For problem 5, the density of the sample is 0.9977 g/ml. and the molar mass of calcium carbonate is 100.0g/mol.5.As described in Topic 2 in the lab manual, the hardness of water is expressed in terms of amountof calcium carbonate according to the ppm expression.Calculate the mass of calcium carbonate present in a 50.00 mL sample of an aqueouscalcium carbonate standard, assuming the standard is known to have a hardness of75.0 ppm (hardness du to CaCO;).a.b.Calculate the number of moles of calcium ions present in this 50.00 mL sample ofaqueous calcium carbonate standard.C.The 50.00 mL sample (at pH 10) was titrated with a 0.00500 M EDTA solution,Write the balance net ionic equation for the reaction of EDTA“ with a calcium ion.Calculate the number of moles of EDTA“ needed to completely react with calciumions in the sample.What volume (in milliliters) of EDTA solution would be needed to reach theequivalence point?

a) 50 ml = 50/1000 L = 0.05 L ppm = mass…

Answered: balance net ionic equation for the…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.9QE

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Calculate the concentration of SCN in each of the following standard solutions. Use 0.0500 M Fe3+ and 0.00200 M SCN- a. 1.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL) b. 2.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL) c. 3.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL) d. 4.00 mL SCN- + 5.00 mL Fe3+ (final volume = 10.00 mL)
a. A 1.00 liter solution contains 0.45 moles nitrous acid and 0.35 moles potassium nitrite .If 0.17 moles of hydroiodic acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of hydroiodic acid.) A. The number of moles of HNO2 will decrease. B. The number of moles of NO2- will decrease. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase. b. A 1.00 liter solution contains 0.38 M ammonia and 0.49 M ammonium bromide. If 0.120 moles of barium hydroxide are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of barium hydroxide.) A. The number of moles of NH3 will decrease. B. The number of moles of NH4+ will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will increase. E. The ratio of [NH3] /…
A 1.00 liter solution contains 0.60 moles nitrous acid and 0.46 moles potassium nitrite .If 0.23 moles of perchloric acid are added to this system, indicate whether the following statements are true or false.(Assume that the volume does not change upon the addition of perchloric acid.) A. The number of moles of HNO2 will increase. B. The number of moles of NO2- will remain the same. C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HNO2] / [NO2-] will increase.
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An analyst was titrating a solution of unknown acetic acid concentration with 0.01 M NaOH using phenolphthalein as indicator. After adding exactly 39.4 ml of the titrant drop-wise, the analyte solution started to turn light pink. The titrant volume 39.4 ml is best referred to as the O equivalence point. Onone of the choices O standardization point. O equilibrium point. O endpoint.
What is standard solution ? Why is a standard solution necessary for titration?

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