Medical Chemistry Exam Super saturated solutions * Darker color Lighter color Intermediate color Coulometric titrimetry: The time required to Consuming the analyte for the standard solution Fractionation the analyte for the standard solution Destroyed the analyte for the standard solution Organic chemistry it deals with Living organisms

Medical Chemistry Exam Super saturated solutions * Darker color Lighter color Intermediate color Coulometric titrimetry: The time required to Consuming the analyte for the standard solution Fractionation the analyte for the standard solution Destroyed the analyte for the standard solution Organic chemistry it deals with Living organisms

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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QUESTION 6 Which of the following steps MUST be done prior to titration of an analyte? I. Prepare a standardized solution II. Wash the burette with a standardized solution III. Fill the burette to the 50-ml mark IV. Prepare a contrast paper to determine burette volume and titration endpoint I, Il and IV only I, III and IV only O I, Ill and IV only O , II, and II only
1. What must be the normality of a solution of silver nitrate so that each milliliter shall be equivalent to 6mg of sodium chloride? 2. If 44mL of EDTA solution was measured using 202mg of calcium carbonate, what is the molarity of the solution? 3. A volumetric solution was standardized against oxalic acid, H2C2O4The volume of solution required to neutralize 1.8231 grams of oxalic acid dihydrate was 38.24 mL. What is the normality and molarity of the VS? 4. How many grams of sodium carbonate are needed to react with one liter of a 0.05M NaOH solution?
list the apparatus involved in volumetric or titrimetric analysis
The Mg2+ concentration in a saturated solution of magnesium hydroxide is measured and found to be 1.59 \times 10-4 M. Use this information to calculate a Ksp value for magnesium hydroxide.
Sodium iodate is added to a solution containing calcium, cobalt (II), copper (II), and lead (II) ions to selectively precipitate a target ion out of solution. If the ions that needs to be removed is the one that will form a precipitate first, which ion is target of the selective precipitation? Calcium iodate Cobalt (II) iodate Copper (II) iodate Lead (II) iodate Copper (II) Calcium lodate Cobalt (II) Lead (II) Ksp = 6.47 x 106 Ksp = 1.21 x 102 Ksp = 6.94 x 108 Ksp = 3.69 x 10-13
a) Amount of Ba(NO3)2 dissolved in grams. Molar mass of Ba(NO3)2 = 261.3g/molb) Solubility product, Kspc) Vapor pressure of the solution in kPa
Answer the following questions. 5-6
Titration of a 0.500 g sample with 0.50 mL of 0.011 M potassium dichromate required 15.80 mL of standard 0.1160 M silver nitrate solution. Calculate the weight percent of NaCl (F W=58.44 g/mol) in the sample. * Identify the name of the Argenometric method used * Identify the indicator in the titration * Identify the color at the endpoint
Calculate the solubility of Mg(OH)2 in water at 25 °C. You'll find Ksp data in the ALEKS Data tab. Round your answer to 2 significant digits. ☐ x10
2. After dissolving the KHP with water, a student noticed some undissolved solid, but continued with the titration as instructed by the procedure. He titrated until the pink color persisted for 30 sec and recorded the volume of titrant required. Preparing for the second determination, he set the reaction solution aside and added some more NaOH to the buret. He was about to pour the reaction solution down the drain, so he could rinse and reuse the flask, when he saw that the pink color had disappeared! a) What happened? b) What can the student do to correct for this erTor and salvage this trial? How should the data sheet be modified to reflect this correction? 3. Another student began adding titrant to the acid solution, but stopped when she suddenly realized that she forgot to add the 3 drops of phenolphthalein. When she did, the solution immediately turned dark red! a) What happened? b) What can the student do to correct for this error and salvage this trial? How should the data sheet…
A 5.4681 gram sample of beef was analyzed for its N (14g/mole) content and the liberated NH3 was collected in a 99.31 mL of 0.2012 M HCI and 6.28 mL back titration with 0.0120 M NaOH was required. Calculate the percentage protein in the beef sample. (Answers should be written in 2 decimals place and do not include the UNIT)
What happens to the particles of a precipitate if particle growth is the dominant process by which they form? Small but many Large and many Large but few Small and few