Use the pC-pH diagram for open carbonatesystem to find the equilibrium pH for a solutionprepared by adding 10-5 molepH2145.8.9.1011 1213141.3.45n6.8.9.1011121314N22CO3 into 1L DI water. Hint: the solution isequilibrated with air above.Can you also show the purpose and relationship ofthe other lines on the graph as it relates to thequestion? Thanks!

Answered: Image /qna-images/answer/626f64e5-c2cd-42c1-b043-25979aa9c17b.jpg

Use the pC-pH diagram for open carbonate system to find the equilibrium pH for a solution prepared by adding 10-5 mole pH 8. 9. 10 11 12 13 14 1 2. 3. 4. 5. 6. 8. 9. 10 11 12 13 14 Na2CO3 into 1L DI water. Hint: the solution is equilibrated with air above. Can you also show the purpose and relationship of the other lines on the graph as it relates to the question? Thanks!

Use the pC-pH diagram for open carbonate system to find the equilibrium pH for a solution prepared by adding 10-5 mole pH 8. 9. 10 11 12 13 14 1 2. 3. 4. 5. 6. 8. 9. 10 11 12 13 14 Na2CO3 into 1L DI water. Hint: the solution is equilibrated with air above. Can you also show the purpose and relationship of the other lines on the graph as it relates to the question? Thanks!

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...

See similar textbooks

Similar questions

1). You are running an experiment and need to keep your solution within a certain pH range: 3.5 +/- 1pH unit. Choose a buffer system (e.g. a conjugate acid/base) with a pKa in the appropriate range.. Assuming you have 0.2M stock solutions of the acid and conjugate base, calculate the L of each need to make 400 mL of buffer. Describe clearly your protocol for making the buffer solution to the desired pH. Calculate pH for the following. Add 100 mL of 0.100 M HCl to pure water Add 100 mL of 0.100 M HCl to the 400 mL of buffer you made Add 100 mL of 0.100 M NaOH to pure water Add 100 mL of 0.100 M NaOH to the 400 mL of buffer you made
39. Three more samples of KHP (GFW=204.23g/mole) weighing 0.8001g, 0.7001, and 0.7666g were titrated with the same sodium hydroxide solution. The volumes for the titrations were 21.55mL, 17.44, and 18.37mL respectively. A.) Calculate three more values for the molarity =, then B.) Calculate the mean for all four measurements. And calculate the average for all for measureme ement ave. mean.
Select Weak Acid as the analyte in the titration interactive. Analyte, 25.0 ml. Weak Acid, 1.0.. Determine the pK, of this weak acid. colortess Indicator No Indicator 14 13.83 pK, = Incorrect pH=2.50 25 50 Titrant Added (mL) Titration Curve Concentration Chart Titrant: Strong Base, 1.0 M MOH 50 0.0 ml + Hd
Calculate the expected pH based on how the solution was prepared, again allowing for any dilution taking place. For Solutions 7 and 8, make sure to take into account the acid–base reaction that occurs when an acid or base is added to the buffer.
Give typed solution not written
I. Preparation of acetate buffer solutions with different pH values 1. Calculate the salt and acid volumes required to prepare 10 ml of the acetate buffer with the following ratio of sodium acetate and acetic acid: Test tube #1: Ratio - 1:9 Salt volume Acid volume ml ml
16.14
Give a clear handwritten answer with explanation...
6. Open the bags and add 3 drops of bromothymol blue to each bottle. The indicator turns yellow if vinegar is still present and is blue-green when vinegar is not present. Record the color of each solution in the table provided. Data Table 1: Reaction Data Sample 7. Add a 4 teaspoon of baking soda to each bag. Effervescence of CO₂ occurs if excess vinegar is present. Record your observations in the table provided. Moles of vinegar (mol) Moles of baking soda (mol) mistry Relative size of bag Was excess vinegar present? Color with indicator? Reacts with additional baking soda? Moles of gas produced (mol) Watch the limiting reagent! #1 0.042 0.014 чем yes yellow #2 0.042 0.028 #3 yes yellow 0.042 0.042 Experiment 11 yes yellow #4 Stoichiometry 0.042 0.88 more small big bigger bigger No 0.071 #5 NO Geen 0.042 Blue Calculations 1. Use Table 1 to determine which reactant was limiting in each trial. Use the amount of limiting reactant to calculate the moles of carbon dioxide gas that were…
4
Name: Date: Section: Report Sheet: pH: Measurement and Application. A: Determination of pH Using Acid-Base Indicators: Indicator Color NaH,PO, HC,H,O, ZNSO, Methyl Violet Thymol Blue Methyl Yellow Congo Red Bromocresol Green pH Range B: Measurement of the pH of Solutions Record the measured pH and the color observed using bromocresol green for each 0.1 M solution NaH,PO, HC,H,O, ZNSO, C: Determination of K, for a Weak Acid Volume Used(Liters) Moles [HC,H,O,] M HC,H;O, () HC,H,O, |NaC,H;O,] M NaC,H,O, (L) NaC,H,O; Buffer pH pK, HC,H,O, K, HC,H,O, 115
The potentiometric titration of a weak base against a stong acid is shown below. In the following problems, calculate the pH at different stages of the titration using the appropriate chemical equation & formula and then select the appropriate answer. Example of answer: Between pH 8 and 9. (no decimals) A.) - Between what is the pH of the solution before any strong acid has been added? - Between what is the pH of the solution after 10.00 mL strong acid has been added? - Between what is the pH of the solution after 25.00 mL strong acid has been added? - Between what is the pH of the solution after 40.00 mL strong acid has been added? - Between what is the pH of the solution after 50.00 mL strong acid has been added? - Between what is the pH of the solution after 60.00 mL strong acid has been added?