Respuesta :
The pH of the solution is 13.
The amount of a substance in a specific volume of solution is known as its molarity (M). The number of moles of a solute per liter of a solution is known as molarity. The molar concentration of a solution is another name for molarity.
Finding the molecular weight of the 716.mg of KOH is the first step.
KOH's molar mass is 39 + 16 + 1 = 56 g/mol.
KOH mass concentration: 716 mg
If we convert mg to g, we have
716/1000 = 0.716g
Mole number = mass multiplied by MM
= 0.716/56 = 0.0128mol
Next, we determine how many moles of KOH are present in 1L of the solution.
In 130mL of solution (i.e., 0.13L), 0.0128mol of KOH dissolves.
As a result, 1L of the solution will contain Xmol of KOH that will dissolve.
KOH Xmol=(0.0128)/0.13 = 0.098mol/L
The [OH⁻] is the following.
KOH <==> KOH = 0.098 mol/L [K+ + OH⁻] [K⁺] = 0.098 mol/L [OH⁻] = 0.098 mol/L
The pOH pOH= -log [OH⁻] is then discovered.
= - log pOH 0.098 \s pOH = 1
Recall
pH + pOH = 14
pH = 14 — pOH
pH = 14 — 1 pH = 13
The solution has a pH of 13.
Learn more about the Molarity with the help of the given link:
https://brainly.com/question/12127540
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I understand that the question you are looking for is "A chemist dissolves 716.mg of pure potassium hydroxide in enough water to make up 130.mL cof solution. Calculate the pH of the solution".
