The pH of the solution is the negative logarithm of a proton or the hydrogen ion concentration. The pH of 0.39 M acetic acid solution (CH₃COONa) is 2.58.
<h3>What is pH?</h3>
The pH has been said to be the hydrogen ion concentration that can also be given by the pOH.
Given,
The acid dissociation constant Ka = 1.8 × 10⁻⁵
Concentration of acetic acid (C) = 0.39 M
The hydrogen ion concentration from Ka and molar concentration are calculated as:
H⁺ = √ Ka × C
= √1.8 × 10⁻⁵ × 0.39
= √0.00000702
= 0.0026
Now, pH from hydrogen ion is calculated as,
pH = - log [H⁺]
= - log [0.0026]
= 2.58
Therefore, the pH of acetic acid is 2.58.
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335K would be expressed as 61.85 degrees Celsius
Answer :
(A) 
: It is soluble in water.
(B) 
: It is insoluble in water.
Explanation :
Solubility : It is defined as the amount of solute dissolved in a solvent at a given temperature.
According to the solubility rules:
All chlorides are soluble except 
All sulfates are soluble except 
From this we conclude that,
(A) : It is soluble in water.
(B) : It is insoluble in water.
