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[DOC File]EQUILIBRIUM - SISD
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NH3(aq) + H2O(l) ( NH4+(aq) + OH-(aq) In aqueous solution, ammonia reacts as represented above. In 0.0180 M NH3(aq) at 25°C, the hydroxide ion concentration, [OH-] , is 5.60 × 10-4 M. In answering the following, assume that temperature is constant at 25°C and that volumes are additive. a. Write the equilibrium-constant expression for the ...

[DOC File]EXAM 2 PRACTICE MULTIPLE CHOICE QUESTIONS – ANSWER …
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(aq) NH3(aq) + H2O(l) b. NH4+ (aq) + H2O(l) NH3(aq) + H3O+(aq) c. NH4+ (aq) + H2O(l) NH52+(aq) + OH – (aq) d. NH4+ (aq) NH2+(aq) + H2(g) 13. Which of the following is true? a. HF is a stronger acid than HI, because F is more electronegative than I. b. HF is a stronger acid than HI, because the HF bond is weaker than the HI bond.

[DOC File]Chapter 16 Worksheet 1
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NH3 (aq) + H2O (l) = NH4+ (aq) + OH- (aq) Keq = Kb for NH3 = 1.8 x 10--5. The products are the stronger acid and base so Keq is very small! a. The equilibrium constant for which of the above reactions is an example of either a Ka (acid . ionization constant) or a Kb (base ionization constant)?

[DOC File]Chapter 17 Study Questions and Problems
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NH3(aq) + H2O(l) NH4+(aq) + OH (aq) A B CA CB HCN(aq) + H2O(l) H3O+(aq) + CN (aq) A B CB CA. c. NH4+(aq) + CO32 (aq) NH3(aq) + HCO3 (aq) 2. Write the name and formula for the conjugate bases of the following: a. HNO2 NO2- nitrite. b. H2SO4 HSO4- bisulfate. c. H2PO4 ...

[DOC File]CHEMICAL EQUILIBRIA--ACID/BASE
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NH3(aq) + H2O(l) ( NH4+(aq) + OH¯(aq) Initial 0.10 M 0 0. Change. Equilibrium. We are assuming that before equilibrium is established, no NH4+ or OH- has formed. To establish equilibrium, a shift to the right has to occur. Since the amount of NH3 lost, and the amounts of NH4+ and OH- formed are not known, we assign the value of -x and +x ...

[DOC File]5 - Weebly
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NH3(aq) + H2O(l) ( NH4+(aq) + OH(aq) Kb (NH3) = 1.8 ( 10–5. The equilibrium concentration of an ammonia (NH3) solution is 0.500 M. The pOH of the solution is. A. 11.5. B. 8.95. C. 2.52. D. 2.00 25. Which one of the following equations contains a conjugate acid-base pair from which a …

[DOC File]CHAPTER 15 - APPLICATIONS OF AQUEOUS EQUILIBRIA
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NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) The effect is called the common ion effect and illustrates how an equilibrium does not discriminate between species of different origins. This suggests how to handle the calculations: Equilibrium Calculations. Example: (15.1)

[DOC File]Equilibrium Practice Problems - LCPS
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NH3 (aq) + H2O ( NH4+ (aq) + OH- (aq) K = 1.8 x 10-5. Calculate [NH3], [NH4+] and [OH-] in a solution originally 0.200 M NH3. NH3 (aq) + H2O ( NH4+ (aq) + OH- (aq . Initial 0.200 M 0 0. Change -x +x +x. After 0.2 – x x x Plug into equilibrium expression and solve for x. ...

[DOC File]CHM152 Group Work 3 Name ...
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HPO42- + H2O(l) H3O+(aq) + PO43-(aq) 13. Write and balance the reaction for ammonia in water. NH3(aq) + H2O(l) NH4+(aq) + OH-(aq) 14. What is the strongest base among the following? a. ClO-b. ClO2-c. ClO3-d. ClO4-15. From the following chemical reaction, determine the relative Bronsted-Lowry acid strengths (from strongest to weakest)

[DOC File]Ch 16 Acid - Base Equilibria
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NH3(aq) + H2O(l) ( NH4+(aq) + OH-(aq) add the above two equilibria, net is: two equilibria are consecutive reactions leading to the overall above, equ’m constant for equlibria thus added is

Nh3 aq h2o l nh4 aq oh aq