3. A 100 mL sample of hard water is titrated with 22.4 mL of the EDTA solution from problem 2. The same amount of MgCl, is added as previously and the total volume of EDTA solution required is 22.44 mL. a) What volume of EDTA is used in titrating the Ca2+ in the hard water? mL

3. A 100 mL sample of hard water is titrated with 22.4 mL of the EDTA solution from problem 2. The same amount of MgCl, is added as previously and the total volume of EDTA solution required is 22.44 mL. a) What volume of EDTA is used in titrating the Ca2+ in the hard water? mL

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Calculate the volume of 0.0407 M EDTA needed to titrate the Ca in a 0.1622 g CaCO3 (MM = 100.0869 g/mol).
If an unknown consisted of Co+2, Fe+2, Sr+2, or Ni+2, which cation would completely complex with EDTA first? Second? Third? Also, what are the minimum pH values for satisfactory titrations of the above metal cations?
The Telluride ion was determined by indirect titration with EDTA. To a solution containing 50.00 mL of 0.08664M Zn(CIOA)2 plus 15 mL of 1 M acetate buffer (pH 4.5) were added 50.00 mL of unknown telluride solution with vigorous stirring. The ZnTe precipitate was filtered and washed with hot water. Then NH3 was added to the filtrate (which contained excess Zn2+) until the blue colour of Zn(NH3)42+ was observed. Titration of the filtrate with 0.07854 M EDTA required 24.22 mL to reach the murexide end point. Calculate the molarity of telluride ion in the unknown.
Is this for Average Molarity of EDTA Standard Solution? Then, would it be always the same with average Molarity of EDTA? How about the Ca Titer (mg Ca/mL of EDTA Solution? Show step by step solution.
Calculations: Standardization of HCl Titrating Solution: Using your best two or three standardization titrations, calculate the concentration of the HCl titrating solution for each trial using the balanced equation between HCl and Na2CO3. What is the average concentration of your HCl solution? Ksp Determination at both temperatures Calculate the room temperature Ksp for borax. From the HCl volume used in each titration, calculate the concentration of borate in each room temperature aliquot using the equation between HCl and borate From the stoichiometric relationship between borate and sodium ion, calculate [Na+ ] in each aliquot. Calculate the room temperature Ksp for each titration using the following equation calculate the average Ksp value. Ice Bath Temperature Ksp Determination: Calculate Ksp for borax as you did for the room temperature system. Calculate the concentration of borate in each ice temperature aliquot. Calculate [Na+ ] for each ice temperature aliquot.…
Which rapid and quantitative analysis requires a sample solution of metal ion to be titrated against a standard solution of EDTA, in the presence of a buffer?* Alkalimetric Replacement Back Titration Direct Which agent is added into a solution if direct titration is deemed to proceed slowly?* Indicator Titrant Catalyst Demasking agent Which method uses an excess solution of EDTA added to a sample and then pH is adjusted for back titration with a metal ion solution?* Replacement Residual Alkalimetric Direct Which reagent will form a more stable complex with interfering ions rather than the with the indicator and EDTA?* Masking agents Demasking agents Chelating agents Complex agents Which of the following contains a set of incorrectly paired words?* Chelatometry - Complexation / Precipitimetry - Argentometric…
a. Calculate the molar solubility of AgI in pure water. Ksp for AgI is 1.5 x 10-¹6. Solubility= M b. Calculate the molar solubility of AgI in 3.3 MNH3. The overall formation constant for Ag (NH3)₂* is 1.7 x 107. Solubility= M c. Compare the calculated solubilities from parts a and b. O The solubility from (a) is greater. The solubility from (b) is greater. O The solubilities from (a) and (b) are the same.
You want to separate Cd2* and Fe2+ (initial concentration 103 mol/L) by means ofprecipitation of the corresponding sulphides. Is therea pH range in which one of the two metals is precipitated quantitatively(concentration in the solution less than or equal to 10" mol/L) is precipitatedwhile the other is still completely_in solution?Calculate and name this pH range where pH values below 0are set equal to O. Illustrate the situation graphically by drawing
Which of the following DOES NOT meet the requirement for primary standards? a. Large molar mass b. High affinity towards water c. High purity d. Soluble in titration medium
please sir just solve these the two questions
The answer to the previous question I calculated was 0.0324 M of the standard Ca solution and now I'm not sure what I'm doing wrong in my calculations for the next problem. 2. "For each of the calcium standard titrations, determine the exact concentration (M) of the EDTA solution, using the concentration of the standard Ca solution you calculated in 1. Find an average of the calculated concentrations." My volumes for the titrations were: Ca volume used in titration 1 = 10.00 mL and for the second titration = 9.98 mL Ca used EDTA volume used in titration 1 = 16.98 mL and for the second titration = 17.00 mL EDTA used
If you have a sample of 100 mg/L of calcium, and you have two standardized EDTA solutions of 0.005 M and 0.001 M, which one is more adequate to spend approximately 15.00 mL of the titrant if 25.00 mL of sample are added in the Erlenmeyer flask? How many mL of titrant will be used? Solution: The 0.005 M solution. 12.5 mL will be used.