Respuesta :
Answer;
pH =7.58
Explanation;
The KOH will react with the HClO to produce KClO. You will have a solution containing unreacted HClO and KOH. This is a buffer solution.
Equation:
HClO + KOH → KClO + H2O
HClO reacts with KOH in 1:1 molar ratio
Mol HClO in 50mL of 0.150M solution = 50/1000*0.150 = 0.0075 mol HClO
Mol KOH in 30mL of 0.150M solution = 30/1000*0.150 = 0.0045 mol KOH
These react to produce 0.0045 mol KClO and there is 0.0030 mol HClO unreacted
Volume of solution = 50mL + 30mL = 80mL = 0.080L
Molarity of HClO in solution = 0.0030/0.080 = 0.0375M
Molarity of KClO in solution = 0.0045/0.080 = 0.0562M
Using the Henderson-Hasselbalch equation we can calculate the pH;
pKa HClO = -log ( 4.0*10^-8) = 7.40
pH = pKa + log ([KClO]/[HClO])
pH = 7.40 + log( 0.0562/0.0375)
pH = 7.40 + log 1.50
pH = 7.40+ 0.18
pH = 7.58
PH = 7.58
Further Explanation
KOH will interact with HClO to provide KClO. you may have an answer that contains unreacted HClO and KOH. this is often a solution.
Equation:
HClO + KOH → KClO + H2O
HClO reacts with KOH in a very 1: 1 molar ratio
Mole of acid in 50 ml of an answer of 0.150 m = 50/1000 * 0,150 = 0.0075 mole of acid
Mole of KOH in 30 ml of 150 M solution = 30/1000 * 0,150 = 0.0045 mole of KOH
This reacts to provide 0.0045 moles of KClO and there are 0.0030 moles of HClO unreacted
The volume of the answer = 50 ml + 30 ml = 80 ml = 0.080 l
Deposition of acid in solution = 0.0030 / 0.080 = 0.0375M
KClO deposit in solution = 0.0045 / 0.080 = 0.0562 m
Using the Henderson-Hasselbalch equation, we will calculate pH;
pKa HClO = -log (4.0 * 10 ^ -8) = 7.40
PH = pKa + log ([KClO] / [HClO])
PH = 7.40 + notes (0.0562 / 0.0375)
PH = 7.40 + 1.50 notes
PH = 7.40+ 0.18
PH = 7.58
Learn More
Mole of Acid https://brainly.com/question/9465562
HClO https://brainly.com/question/12355703
Details
Grade: College
Subject: Chemistry
Keyword: mole, acid, HClO
