Respuesta :
KBrO is produced by reaction of a strong base (KOH) with a weak acid (HBrO).
KOH + HBrO ==> KBrO + H2O
This salt, when diisoved in H2O, produce an alkaline solution (produced from a STRONG base). Since OH- is produced, this is a Kb problem.
Molarity . . . . . . . . .BrO- + H2O <==> HBrO + OH-
Initial.....................0.800 0 0 0
Final.......................0.800-x x x x
Kb BrO- = Kw / Ka HBrO = (1 x 10^-14) / (2.0 x 10^-9) = 5.0 x 10^-6
Kb = [HBrO][OH-] / [BrO-] = (x)(x) / (0.800 - x) = 5.0 x 10^-6
Since Kb is small compared to 0.800, we can neglect the -x term to simplify the calculation.
x^2 / 0.800 = 5.0 x 10^-6
x^2 = 4.0 x 10^-6
x = 2 x 10^-3 = [OH-]
pOH = -log[OH-] = -log (2.0 x 10^-3) = 2.69
pH + pOH = 14.00
pH = 14.00 - pOH = 14.00 - 2.69 = 11.3
The pH value is the negative log of H⁺ ions. The pH value of the KBrO solution is 11.3.
What is pH value?
The pH value is used to calculate the strongness of acid and base. The value of pH is from 0 to 14.
Let the following equations will be
KOH + HBrO → KBrO + H₂O
This salt, when dissolved in H₂O, produces an alkaline solution.
Since OH⁻ is produced, this is a Kb problem.
BrO⁻ + H₂O → HBrO + OH⁻
Kb = [HBrO][OH⁻]/[BrO⁻] = (x)(x)/(0.800 -x) = 5.0 × 10⁻⁶
Since Kb is small compared to 0.800, we can neglect the x-term to simplify the calculation.
x² / 0.800 = 5 × 10⁻⁶
x = 2 × 10⁻³
Then the pH value will be
pOH = -log[OH⁻] = -log (2.0 × 10⁻³) = 2.69
pH + pOH = 14
pH = 14 - pOH
pH = 14 - 2.69
pH = 11.3
More about the pH value link is given below.
https://brainly.com/question/1503669
