Question

Calculate the molar concentration of oh− ions in a 0.555 m solution of hypobromite ion (bro−; kb=4.0×10−6).

Answer 1

according to the reaction equation:

and by using ICE table:

              BrO-  + H2O → HBrO + OH-
initial   0.555m                   0           0

change  -X                         +X         +X

Equ      (0.555-X)                  X           X

when Kb = [HBrO][OH-] / [BrO-]

by substitution:

4 x 10^-6 = X^2 / (0.555-X)   by solving for X 

∴ X = 0.00149 

∴[OH-] = X = 0.00149 m

Answer 2

The molar concentration of OH⁻ ions in a 0.555 M solution of hypobromite ion is 1.5 × 10⁻³ M.

What is a Bronsted-Lowry base?

A Bronsted-Lowry base is a species that accepts H⁺.

Let's consider the basic reaction for hypobromite ion.

BrO⁻ + H₂O ⇄ HBrO + OH⁻

Since BrO⁻ is a weak base, we can calculate the concentration of OH⁻ using the following expression.

[OH⁻] = √(Kb × Cb)

[OH⁻] = √(4.0 × 10⁻⁶ × 0.555) = 1.5 × 10⁻³ M

where,

• Kb is the basic ionization constant.
• Cb is the concentration of hypobromite ion.

The molar concentration of OH⁻ ions in a 0.555 M solution of hypobromite ion is 1.5 × 10⁻³ M.

Learn more about Bronsted-Lowry bases here: https://brainly.com/question/25829979