5. You start with 25.00 mL of 1.00 M NaOH. After 4.32 g leaves produce CO₂ over a period of days, you precipitate out the sodium carbonate and titrate the leftover NaOH. The titration requires 22.44 mL of 1.00 M HCl. (see lab for hint on how to solve this problem if you need help!) How many moles of sodium hydroxide reacted with the leaves? How many moles of CO₂ was produced? How many grams of CO2 were produced per day per gram of leaf?

5. You start with 25.00 mL of 1.00 M NaOH. After 4.32 g leaves produce CO₂ over a period of days, you precipitate out the sodium carbonate and titrate the leftover NaOH. The titration requires 22.44 mL of 1.00 M HCl. (see lab for hint on how to solve this problem if you need help!) How many moles of sodium hydroxide reacted with the leaves? How many moles of CO₂ was produced? How many grams of CO2 were produced per day per gram of leaf?

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section: Chapter Questions

Problem 108GQ

See similar textbooks

Similar questions

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 1.00 liter solution contains 0.35 M ammonia and 0.27 M ammonium bromide.If 0.13 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 NH3 will decrease. B. The number of moles of NH4+ will remain the same. C. The equilibrium concentration of H3O+ will increase. D. The pH will decrease. E. The ratio of [NH3] / [NH4+] will increase.
A 1.00 liter solution contains 0.36 moles hydrofluoric acid and 0.28 moles sodium fluoride .If 0.14 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 HF will remain the same. B. The number of moles of F- will decrease. C. The equilibrium concentration of H3O+ will increase. D. The pH will remain the same. E. The ratio of [HF] / [F-] will remain the same.
A 1.00 liter solution contains 0.59 M ammonia and 0.45 M ammonium bromide.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 NH3 will increase. B. The number of moles of NH4+ will remain the same. C. The equilibrium concentration of H3O+ will decrease. D. The pH will remain the same. E. The ratio of [NH3] / [NH4+] will remain the same.
A 1.00 liter solution contains 0.36 moles hydrocyanic acid and 0.28 moles potassium cyanide. If 0.14 moles of hydrochloric 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 hydrochloric acid.) ✓ A. The number of moles of HCN will decrease. True B. The number of moles of CN will increase. False C. The equilibrium concentration of H3O+ will remain the same. D. The pH will increase. E. The ratio of [HCN] [CN] will increase.
A 1.00 liter solution contains 0.48 M ammonia and 0.37 M ammonium iodide. If 0.18 moles of hydrobromic 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 hydrobromic acid.) 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 decrease. D. The pH will remain the same. E. The ratio of [NH3] / [NH4+] will decrease.
What volume of 0.1951 M NaOH is needed to titrate 19.5100 m L of 0.2130 M acetic acid to the phenolphthalein endpoint? Answer with two decimal places. Your Answer: Answer View hint for Question 3. units H
Vinegar? required to neutralize the acetic acid in each sample of vinegar, 16. Complete the calculations to find the molarity and percentage of acetic acid in vinegar. Convert the average volume of NaOH required to reach endpoint from mL to L Average volume of NaOH required to reach endpoint in mL 15. Subtract the initial volume from the final volume to calculate the volume of NaOH I DATA 269 12.55 TITRATION DATA (REPORT YOUR VOLUMES TO 1/100TH MI TRIAL 1 TRIAL 2 Initial base buret reading Final base buret reading Volume of sodium hydroxide (NaOH) required to reach endpoint in mL Volume of vinegar used O15 12.55 TRIAL 3 12:55 24.11 EXTRA TRIAL 24.11 35.39 11.78 12.05 11.56 15.00 mL 15.00 mL 15.00 mL 15.00 mL (Show calculations here.) 12.05711-56+1178 -27.54 27.54ML (Show calculations here.) a7.54ML X IL 0-02754L :0.02754L nd bon 1600 Molarity of NAOH (recorded from the standard solution bottle) 0.1 I CALCULATIONS FOR MOLARITY OF ACETIC ACID IN VINEGAR 1. Using the known molarity of…
Suppose a student performed a similar standardization titration experiment. Below is the calculated concentration of NaOH from each of their titrations. Titration #1 Titration #2 Titration #3 Concentration of NaOH (M) 0.9554 0.9540 0.9551 Using the 3 concentrations, calculate the average concentration of the student's NaOH solution and calculate the ± error in parts per thousand (ppt). Show the complete calculation. Express your final answer in the form of average (with units) ± error in ppt. use the right significant figures
A 1.00 liter solution contains 0.45 M hydrocyanic acid and 0.58 M sodium cyanide. If 0.15 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 HCN will decrease. B. The number of moles of CN will remain the same. BC. The equilibrium concentration of H3O+ will remain the same. D. The pH will remain the same. E. The ratio of [HCN] [CN] will increase.
PRE-LAB QUESTIONS Calculate the volume, in mL, of a 0.50 M NaOH solution that will be required to titrate 1.2 g of potassium hydrogen phthalate to the phenolphthalein end point. The molar mass of KHP is 204.2 g/mol. 1.
Suppose a student performed a similar standardization titration experiment. Below is the calculated concentration of NaOH from each of their titrations. Titration #1 Titration #2 Titration #3 The concentration of NaOH (M) 0.9554 0.9540 0.9551 Using the 3 concentrations, calculate the average concentration of the student's NaOH solution and calculate the ± error in parts per thousand (ppt). Show the complete calculation. Express your final answer in the form of average (with units) ± error in ppt.