Acetic acid is added to DI water at an initial concentration of 10 -6 M (Ka=1.8x10-5)A. Using the "ICE" Method, what would the pH be at equilibrium? State assumptions and show yourwork.B. Using the simultaneous equations method, what would the pH be at equilibrium? Show your work

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Answered: Acetic acid is added to DI water at an…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter6: The Systematic Approach To Equilibria: Solving Many Equations

Section: Chapter Questions

Problem 13P

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Quantity Your Data 1. Grams of vinegar sample used for your titration 25.000 g 2. Initial Buret Reading of Sodium Hydroxide solution 10.00 mL 3. Final Buret Reading of Sodium Hydroxide solution 28.00 mL 4. Amount of Sodium Hydroxide Solution used to neutralize the vinegar sample 5. Concentration of NaOH in the NaOH solution 0.050 g/mL 6. Grams of NaOH used to neutralize the vinegar 7. Grams of acetic neutralized by the amount of NaOH 8. Percent acetic acid in the vinegar Hints: For #4, The amount of NaOH used is the difference between the starting buret value and the ending buret value. For #6, Once you calculate the amount of sodium hydroxide used, multiple that value by the concentration of NaOH in the NaOH solution. For #7, Multiply the value obtained in number 6 by the number 1.5. Remember, we learned that every 1 gram of NaOH neutralizes 1.5 grams of acetic acid. For #8, Divide the grams of acetic acid by the grams of vinegar sample and multiply this value by…
please help I am having a difficult time answering these questions. I am submitting it as one because they are all related so please answer all of them. Fill in the entire table and then answer the following questions. please type the answers ( show all steps, states of matter for all equations.) all these questions are related to that pre-lab table. 1. Fill in the following table with the Ksp values for any insoluble salt that forms from a metal ion in the left column and the anions in the other columns. Some have already been provided for you. If a salt is soluble in water write N/A. a) Why were you unable to find some of the Ksp values for some ions? 2. In a test tube containing a precipitate of PbCrO4 in water: What are the concentrations of the lead (II) and chromate ions in equilibrium with the solid? Show your calculations. Use the Ksp from the Prelab table above . [Pb+2] = M [CrO4-2] = M 3. How can AgCl(s) be dissolved…
please help I am having a difficult time answering these questions. I am submitting it as one because they are all related so please answer all of them. Fill in the entire table and then answer the following questions. please type the answers ( show all steps, states of matter for all equations.) all these questions are related to that pre-lab table. 1. Fill in the following table with the Ksp values for any insoluble salt that forms from a metal ion in the left column and the anions in the other columns. Some have already been provided for you. If a salt is soluble in water write N/A Prelab Table. Selected Ksp Values Metal Cl- OH- SO42- CrO42- C2O42- Ag+ 1.8 x 10-10 Pb2+ 1.7 x 10-5 1.4x10-20 1.3x10-8 2.3x10-13 Hg22+ 1.4 x 10-18 Ba2+ Ca2+ Mg2+ Na+ K+ NH4+…
sovle this ASAP 10mins calculate the moles of HCl you may look at ref page if need
[Referencess) Calculate the sodium ion concentration when 60.0 mL of 2.0 M sodium carbonate is added to 40.0 mL of 1.3 M sodium bicarbonate. Assume that the volumes are additive. Concentration M Suhmit Answer Visited Try Another Version 6 item attempts remaining
A reagent of known concentration that is often placed inside a buret titrant Chemicals are sold and classified based on their % purity. Arrange the following classifications according to increasing % purity. 1. Chemically pure (CP) II. Primary standard III. Reagent-grade a. l< ll
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Needing help with #1-3
Use the References to access important values if needed for this question. The Solubility Product Constant for magnesium hydroxide is 1.5 × 10-¹¹. The molar solubility of magnesium hydroxide in a water solution is M. Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next
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Acetic acid is added to DI water at an initial concentration of 10 -6 M (Ka=1.8x10-5) A. Using the "ICE" Method, what would the pH be at equilibrium? State assumptions and show your work. B. Using the simultaneous equations method, what would the pH be at equilibrium? Show your work