 24.90 25.10 25.0 Final reading, mL 27.46 25.08 25.06 24.99 Initial Reading, mL 0.00 0.02 0.02 0.02 Volume of EDTA, mL 27.46 Molarity of EDTA, M 0.009992 Ca" concentration, ppm 440 STATISTICAL EVALUATION OF RESULTS Standardization of EDTA Mean, M EDTA Median, M EDTA Standard Deviation Ci for u at 95% Prob. Level Reported value: M EDTA Ca" Concentration Mean, Ca" ppm Median, Ca" ppm Standard deviation Cl for u at 95% Prob. Level Reported value: Ca" ppm
The Cl– content of a solution was analyzed via an EDTA titration. 2.00 g of AgNO3 was added to 25.00 mL of the sample solution. A titration with 0.096 53 M EDTA was then carried out, reaching an endpoint at 38.25 mL. What’s the concentration of Cl – (M)?
A carefully weighed 280mg Calcium carbonate was used in the standardization of an EDTA solution. Initially, 25mL of the titrant was consumed but only after the addition of another 10mL of the titrant did an endpoint was visible.What is the MW of calcium carbonate?102 g/mol98 g/mL100 g/mL100 g/molWhat is the molar concentration of the standardized EDTA solution?0.08m0.8M0.08N0.08MHow many grams of EDTA (MW: 292 g/mole) is required to prepare 250mL of a 0.025M solution?0.18250.18521.8251.1852
A 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution. It is determined that 8.54 mL of EDTA is required to reach the end point. The blank titre was determined to be 1.50 mL. Determine the concentration of Calcium in the water sample in ppm. (mwt. of CaCO3 = 100.0892 g/mol).
4G I. Instagram +962 7 9927 4145 تحديد 1 من الصور Imssb1.mutah.edu.jo/n 0 PHag question New August 17, 2020. Titration of 50.00 mL of 0.05251 M NazC204 required 36.75 mL of a potassium permanganate solution, 2MNO4 + 5H2C204 + 6H* - 2Mn2* + 10CO2(g) + 8H20, Calculate the molarity of the KMNO4 solution. Select one: a. 0.02858 M b. 0.1429 M c. 0.03573 M d. 0.07144 M Next page Ouiz novigation
5. A 300.0 mg sample containing Na,CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
If in procedure B analysis of Zn2+ alone, 8.55 mL of 0.0100 M EDTA solution is used to fully titrate the Zn2+ content (FW = 65 g/moL) in the 10-mL of brass working solution, then mmol of Zn2+ is present in the 10-mL solution. Therefore, the Zn2+ concentration in the working solution is mM. Taken into the 10x dilution from the "stock solution", we can determine the concentration of the stock to be mM. Since there are total of 100-mL of stock solution, there are a total of mmol of Zn in the washer, which is mg (3 s.f.).
5. A 300.0 mg sample containing Na,CO3, NaHCO, and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1000 M HCI the titration required 24.41 ml to reach the phenolphthalein endpoint. And an additional 8.67 mL to reach the methyl red endpoint. Determine the composition of the sample and calculate the percent of each titrated component.
In the titration of MgSO4.2H2O (2g per litre) against a 0.01 M solution of the disodium salt of ethylenediamine tetraacetic acid (EDTA) the titres obtained were as follows ; titre 1: start - 0.7 ml and end - 13.3 ml (12.6ml) titre 2: start - 13.3 ml and end 25.7 ml (12.4ml) The average titre is 12.5ml Q. Calculate, based on the average titre of the accurate titres, the percentage of magnesium in the magnesium salt
In the determination of Ca2+ in milk powder, 12.1 mL 0.01 M EDTA is used for 1.50 grams of sample. Which of the following is the percentage of Ca2+ in the sample? (Ca: 40 g / mol) A. 0,32 B. 0,48 C. 0,96 D. 0,16
3. A sample of pure CaCO3 (MW 100.09) weighing 0.4148 g is dissolved in 1: 1 hydrochloric acid and the solution is diluted to 500 mL in a volumetric flask. A 50.0 –mL aliquot is withdrawn with a pipet and placed in an Erlenmeyer flask. The solution is titrated with 40.34 mL of an EDTA solution using Erichrome Black T indicator. Calculate the molarity of the EDTA solution. Hint: This problem involves analysis of an aliquot from a standard solution. In solving for the molarity of the EDTA solution, you should consider the amount of the standard in the aliquot which is used in the titration process. In this analysis, one mole of CaCO3 reacts with one mole of EDTA.
A 50.00 mL aliquot of standard CaCO3 (0.3834g CaCO3 per liter) consumed 42.35 mL of EDTA solution. The same EDTA standard solution was used for the titration of a 3.00 mL water sample. This required 30.56 mL of the titrant. Calculate the molar concentration of EDTA standard solution. What is the total hardness of water sample (then after solving explain how it come up to the final answer.)