5. A student conducted a titration experiment. He/she used 12.0 mL of silver nitrate (titrant) solution to reach the endpoint. If the student used 25.4 mL of the chloride (analyte) for the titration and found the concentration of chloride ions to be 2.2 M, what is the mass (in grams) of silver nitrate titrant LaClic

5. A student conducted a titration experiment. He/she used 12.0 mL of silver nitrate (titrant) solution to reach the endpoint. If the student used 25.4 mL of the chloride (analyte) for the titration and found the concentration of chloride ions to be 2.2 M, what is the mass (in grams) of silver nitrate titrant LaClic

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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4. The concentration of a NaOH solution is determine by using the solution to titrate a sample of potassium hydrogen phthalate (C8H5O4K, M = 204.22 g/mol). In the titration 34.67 mL of NaOH solution is required to react with 0.1082 g C8H5O4K to reach the equivalence point. a) Calculate the concentration of the sodium hydroxide solution. Potassium hydrogen Phthalate = 0-10829, Molar mass of KMP=204-22 Hales of KMP = Mass 0.10829 g/mol Mm 6.000529 mal 204229/Mal Concentration of NaOH = Males = = of volume of Naot (L) = 0-000529 mal 34-67 mе onl ها NaOH (mal) = 0.000015258 mal/L 0.015M b) This solution of sodium hydroxide is used for another titration. A sample of 10.0 mL of HCI is neutralized using 22.1 mL of sodium hydroxide solution. Calculate the concentration of the HCI solution. sodium hydroxide 222.1 ml, Nal100
24.16 mL of 0.2704 M sodium hydroxide is titrated with 29.00 mL of phosphoric acid. Calculate the molarity of phosphoric acid.
Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g Calculate the molarity of an NaOH solution from the following titration data. Be sure the answer has the correct amount of significant figures. The chemical equation for this titration is as follows: NaOH + KHP ⟶ NaKP + H2O NaOH buret reading, inital: 15.27 mL NaOH buret reading, final: 8.32 mL Mass of KHP (204.22 g/mol): 1.1592 g
25.0-mL samples "A" and "B" (both containing HCl) were titrated with 0.100 M NaOH. When titrating sample "A", it took 23.8 mL of titrant to reach the endpoint. When titrating sample "B", it also took 23.8 mL of titrant to reach the endpoint. Which of the following is correct? a. Sample A has a higher concentration of HCl b. Sample B has a higher concentration of HCl c. Sample A has the same concentration as Sample B d. We are unable to deduce the concentration of either sample.
You are trying to determine the percentage of acetic acid in vinegar by titrating a sample of the vinegar with a standardized NaOH solution. Why is bromcresol green not a good choice for an indicator for this titration? If you do use bromcresol green as an indicator, will your result for the percentage of acetic acid in vinegar be too high or too low? What would be a better choice for an indicator for this titration? Why is your choice better?
A student is asked to standardize a solution of sodium hydroxide. He weighs out 1.09 g potassium hydrogen phthalate (KHC8H404, treat this as a monoprotic acid). It requires 33.5 mL of sodium hydroxide to reach the endpoint. Use the References to access important values if needed for this question. A. What is the molarity of the sodium hydroxide solution? This sodium hydroxide solution is then used to titrate an unknown solution of nitric acid. Submit Answer M B. If 18.7 mL of the sodium hydroxide solution is required to neutralize 10.3 mL of nitric acid, what is the molarity of the nitric acid solution? 2 question attempts remaining M
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A solution of malonic acid, H2C3H2O4H2C3H2O4 , was standardized by titration with 0.1000 M NaOHNaOH solution. If 20.19 mLmL of the NaOHNaOH solution were required to neutralize completely 12.25 mLmL of the malonic acid solution, what is the molarity of the malonic acid solution? H2C3H2O4+2NaOH→Na2C3H2O4+2H2OH2C3H2O4+2NaOH→Na2C3H2O4+2H2O
7. 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 titration.
Question 4: After the student made the working NaOH solution above, he conducted a titration of an HCl solution of unknown concentration. If the student used a 20.5 ml aliquot of the HCl solution and used 22.7 ml of the NaOH solution from #3 above to reach the endpoint, what is the concentration of the HCl solution?
In an experiment to determine the molar mass of an unknown monoprotic acid, a 8.642×10-2 g sample of the acid was titrated with 0.107 mol L-1 of KOH. The equivalence point of the titration was found to occur when 23.38 mL of the KOH solution was added. What is the molar mass of the unknown acid?