Concentration of EDTA solution is 1.006 mg CaCO3/mL 10mL of unknown diluted with 40mL of distilled water 5mL of buffer and 5 drops of indicator what is the mg, ppm, and molarity for both trials?? Unknown titration with EDTA Trial 1 Trial 2 Volume of titrated 10mL 10mL Final Buret volume 4.1 4.5 Initial Buret Volume 25 25 Volume of EDTA solution used 20.9 20.5 mg of CaCO3 in sample ppm CaCO3 in sample Molarity of Ca2+

Concentration of EDTA solution is 1.006 mg CaCO3/mL 10mL of unknown diluted with 40mL of distilled water 5mL of buffer and 5 drops of indicator what is the mg, ppm, and molarity for both trials?? Unknown titration with EDTA Trial 1 Trial 2 Volume of titrated 10mL 10mL Final Buret volume 4.1 4.5 Initial Buret Volume 25 25 Volume of EDTA solution used 20.9 20.5 mg of CaCO3 in sample ppm CaCO3 in sample Molarity of Ca2+

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.28QAP

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A 0.3012g sample of an unknown monoprotic acid requires 24.13mL of 0.0944MNaOH for neutralization to a phenolphthalein end point. There are 0.32mL of 0.0997MHCl used for back titration. a. How many moles of OH are used? How many moles of H+ from HCl? _______moles OH ________moles H+ b. How many moles of H+ are there in the solid acid? Use Eq.5. ____________ moles H+ in solid c. What is the molar mass of the unknown acid? Use Eq.4. ____________ g/mol
4) A 25.00-mL sample of vinegar is diluted with deionized to 100.0 mL. Then a 10.00-mL aliquot (portion) of the dilute vinegar solutionis titrated with 0.1055 M NaOH solution using phenolphthalein as theindicator. (a) If 19.60 mL of the base solution is required to reach the end-point, calculate the molar concentration of acetic in dilute vinegar solution. (b) What is the molar concentration of acetic acid in the original (undiluted) vinegar? The acid-base reaction occurs as follows: HC2H3O2(aq) + NaOH(aq) --> H2O(l) + NaC2H3O2(aq)
A 25.00-mL sample of vinegar is diluted with deionized to 100.0 mL. Then a 10.00-mL aliquot (portion) of the dilute vinegar solutionis titrated with 0.1055MNaOHsolution using phenolphthalein as theindicator. (a) If 19.60mL of the base solution is required to reach the end-point, calculate the molar concentration of acetic in dilute vinegar solution. (b) What is the molar concentration of acetic acid in the original (undiluted) vinegar? At the end-point, the volume of NaOH consumed was found to be 32.00 mL. The acid-base reaction occurs as follows: HC2H3O2(aq) + NaOH(aq) --> H2O(l) + NaC2H3O2(aq)
A titrant solution of KMNO4 was standardized with 0.2g of Na2C2O4 amd consumed 27.75 mL to reach endpoint. What is the standardized normal concentration of the titrant?
Salt (NaCl) in food is determined by a potentiometric titration with silver nitrate as titrant and precipitation of Chloride. The salt content of a cracker is determined by extracting 10.0g of cracker with 100.0ml of water, filtered, and a 25ml aliquot titrated with 0.02M AgNO3. It takes 17.25ml to reach the end point. Calculate the weight % salt in the cracker.
It is desired to determine the concentration of chlorides in a powdered milk following the method of Volhard, for such case 1.5g of milk is weighed, it is heated in a muffle until obtaining ashes, which are treated with acid water with some drops of HNO3, the solution is filtered and the obtained filtrate is collected in an Erlenmeyer and 20 mL of AgNO3 0 is added. 1M excess silver is titrated with 0.05M potassium thiocyanate, if 8 mL of KSCN has been used up at the time of the indicator turn. Calculate the % of chloride in the milk powder.
Directions: Solve the problem with a complete step-by-step solution. Titration of 0.2121 g of pure Na2C2O4 (134.00 g/mol) required 43.31 mL of KMnO4. What is the molar concentration of the KMnO4 solution? The chemical reaction is 2MnO4- + 5C2O42- + 16H+ + ----> 2Mn2+ + 10CO2 + 8H2O
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If you had used 40mL of wash water to was .8555g of AgCl precipitate, and yhe wash water became 60% maximum saturation, how many grams of AgCl would you be washing away? Ksp for AgCl=1.8x10^-10 what % error too low would be in ur final answer, ie what % of the solid would be washed away
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Unknown titration with EDTA	Trial 1	Trial 2
Volume of titrated	10mL	10mL
Final Buret volume	4.1	4.5
Initial Buret Volume	25	25
Volume of EDTA solution used	20.9	20.5
mg of CaCO_{3 in sample}
ppm CaCO_{3 in sample}
Molarity of Ca²⁺