2) The ionization constant for NH3 in water is 1.8 x 10 - 5. Determine the hydroxide ion concentration and the pH of a 0.075 M solution of ammonia. 3) What is the pH of a buffer solution made by adding 0.15 mole of lactic acid HC;H;O, and 0.12 mole sodium lactate to enough water to make 1.0 L of solution? What is the concentration of the hydroxide ion in the solution? K, lactic acid = 1.4 x 10 -4

2) The ionization constant for NH3 in water is 1.8 x 10 - 5. Determine the hydroxide ion concentration and the pH of a 0.075 M solution of ammonia. 3) What is the pH of a buffer solution made by adding 0.15 mole of lactic acid HC;H;O, and 0.12 mole sodium lactate to enough water to make 1.0 L of solution? What is the concentration of the hydroxide ion in the solution? K, lactic acid = 1.4 x 10 -4

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...

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Please help us with number five in picture. We are getting 1.5 and I'm not sure if they are asking and telling us that .5 is the equilibrium pressure of dinitrogen pentoxide. Or if .5 is the total.This is not a graded question as it is a practice question . I am 60 years old and helping my son prepare for the AP exam in a few months. We do questions at the back of the textbook by Zumdahl and Zumdahl. I believe the answer is D but I am getting 1.5
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Consider The Following Reaction M Inbox (208) - eleganceextreme1 X + 05657571&snapshotld=13245488id-563649000&takeld-4bfba59b09f0e5b& X X QSearch this course X References Use the References to access important values if d for this question. *** The equilibrium constant, K,, for the following reaction is 8.46x10 at 298 K: 1 00 NH3(g) + H2Se(g) NH4HSe(s) A-Z Calculate the partial pressure of each gas and the total pressure at equilibrium when 0.469 moles of NHHSe(s) is introduced into a 1.00 L vessel at 298 K. Assume that the volume occupied by the solid is negligible. PNH3 atm atm PH2SE atm Ptotal 6. Equilibrium Calculations with Partial Pressur... : This is group attempt 1 of 5 Next Autosaved at 1:06 PM Back 1:06 PM xa 11 9/24/2019 1 hp delete rt co
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AutoSave 20200930175438D1747_Assigment 5 Equilibrium Compatibility Mode - Word P Search Gleyren Zefanya O X ff ?ם) File Home Insert Design Layout References Mailings Review View Help Acrobat A Share P Comments Find - Calibri (Body) v11 - A A Aa v A AaBЬСcDd AaBbСcDd AaBbC AаВЬСс. АаВ LG Paste E Replace BIU v ab x, x A vev A I Normal 1 No Spac. Heading 1 Heading 2 Title Create and Share Request Dictate Sensitivity Editor A Select v Adobe PDF Signatures Clipboard N Font Paragraph Styles Editing Adobe Acrobat Voice Sensitivity Editor 3. 5.. 6.|7. 8. 1 10. 1 11. 1 12. 1 13. 1 14. 15. I 16. 1 17. | 18. 1 1. Write equilibrium expressions for each of the following equilibria: (a) 2 C(s) + O;(g)22 CO(g) (b) Zn²*(aq) + H,S(g)2ZnS(s) + 2 H*(aq) (c) HCl(g) + H,O(e)2H;O*(aq) + Cl^(aq) (d) H;(g) + O,(g)2H,O(g) 2. The equilibrium constant for the reaction, 3 H;(g) + N2(g) 22 NH;(g), at a given temperature is 1.4 x 10-7. Calcu- late the equilibrium concentration of ammonia, if [H2] = 1.2 × 10-2 molL-…
Use data in Table 2.1, calculate the equilibrium constant, Ke for reactions a. 2S02 (g) + O2 (g) = 2S03 (g) b. 2S0s (g) 2SO2 (g) + O2 (g) 7. Initial concentrations, M Equilibrium concentrations, M (SO.] (02] (SO) (SO2] (SO) Experiment (a) 0.800 0.400 0.688 0.316 0.112 Experiment (b) 0.80 0.590 0.441 0.113 Table 2.1: An experimental results of initial and equilibrium concentrations for reaction of SO2 with Oz and the dissociation of SO3.
[Rev Topics] [References] Use the References to access important values if needed for this question. Consider the following reaction where Ke = 6.30 at 723 K. 2NH3 (9) N₂(g) + 3H₂(g) A reaction mixture was found to contain 0.000687 moles of NH3(g), 0.0258 moles of N₂ (g), and 0.0435 moles of H₂(g), in a 1.00 liter container. Calculate Qc. Qc = 1 Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium? The reaction must run in the forward direction to reach equilibrium. The reaction must run in the reverse direction to reach equilibrium. The reaction is at equilibrium. Submit Answer Retry Entire Group 9 more group attempts remaining Previous Next> ad Exit ? or n er