pH is referred to as the scale to describe the hydronium ion concentration of a
solution. It is used to measure the acidity or basicity of a solution. pH of an acidic solution is less than 7, a neutral solution is 7, and a basic solution is greater than 7.
pH can be calculated using the formula:
![pH = - log [H_{3}O^{+}]](https://tex.z-dn.net/?f=%20pH%20%3D%20-%20log%20%5BH_%7B3%7DO%5E%7B%2B%7D%5D%20%20%20)
Given the pH of solution is 3.2.
Finding out the concentration of hydronium ion from pH.
![pH = - log[H_{3}O^{+}]](https://tex.z-dn.net/?f=%20pH%20%3D%20-%20log%5BH_%7B3%7DO%5E%7B%2B%7D%5D)
![3.2 = - log [H_{3}O^{+}]](https://tex.z-dn.net/?f=%203.2%20%3D%20-%20log%20%5BH_%7B3%7DO%5E%7B%2B%7D%5D%20%20%20)
![[H_{3}O^{+}] = 10^{-3.2}](https://tex.z-dn.net/?f=%20%5BH_%7B3%7DO%5E%7B%2B%7D%5D%20%3D%2010%5E%7B-3.2%7D%20%20%20%20)
![[H_{3}O^{+}] = 6.3 * 10^{-4} M](https://tex.z-dn.net/?f=%20%5BH_%7B3%7DO%5E%7B%2B%7D%5D%20%3D%20%20%206.3%20%2A%2010%5E%7B-4%7D%20M%20%20)
Therefore, the hydronium ion concetration of the solution is 
[H+] = ?
pH = -log[H+]
[H+] = 10^-pH
[H+] = 10^-11,3
[H+] = 5,01 × 10^-12 mol/l
Answer: H+ concentration in this solution equal 5,01 × 10^-12 mol/l.
:-) ;-)
Answer:
A liquid has a definite volume but not a definite shape
Answer:
Option 5 → 7.01 g
Explanation:
Molarity . volume (L) = Moles
This can help us to determine the moles of KOH that are in the solution.
We convert the volume from mL to L → 250 mL . 1L / 1000mL = 0.250 L
0.5 mol /L . 0.250L = 0.125 moles of KOH
Now, we only have to convert the moles to mass, by the molar mass:
Moles . molar mass = mass → 0.125 mol . 56.1 g/mol = 7.01 g
Answer:
do you mean?
Explanation:
the structural formula of butyl pentyl ether
