What is the purity of the limestone in terms of %w/w CaCO3? Zhongli is a speleologist tasked to analyze the CaCO, content of a limestonestalactite. A 5.0000-g sample was dissolved in 25.00 mL of 1.350 M HCI, it wasthen heated to expel any CO2 formed. The excess HCI was titrated to aphenolphthalein end point, it used 37.50 mL of 0.1200 M NAOH.This problem will cover the next 4 items

Initial number of moles of hydrochloric acid can be determined as follows: Number of moles =…

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What is the purity of the limestone in terms of %w/w CaCO3?

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

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 132IP: A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in...

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A 10.00-g sample of the ionic compound NaA, where A is the anion of a weak acid, was dissolved in enough water to make 100.0 mL of solution and was then titrated with 0.100 M HCl. After 500.0 mL HCl was added, the pH was 5.00. The experimenter found that 1.00 L of 0.100 M HCl was required to reach the stoichiometric point of the titration. a. What is the molar mass of NaA? b. Calculate the pH of the solution at the stoichiometric point of the titration.
A solution containing a mixture of metal cations was treated with dilute HClHCl and a precipitate formed. The solution was filtered, and H2SH2S was bubbled through the acidic solution. A precipitate again formed and was filtered off. Then, the pH was raised to about 88 and H2SH2S was again bubbled through the solution. This time, no precipitate formed. Finally, the solution was treated with a sodium carbonate solution, which resulted in the formation of a precipitate. Classify the metal ions based on whether they were definitely present, definitely absent, or whether it was possible they were present in the original mixture.
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I would really appreciate some help in confirming a value computed in a prelab problem to be used in a lab for analytical chemistry! We're working on redox reactions and are looking at the reaction: Fe2+ + K2Cr2O7 + H+ = Fe3+ + K+ + Cr3+ + H2O The final questions asks, "calculate the amount of unknown sample needed to achieve about a 25.00 mL titration volume of 0.01600 M K2Cr2O7 if the %Fe of the unknown is approximately 8%. Make sure to use the coefficients from the balanced reaction" I have found the balanced equation; however, I was hoping to be able to confirm my values! Thank you in advance!
A solid sample of Zn1OH22 is added to 0.350 L of 0.500 Maqueous HBr. The solution that remains is still acidic. It isthen titrated with 0.500 M NaOH solution, and it takes 88.5mL of the NaOH solution to reach the equivalence point.What mass of Zn1OH22 was added to the HBr solution?
1. 0.646 g of sample containing BaCl2.2H2O (244.26 g/mol) was dissolved and enoughpotassium chromate was added. After filtering, the precipitate was dissolved in acid andenough KI was added and titrated with thiosulfate. Since 48.7 mL of 0.137 M thiosulfateis used for this, what is the percentage of BaCl2.2H2O in the sample?K2Cr2O7 + 7H2SO4 + 6KI  4K2SO4 + Cr2(SO4)3 + 7H2O + 3I2
A buffer is made from 25.0mL of 1.0M CH3COOH and 25.0mL of 1.0M CH3COONa, what would be the pH of the buffer?
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