(10pts) Post-Lab QuestionsUse this reaction to answer both post-lab questions.One of the reactions that is often studied in an equilibrium experiment is:NH3 (aq) + H2O (1)NH4 (aq) + OH(aq). Use this reaction to answer post-lab questions 1-3.(5pts)1. Which way would the equilibrium shift if NH4Cl was added to the solution? Briefly explain.Normal : BIUX2 X2=fx 8e=(5pts)2. What would happen to the concentration of NH4 if you added OH- to the reaction? Briefly explain.NormalBIU==fx 8TxTx

Step 1:Le Chatelier's principleLe Chatelier's principle states that if a dynamic equilibrium is…

Answered: (10pts) Post-Lab Questions Use this…

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

Writing the concentration equilibrium expression for a.. Write the concentration equilibrium constant expression for this reaction. CH3CO,H(aq)+C,H,OH(aq)→CH;CO,C,H,(aq)+H,0(1)
req 2req 2req s 2req ats 2req Use the References to access important values if needed for this question. The Solubility Product Constant for calcium carbonate is 3.8 x 10-⁹. The molar solubility of calcium carbonate in a 0.298 M ammonium carbonate solution is Submit Answer Retry Entire Group 9 more group attempts remaining Cengage Learning Cengage Technical Support M. Previous Email Instructor Next Save and Exit
How did the change of stress (adding or removing reactants or products) cause a shift in the equilibrium system of the solutions (in which direction) use an example. Use trial one as an example
Based on your ICE table and the equilibrium expression for Ka, set up the expression for Ka in order to determine the unknown concentrations. Each reaction participant must be represented by one tile. Do not combine terms. Ka = = 1.5 × 10-5 RESET [0] [0.100] [0.120] [0.140] [0.0200] [0.0400] [x] [2x] [0.100 + x] [0.100-x] [0.120+x] [0.120-x] [0.140 + x] [0.140-x] [0.0200 + x] [0.0200 - x] [0.0400+x] [0.0400 - x] < PREV 2 3 Based on your ICE table and the equilibrium expression for Ka, determine the pH of this solution. pH = RESET 0 4.35 4.49 x 10-5 9.65 3.99 10.0 2.23 x 10-10 1.40 3.23
Please answer both b and c part otherwise I'll downvote
8 Chem101 14.4 Hydrolysis of Salt X Microsoft PowerPoint X |M Inbox (569) - mirandae X M Lab 3/1-elaine.mirand X Sy -log (10)(2.54*10^(-3)) x Question 25 of 66 Consider the equilibrium system described by the chemical reaction below. At equilibrium, a 200 mL reaction vessel contained a mixture of 0.55 atm NO,, 6.5 x 10-5 atm NO, and 4.5 x 10-5 atm O, at 103.0 °C. What are the values of Kp and Kc for the reaction at this temperature? 2 NO:(g) = 2 N0(g) + O2(g) 2 NEXT Based on the given data, set up the expression for Kp. Each reaction participant must be represented by one tile. Do not combine terms. Once the expression is constructed, solve for Kc. %3D 5 RESET (0.55) (6.5 x 10-5) (4.5 x 10-) (2.75) (3.3 x 10-4) (2.3 x 10-4) (2.75 x 10-9) (3.25 x 10-7) (2.25 x 10-7) 2(0.55) 2(6.5 x 10-5) 2(4.5 x 10-5) (0.55)? (6.5 x 10-5)2 5.3 x 10-9 gp א a-0E) 1.9 x 108 1.6 x 1012 6.3 x 10-13 * 23 2$ 7. 6 5. 9. 3. in
Can you help me calculate the equilibrium constant using this data? (2 data sets) equilibrium reaction: Co(H2O)62+ (aq) + 4 Cl- (aq) ⇄ CoCl42- (aq) + 6 H2O (l)
Assume we are to tackle a complex aqueous equilibria problem using the systematic process we learned in class. In our example, we’re going to look at dissolving silver chromate (Ag2CrO4, Ksp = 1.2 x 10–12) in water. Write 4 relevant equilibrium reactions. Answer: Dissolving silver chromate (Ag2CrO4, Ksp = 1.2 x 10–12) in water, The 4 relevant equilibrium reactions are given by, Ag2CrO4⇌2Ag++CrO−24CrO−24+H2O⇌HCrO−4+OH−HCrO−4+H2O⇌H2CrO4+OH−2Ag++2OH−⇌2AgOHH2O⇌H++OH− This is the part I need help with: Assume we are to tackle a complex aqueous equilibria problem using the systematic process we learned in class. In our example, we’re going to look at dissolving silver chromate (Ag2CrO4, Ksp = 1.2 x 10–12) in water. Write 1 charge balance equation (based on your answer from the previous question).
I need accurate answers with full details. This is my chance to submit it so, please solve carefully.
Give correct answer please..don't use Ai for answering this
Determine the Ka for a weak acid by constructing an ICE table and using this information to construct and solve the equilibrium constant expression. Complete Parts 1-2 before submitting your answer. 1 2 NEXT > A 0.1000 M solution of a weak acid, HA, is 3.0% dissociated. Fill in the ICE table with the appropriate value for each involved species to determine the unknown concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) HA(aq) H₂O(1) H3O+(aq) A¯(aq) RESET 0 0.1000 3.0 -3.0 0.030 -0.030 0.0030 -0.0030 0.0970 -0.0970 0.0097 -0.0097 30 APR 3 n MacBook Air

Recommended textbooks for you

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

Chemistry

ISBN:

9781259911156

Author:

Raymond Chang Dr., Jason Overby Professor

Publisher:

McGraw-Hill Education

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Organic Chemistry

Chemistry

ISBN:

9780078021558

Author:

Janice Gorzynski Smith Dr.

Publisher:

McGraw-Hill Education

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Elementary Principles of Chemical Processes, Bind…

Chemistry

ISBN:

9781118431221

Author:

Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard

Publisher:

WILEY

SEE MORE TEXTBOOKS