When a molecule is broken down into its constituent atoms, these atoms do not have the same properties as the molecule.
We can use an everyday molecule, such as water, H20, to show this property. Water is a liquid with unique properties that stem from its hydrogen bonding. On the other hand, its constituent atoms, hydrogen and oxygen, are not liquids, and have very different properties. Oxygen and hydrogen are both gases; hydrogen is dangerous and very flammable, while we breathe in oxygen throughout our lives. This example illustrates how the atoms that make up a molecule usually have different properties than the completed molecule.
Hope this helps!
Answer is: volume of H₂SO₄ is 42.1 mL.<span>
Chemical reaction: H</span>₂SO₄ + 2NaOH → Na₂SO₄ + 2H₂O.<span>
c(H</span>₂SO₄) = 0,4567 M = 0,4567 mol/L.<span>
V(NaOH) = 30 mL </span>÷ 1000 mL/L <span>= 0,03 L.
c(NaOH) = 0,321 M = 0,321 mol/L.
n(NaOH) = c(NaOH) · V(NaOH).
n(NaOH) = 0,321 mol/L · 0,030 L.
n(NaOH) = 0,00963 mol.
From chemical reaction: n(H</span>₂SO₄) : n(NaOH) = 1 : 2.<span>
n(H</span>₂SO₄) = 0,01926 mol.<span>
V(H</span>₂SO₄) = n(H₂SO₄) ÷ c(H₂SO₄).<span>
V(H</span>₂SO₄) = 0,01926 mol ÷ 0,4567 mol/L.<span>
V(H</span>₂SO₄<span>) = 0,0421 L = 42,1 mL.</span>
H. Hydrogen
He. Helium
Li. Lithium
Be. Beryllium
B. Boron
C. Carbon
N. Nitrogen
O. Oxygen
F. Fluorine
N. Neon
Answer : the hydrogen ion concentrations for pH = 7.35 and pH = 7.45 are 4.46 x 10⁻⁸ M and 3.54 x 10⁻⁸ M respectively.
When the pH of a solution is less than 7, the hydrogen ion concentration is higher and therefore the solution is acidic.
On the other hand, when the pH of a solution is greater than 7, hydroxide ion concentration is higher and the solution acts as a base.
The normal pH range of blood is given as 7.35 - 7.45 which is greater than 7. That means blood is slight basic in nature.
Let us find hydroxide ion concentration of blood.



![pOH = - log [OH-]](https://tex.z-dn.net/?f=pOH%20%3D%20-%20log%20%5BOH-%5D)
![[OH-] = 10^{-6.65}](https://tex.z-dn.net/?f=%5BOH-%5D%20%3D%2010%5E%7B-6.65%7D)
![[OH-] = 2.24 \times 10^{-7}](https://tex.z-dn.net/?f=%5BOH-%5D%20%3D%202.24%20%5Ctimes%2010%5E%7B-7%7D)
Ionic product of water is written as,
![[H+] [OH-] = 1 \times 10^{-14}](https://tex.z-dn.net/?f=%5BH%2B%5D%20%5BOH-%5D%20%3D%201%20%5Ctimes%2010%5E%7B-14%7D)
Let us plug in the calculated value of [OH-]
![[H+] = \frac{1 \times 10^{-14}}{2.24 \times 10^-7} = 4.46 \times 10^{-8} M](https://tex.z-dn.net/?f=%5BH%2B%5D%20%3D%20%5Cfrac%7B1%20%5Ctimes%2010%5E%7B-14%7D%7D%7B2.24%20%5Ctimes%2010%5E-7%7D%20%3D%204.46%20%5Ctimes%2010%5E%7B-8%7D%20M)
The hydrogen ion concentration for pH = 7.35 is 4.46 x 10⁻⁸ M
Calculation of [H+] for pH = 7.45
pOH = 6.55
[OH-] = 2.82 x 10⁻⁷
![[H+] = \frac{1 \times 10^{-14}}{2.82 \times 10^-7} = 3.54 \times 10^{-8} M](https://tex.z-dn.net/?f=%5BH%2B%5D%20%3D%20%5Cfrac%7B1%20%5Ctimes%2010%5E%7B-14%7D%7D%7B2.82%20%5Ctimes%2010%5E-7%7D%20%3D%203.54%20%5Ctimes%2010%5E%7B-8%7D%20M)
Similarly, for pH = 7.45, we get hydrogen ion concentration of 3.54 x 10⁻⁸ M.
Answer:
I've already given an answer to your questions in your previous post. please check it