19. If you used more than half of your NAOH solution in buret-refill It to the 0 mL mark on the fon If vou have more than 30 ml. Jeft. vou do pot need to refill the buret 1. Data Group1 Group 2 Group 3 Group 4 Group 5 Group 6 Volume of vinegar 2 25.00/25.0 25.00 / 25.00 sample 25.00/ 25.00 25.00/ 25.00 25.00/ 25.00 25.00/ 25.00 transferred, mL Molarity of sodium hydroxide solution, M 0.7784 0.7784/ 0.8161 / 0.8161 0.8211/ 0.8211 0.7784 / 0.7784 0.8161 / 0.8161 0.7784/ 0.7784 Final buret reading, 4 mL 26.90 / 26.73 24.10 / 25.65 23.85/ 24.00 28.10 / 27.85 26.20/ 27.00 29.10 / 28.80 Initial buret reading, mL 0.00/ 0.00 0.00/ 0.00 0.00 / 0.00 0.00/0.00 0.00/0.00 0.00/ 0.00

19. If you used more than half of your NAOH solution in buret-refill It to the 0 mL mark on the fon If vou have more than 30 ml. Jeft. vou do pot need to refill the buret 1. Data Group1 Group 2 Group 3 Group 4 Group 5 Group 6 Volume of vinegar 2 25.00/25.0 25.00 / 25.00 sample 25.00/ 25.00 25.00/ 25.00 25.00/ 25.00 25.00/ 25.00 transferred, mL Molarity of sodium hydroxide solution, M 0.7784 0.7784/ 0.8161 / 0.8161 0.8211/ 0.8211 0.7784 / 0.7784 0.8161 / 0.8161 0.7784/ 0.7784 Final buret reading, 4 mL 26.90 / 26.73 24.10 / 25.65 23.85/ 24.00 28.10 / 27.85 26.20/ 27.00 29.10 / 28.80 Initial buret reading, mL 0.00/ 0.00 0.00/ 0.00 0.00 / 0.00 0.00/0.00 0.00/0.00 0.00/ 0.00

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 25P

See similar textbooks

Similar questions

A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
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?
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?
Explain why calcium sulfate is less soluble in sodium sulfate solution than in pure water.
Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
Supersaturated solutions of most solids in water are prepared by cooling saturated solutions. Supersaturated solutions of most gases in water are prepared by heating saturated solutions. Explain the reasons for the difference in the two procedures.
Explain why barium fluoride dissolves in dilute hydrochloric acid but is insoluble in water.
Explain why an acid-base indicator changes color over a range of pH values rather than at a specific pH.