Determine the number of grams of NH Br needed to prepare an aqueous solution at a specific pH by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the initial grams of NH Br required. The Kb of NH3 is 1.8 × 10-5. Complete Parts 1-3 before submitting your answer. 2 3 NEXT > An unknown quantity of NH4Br is dissolved in 1.00 L of water to produce a solution with a pH = 5.16. Let x represent the original concentration of NH4+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) NH.(aq) H₂O(1) HO+(aq) + NH(aq)

Determine the number of grams of NH Br needed to prepare an aqueous solution at a specific pH by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the initial grams of NH Br required. The Kb of NH3 is 1.8 × 10-5. Complete Parts 1-3 before submitting your answer. 2 3 NEXT > An unknown quantity of NH4Br is dissolved in 1.00 L of water to produce a solution with a pH = 5.16. Let x represent the original concentration of NH4+ in the water. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. Initial (M) Change (M) Equilibrium (M) NH.(aq) H₂O(1) HO+(aq) + NH(aq)

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 65AP: . The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in...

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. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
What mass of NaOH(s) must be added to 1.0 L of 0.050 M NH3 to ensure that the percent ionization of NH3 is no greater than 0.0010%? Assume no volume change on addition of NaOH.
For conjugate acidbase pairs, how are Ka and Kb related? Consider the reaction of acetic acid in water CH3CO2H(aq)+H2O(l)CH3CO2(aq)+H3O+(aq) where Ka = 1.8 105 a. Which two bases are competing for the proton? b. Which is the stronger base? c. In light of your answer to part b. why do we classify the acetate ion (CH3CO2) as a weak base? Use an appropriate reaction to justify your answer. In general, as base strength increases, conjugate acid strength decreases. Explain why the conjugate acid of the weak base NH3 is a weak acid. To summarize, the conjugate base of a weak acid is a weak base and the conjugate acid of a weak base is a weak acid (weak gives you weak). Assuming Ka for a monoprotic strong acid is 1 106, calculate Kb for the conjugate base of this strong acid. Why do conjugate bases of strong acids have no basic properties in water? List the conjugate bases of the six common strong acids. To tie it all together, some instructors have students think of Li+, K+, Rb+, Cs+, Ca2+, Sr2+, and Ba2+ as the conjugate acids of the strong bases LiOH, KOH. RbOH, CsOH, Ca(OH)2, Sr(OH)2, and Ba(OH)2. Although not technically correct, the conjugate acid strength of these cations is similar to the conjugate base strength of the strong acids. That is, these cations have no acidic properties in water; similarly, the conjugate bases of strong acids have no basic properties (strong gives you worthless). Fill in the blanks with the correct response. The conjugate base of a weak acid is a_____base. The conjugate acid of a weak base is a_____acid. The conjugate base of a strong acid is a_____base. The conjugate acid of a strong base is a_____ acid. (Hint: Weak gives you weak and strong gives you worthless.)
The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.
Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your answer. NEXT > 0.040 mol of solid NaOH is added to a 200.0 mL buffer containing 0.100 mol C6H5NH3Cl and 0.500 M C6H5NH₂. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. Before (mol) Change (mol) After (mol) 0.060 Initial (M) Change (M) Equilibrium (M) 0 -X 0.700 - x 1 -0.060 C6H5NH3*(aq) + OH (aq) 0 1 0.040 0.140 0.500 + x CoHşNHz(aq) + 0.300 + x 2 0.500 0.500 - x -0.040 0.300 - x -0.140 Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-4 before submitting your…
* 6:55 PM Thu Apr 6 -2.0 x 10 Before (mol Change (mo After (mol) Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Ka for HC₂H3O₂ is 1.8 x 10-5. Complete Parts 1-4 before submitting your answer. 3 4 NEXT> Two solutions are mixed: 20.0 mL of 0.20 M HC₂H3O2 and 20.0 mL of 0.10 M NaOH. Fill in the table with the appropriate value for each involved species to determine the moles of reactant and product after the reaction of the acid and base. You can ignore the amount of water in the reaction. 0 1 20.0 Q Question 10 of 11 HC₂H₂O₂(aq) + OH-(aq) →> H₂O(l) Tap here or pull up for additional resources 3.0 x 10-³ -3.0 x 10-¹ 4.0 x 10-³ @ 2 2 ... W 0.20 # 3 0.10 -4.0 x 10-¹ F 4 1.0 x 10-¹ R + C,H,Oz(aq) -1.0 x 10-¹ 5 T RESET 2.0 x 10-³ 6 Submit V & 7 8 E C A L 9
In determining the pH of 0.010 M solution of weak acid, HCNO, which equations are relevant in the systematic treatment of equilibrium. (K, = 3.47 x 10-4) %3D a) [H3O*][OH-] = 1.00 × 10-14 b) 3.47 x 10-4 = [H*][CNO¯]/[HCNO] c) 2.88 x -11 = [HCNO][OH ]/[CNO¯] d) [H3O*] = [OH-] + [CNO"] e) [OH]+ [CNO¯] = 2[H3O*] %D f) 0.010 = [HCNO] + [CNO¯] g) [CNO] + [OH]) = [HCNO] a b C e f
[Review Topics] [References] Use the References to access important values if needed for this question. Consider the following equilibrium between 3-methylbenzoic acid (K,a-5.0x10) and its conjugate base: %3D CH3- CH3- H2O + H30* (1) Will lowering the pH shift the equilibrium to the right or to the left? (2) Calculate the ratio of the concentration of 3-methylbenzoate ion to the concentration of 3-methylbenzoic acid at a pH of 1.59. ratio [conjugate base] / [acid] Submit Answer Retry Entire Group 9 more group attempts remaining
Consider equimolar solutions of each of the following compounds; rank them in order of increasing pH. Mw CH₂ IV CF₂ A) III
Ascorbic acid (H, C,H,0,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal = 8.00 x 10-5 and K„2 = 1.60 x 10-12. Determine the pH of a 0.134 M solution of ascorbic acid. 2.49 pH = Determine the equilibrium concentrations of all species in the solution. [H,C,H,O,] = 0.131 M [HC,H,0G] = 3.22 x10-3 M 7.18 x10 -8 [C,H,O; = M Incorrect
+ Determine the pH of a solution by constructing a BCA table, constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. The value of Ka for HC₂H₂O₂ is 1.8 × 105. Complete Parts 1-4 before submitting your answer. 3 2 Initial (M) Change (M) Equilibrium (M) PREV Based on the result of the acid-base reaction (Part 1), set up the ICE table in order to determine the unknown concentrations of all reactants and products. HC,H,O,(aq) + 0.050 0.025 + x 0 0.025 0.025 - x 1 0.20 Question 12 of 15 +x 2 0.10 -X H₂O(1) 3 1.0 × 10-³ 0.10 + x H,O*(aq) 2.0 × 10-³ 0.10 - x 4 + 3.0 × 10.³ 0.050 + x NEXT C,H,O,(aq) > RESET 4.0 × 10-³ 0.050 - x Submit
The value of K, for benzoic acid , C¿H¿CcOOH , is 6.30x10-5. Write the equation for the reaction that goes with this equilibrium constant. (Use H;0* instead of H*) + +