<span>pH scale is used to determine how acidic, basic or neutral a solution is.
pH can be calculated using the Hydrogen ion concentration.
pH is calculated using the following formula
pH = -log [H</span>⁺<span>]
[H</span>⁺<span>] can be calculated knowing the pH
[H</span>⁺<span>] = antilog(-pH)
[H</span>⁺<span>] = 1.32 x 10</span>⁻¹⁰<span> M</span>
Answer:
5.0
Explanation:
We have a buffer system formed by a weak base (C₅H₅N) and its conjugate acid (C₅H₆N⁺). We can calculate the pOH using the Henderson-Hasselbach's equation.
pOH = pKb + log [acid]/[base]
pOH = -log 1.8 × 10⁻⁹ + log 0.02/0.01
pOH = 9.0
Then, we will calculate the pH.
pH + pOH = 14
pH = 14 - pOH = 14 - 9.0 = 5.0
Answer:
There must be two Chlorine atoms for every one Calcium atom in order to fulfill Chlorine's octet rule and pair Calcium's unpaired electrons.
Explanation:
Calcium has two unpaired electrons in its Lewis dot structure, while Chlorine has one unpaired electron.
<em>So why can't we just make a double bond for </em><em>one</em><em> Chlorine?</em>
Chlorine has seven valence electrons, so once it shares electrons with Calcium, the octet rule is accomplished, and no more pairs can be made.
Answer:
a) located in the outermost energy level.
Explanation:
A valence electron is an electron in the outer shell associated with an atom, and that can participate in the formation of a chemical bond if the outer shell is not closed; in a single covalent bond, both atoms in the bond contribute one valence electron in order to form a shared pair.
Hope this helped!
Answer:
20 ml 13% solution should the professor use
Explanation:
Let
the volume of the 13% solution should the professor use = a
So, according to question
13% x a + 18% x (50-a) = 50 x 16%
⇒ 0.13 a + 0.18 x 50 - 0.18 a = 50 x 0.16
⇒ - 0.05 a = 8 - 9
⇒
So, <u>20 milliliters of the 13% solution</u> should be the professor used.
& (50 - 20) = 30 ml of the 18 % solution would be use.