Determine the Kb for an unknown base by constructing an ICE table andusing this information to construct and solve the equilibrium constantexpression. Complete Parts 1-2 before submitting your answer.12NEXT >The pH for a 0.185 M solution of an unknown weak base, B, is 12.95. Fill in the ICE tablewith the appropriate value for each involved species to determine the unknownconcentrations of all reactants and products.Initial (M)Change (M)Equilibrium (M)B(aq)H₂O(1)=OH-(aq)+BH+(aq)RESET00.18512.95-12.951.11-1.111.12 × 10-13-1.12 × 10-130.096-0.0960.089-0.089 Determine the Kb for an unknown base by constructing an ICE table andusing this information to construct and solve the equilibrium constantexpression. Complete Parts 1-2 before submitting your answer.PREV12Based on your ICE table (Part 1) and the definition of Kb, set up the expression for Kb.Each reaction participant must be represented by one tile. Do not combine terms.Once the expression is constructed, solve for Kb.Kb==RESET[0][0.185][12.95][1.11][1.12 × 10-13][0.096][0.089]6.8 × 10-261 × 10-140.0836.1 x 10-131.3 x 10-2512

Answered: Image /qna-images/answer/b6b0c3e7-00cf-4e53-8d45-bb29324a40aa.jpg

Determine the Kb for an unknown base 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 > The pH for a 0.185 M solution of an unknown weak base, B, is 12.95. 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) B(aq) H₂O(1) = OH-(aq) + BH-(aq) RESET 0 0.185 12.95 -12.95 1.11 -1.11 1.12 x 10-13

Determine the Kb for an unknown base 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 > The pH for a 0.185 M solution of an unknown weak base, B, is 12.95. 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) B(aq) H₂O(1) = OH-(aq) + BH-(aq) RESET 0 0.185 12.95 -12.95 1.11 -1.11 1.12 x 10-13

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

The ionization of water is an example of a system at equilibrium. In the forward reaction, water ionizes to form a proton and a hydroxide ion. What takes place in the reverse reaction?
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. Is trial one as an example
A solution of 0.28 M concentration of ammonia, has been prepared, the Kb value for ammonia is 1.8 x 10–5.what are the initial, change, and equilibrium values?
Enter your answer in the provided box. Use the equilibrium constant expression, and equilibrium constant to det concentration of H₂S if: [H₂S]² [S₂][H₂]² Keq=1.1 x 107 [H₂] = 1.0 × 10-3 M [S₂] = 5.0 × 10 5 M [H₂S] = 0.55 X Keq = 2 H₂(g) + S₂(g) → 2 H₂S(g)
The ionization product of water, k_WkW, is usually approximated to be 1.0 x 10-14. The chemical equation for the ionization product of water is: 2H2O <==><==> H3O+ + OH- Thinking about the definition of equilibrium constants and then specifically k_WkW, explain why k_WkW is written without units
Write the equilibrium expression (specify K or K) for the hydrolysis reactions. Write the expression in the form; axb K =
EXPLAIN AND ANSWER CORRECTLY
If 0.54 molmol of Br2Br2 and 1.23 molmol of Cl2Cl2 are introduced into a 3.0-LL container at 400 KK, what will be the equilibrium concentration of Br2Br2? If 0.54 molmol of Br2Br2 and 1.23 molmol of Cl2Cl2 are introduced into a 3.0-LL container at 400 KK, what will be the equilibrium concentration of Cl2Cl2? If 0.54 molmol of Br2Br2 and 1.23 molmol of Cl2Cl2 are introduced into a 3.0-LL container at 400 KK, what will be the equilibrium concentration of BrClBrCl?
Consider the reaction of SO2 and O2 described by the chemical reaction below. Determine the equilibrium constant for this reaction by constructing an ICE table, writing the equilibrium constant expression, and solving it. Complete Parts 1-2 before submitting your answer. NEXT > A 2.00 L reaction vessel was filled 0.0432 mol SO2 and 0.0296 mol O2 at 900 K and allowed to react. At equilibrium, the concentration of SO3 was found to be 0.0175 M. 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) -0.00875 0.0209 0 0.00875 2 SO₂(g) + O₂(g) = 2 SO³(g) 2SO2(g) 2.00 0.0216 0.0432 0.0148 + 0.0296 0.0041 O₂(g) 2 0.0175 0.0129 -0.0175 0.0061 2SO3(g) RESET -0.0350 0.0257
Determine the Kb for cocaine (a base) 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 > The pH for 6.1 x 104 M solution of cocaine, a weak base, is 9.60. Let cocaine be represented by the generic base, B. 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) B(aq) + H₂O(1) 0 6.1 × 10-4 9.60 -4.0 x 10-5 2.1 × 10-4 -2.1 × 10-4 5.7 × 10-4 3 =4 OH(aq) + BH*(aq) RESET -9.60 2.5 x 10-10 -2.5 x 10-10 4.0 × 10-5 -5.7 × 10-4 Stv A
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
Write the equilibrium constant expression for the following reaction. Remember to use brackets, [ ], for concentrations and use exponents where needed, but do not show physical states in your answer. C(s) + H2O(g) ⇌ CO(g) + H2(g) Keq =