Multiple Choice Each of the numbered items or incomplete statements is followed by answers or by completions of the statement. Select the one lettered answer or completion that is best in each case. Write your answer before each number. 18.This is the weight of the substance chemically equivalent to 1 mL of the standard solution: a. End point C. Titrand b. Titer d. Equivalence point 19. The apparatus used to wash down drops of standard solution clinging to the tip of the buret is: a. Cassia flask C. Bobcock bottle b. Wash bottle d. Plastic bottle 20. The following characteristics of product with quality, except G

Multiple Choice Each of the numbered items or incomplete statements is followed by answers or by completions of the statement. Select the one lettered answer or completion that is best in each case. Write your answer before each number. 18.This is the weight of the substance chemically equivalent to 1 mL of the standard solution: a. End point C. Titrand b. Titer d. Equivalence point 19. The apparatus used to wash down drops of standard solution clinging to the tip of the buret is: a. Cassia flask C. Bobcock bottle b. Wash bottle d. Plastic bottle 20. The following characteristics of product with quality, except G

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter7: Neutralization Titrations And Graphical Representations

Section: Chapter Questions

Problem 1P

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Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
7. Describe a buffered solution. Give three examples of buffered solutions. For each of your examples, write equations and explain how the components of the buffered solution consume added strong acids or bases. Why is buffering of solutions in biological systems so important?
In Exercise 12.49, what is the allowed concentration of AgCl in g per 100 g of water? The Safe Drinking Water Act of 1974 established the maximum permitted concentration of silver ion at 0.05 ppm. What is the concentration of Ag+ in parts per million in a saturated solution of AgCl? (NOTE: 1 ppm = 1 mgofsolute/L of solution.)
If 55 mg of lead(II) sulfate is placed in 250 mL of pure water, does all of it dissolve? If not, how much dissolves?
Consider the following two acids: In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results. (See Exercise 113.)