A 100-mL solution of the ion Mg2+ at a concentration of 0.0500 M buffered to pH 9.00 was titrated with 0.0500 M EDTA. (a) The formation constant is 1.0 x 1012 and aY(H) = 0.041 ( pH=9.00 ) . Calculate the value of the effective formation constant. (b) Calculate the concentration of Mg2+ at VEDTA = Ve .

A 100-mL solution of the ion Mg2+ at a concentration of 0.0500 M buffered to pH 9.00 was titrated with 0.0500 M EDTA. (a) The formation constant is 1.0 x 1012 and aY(H) = 0.041 ( pH=9.00 ) . Calculate the value of the effective formation constant. (b) Calculate the concentration of Mg2+ at VEDTA = Ve .

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter12: Spectrochemical Methods

Section: Chapter Questions

Problem 15P

See similar textbooks

Similar questions

2) A 100.0 mL sample of drinking water was treated with ammonia buffer and after addition of Eriochrome Black T indicator, required 18.0 mL of 0.00559 M EDTA for titration. (a) Identify the role of ammonia buffer in the analysis. (b) Identify the indicator and endpoint color. (c) Calculate the total hardness of the water sample as ppm CaCO
Titration of Ca2+ and Mg2+ in a 50.00-mL sample of hard water required 23.65 mL of 0.01205 M EDTA. A second 50.00-mL aliquot was made strongly basic with NaOH to precipitate Mg2+ as Mg(OH)2(s). The supernatant liquid was titrated with 14.53 mL of the EDTA. Calculate the concentration in ppm of CaCO3 in the sample. Calculate the concentration in ppm of MgCO3 in the sample.
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
WARIARTAM 2. 1.2589 g of a certain brand of milk powder required 25.89 mL of 0.01873M EDTA to titrate the calcium contained in the sample. (a) What is the percent calcium in the sample? (b) Would the true result be higher, lower, or not be affected if the milk powder sample has been slightly wet?
A 100.0 mL sample of drinking water was buffered at pH 10.0 and, after addition of Calmagite indicator, required 38.11 mL of 4.652 x 10-2 M EDTA for titration. Calculate the total hardness of the water as (a) ppm CaCO3 and (b) ppm CaO|
Titration of Ca 2+ and Mg 2+ in a 50.00 ml sample required 25.50 mL Of 0.01115 M EDTA. A second 50 ml aliquot was made strongly basic with NaOH to precipitate the Mg 2+ as Mg(OH) 2(s). The supernatant liquid was titrated with 16.19 mL of the EDTA solution. Calculate the concetration in ppm of CaCO 3 in the sample О а. 100 O b.568.65 О с. 361.04 O d. 207.61
Be sure to answer all parts. Find the pH during the titration of 20.00 mL of 0.1000 M triethylamine, (CH3CH2)3N (K, = 5.2 x 10), with 0.1000 M HCl solution after the following additions of titrant. %3D (a) 10.00 mL: pH =9.72 (b) 20.70 mL: pH =|8.25 (c) 28.00 mL: pH =|10.17 %3D
A 25.00 ml of Ni2* solution was diluted in HCI and treated with 25.00 ml of 0.05283 M NazEDTA. The solution was neutralized with NaOH followed by addition of acetate buffer until the pH 5.5. The solution turns yellow after addition of few drops of xylenol orange indicator. Back titration using standard 0.022 MZn2* at pH 5.5 requires 17.61 ml until end point, on which the solution will turn red. Calculate for the molarity of the unknown. Ans. 0.03664 M
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.
In a precipitation titration, a 50.0 mL of 0.100 M NaCl was titrated with a standard solution of 0.10 M AgNO3. The titration was carried out with the addition of 0.0, 10.0, 50.0 and 55.0 mL AgNO3. Calculate the pCl and pAg for each addition of AgNO3. (Ksp for AgCl is 1.7 x 10-¹0)
Enumerate at least 2 specific biological applications of precipitation titration and discuss each.
Five drops of dichlorofluorescein have been added to a solution containing 0.800 g sample which required 25.30 mL of 0.100 M AgNO3. (a) Identify the type of argentometric titration method used.