**Determining OH⁻ Concentration in a BrO⁻ Solution***Objective*: Determine the concentration of OH⁻ in a 0.724 M solution of BrO⁻. The base dissociation constant (Kb) is given as 4.0 × 10⁻⁶.*Instructions*:Based on your ICE (Initial, Change, Equilibrium) table and the definition of Kb, set up the expression for Kb to determine the unknown. Do not combine or simplify terms.*Equation Setup*:\[ K_b = \boxed{\text{numerator expression}} \]\[ = \boxed{\text{denominator expression}} \]\[ = 4.0 \times 10^{-6} \]Choose the correct terms from the options below to set up the Kb expression accurately.*Options to Choose*:- [0]- [0.724]- [4.0 × 10⁻⁶]- [0.362]- [x]- [2x]- [2x]²- [0.724 + x]- [0.724 - x]- [0.724 + 2x]- [0.724 - 2x]- [4.0 × 10⁻⁶ + x]- [4.0 × 10⁻⁶ - x]- [4.0 × 10⁻⁶ + 2x]- [4.0 × 10⁻⁶ - 2x]*Note*:Make sure to correctly identify the expressions related to initial concentrations, changes in concentrations, and equilibrium concentrations as outlined in the ICE table approach. Press the "RESET" button to start over if needed. **Title: Determining the Concentration of OH⁻ in a BrO⁻ Solution**---**Objective:**Determine the concentration of OH⁻ in a 0.724 M solution of BrO⁻, given that the base dissociation constant (Kb) is 4.0 × 10⁻⁶.**Instruction:**Based on the given values, set up an ICE table to determine the unknown concentration at equilibrium.---**ICE Table Setup:**The reaction is:\[ \text{BrO}^- (aq) + \text{H}_2\text{O} (l) \rightleftharpoons \text{OH}^- (aq) + \text{HBrO} (aq) \]| | BrO⁻ (aq) | + | H₂O (l) | ⇌ | OH⁻ (aq) | + | HBrO (aq) ||----------------|-----------|---|---------|---|-----------|---|------------|| **Initial (M)** | | | | | | | || **Change (M)** | | | | | | | || **Equilibrium (M)** | | | | | | | |**Available Values:**- Initial BrO⁻ concentration: 0.724 M- Possible changes and equilibrium expressions include: - **Change (M):** -x, +x, +2x, -2x - **Equilibrium (M):** 0.724 - x, 0.724 + x, 4.0 × 10⁻⁶ - 2x, and so on.**Note:**Click on the values to input them into the ICE table. Use these expressions to solve for the equilibrium concentrations.**Reset Option:**If needed, click the "RESET" button to clear the values and start again.---This exercise helps you understand the process of setting up and solving an ICE table for equilibrium concentration calculations in chemical solutions.

Answered: Image /qna-images/answer/bc395894-9f44-4818-9d90-9130b05fecdd.jpg

Determine concentration of OH" in a 0.724 M solution of BrO" (Kb = 4.0 x 10-6). 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. BrO (aq) H20(1) ОН (ад) HBRO(aq) + + Initial (M) Change (M) Equilibrium (M) 2 RESET 0.724 4.0 x 10-6 0.362 +x +2x -x -2x 0.724 + x 0.724 - x 0.724 + 2x 0.724 - 2x 4.0 x 10-6 4.0 x 10-6 4.0 x 10-6 + 2x 4.0 x 10-6 - 2x

Determine concentration of OH" in a 0.724 M solution of BrO" (Kb = 4.0 x 10-6). 2 3 NEXT > Based on the given values, set up ICE table in order to determine the unknown. BrO (aq) H20(1) ОН (ад) HBRO(aq) + + Initial (M) Change (M) Equilibrium (M) 2 RESET 0.724 4.0 x 10-6 0.362 +x +2x -x -2x 0.724 + x 0.724 - x 0.724 + 2x 0.724 - 2x 4.0 x 10-6 4.0 x 10-6 4.0 x 10-6 + 2x 4.0 x 10-6 - 2x

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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