Four beakers have water at 20 °C. A piece of metal is dropped into the water in each beaker. The table below shows the initial t
2 answers:
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The question is incomplete, here is the complete question:
A chemist titrates 110.0 mL of a 0.2412 M hypochlorous acid (HCIO) solution with 0.0613 M NaOH solution at 25°C. Calculate the pH at equivalence. The pKa of hypochlorous acid is 7.50. Round your answer to 2 decimal places
<u>Answer:</u> The pH of the solution is 10.09
<u>Explanation:</u>
To calculate the volume of base, we use the equation given by neutralization reaction:
where,
are the n-factor, molarity and volume of acid which is
are the n-factor, molarity and volume of base which is NaOH.
We are given:
Putting values in above equation, we get:
At equivalence, the number of moles of acid is equal to the number of moles of base. Also, the moles of salt which is NaClO will also be the same.
To calculate the number of moles for given molarity, we use the equation:
.....(1)
- <u>For HClO:</u>
Molarity of HClO solution = 0.2412 M
Volume of solution = 110.0 mL
Putting values in equation 1, we get:
- <u>For NaClO:</u>
Moles of NaClO = 0.026532 moles
Volume of solution = [432.8 + 110] mL = 542.8 mL
Putting values in above equation, we get:
To calculate the pH of the solution, we use the equation:
where,
= negative logarithm of weak acid which is hypochlorous acid = 7.50
C = concentration of the salt = 0.0489 M
Putting values in above equation, we get:
Hence, the pH of the solution is 10.09
Answer:
<h2>pH = 3.9</h2><h2>pOH = 10.1</h2>Explanation:
Since is a weak acid to find the pH of
we use the formula
where
Ka is the acid dissociation constant
c is the concentration
From the question
Ka of = 1.75 × 10^-5
c = 1.00 × 10-³M
Substitute the values into the above formula and solve for the pH
That's
We have the answer as
<h3>pH = 3.9</h3>To find the pOH we use the formula
pH + pOH = 14
pOH = 14 - pH
pOH = 14 - 3.9
We have the answer as
<h3>pOH = 10.1</h3>Hope this helps you
Answer:
1.51448 atms
Explanation:
