Answer:
The hydrogen ion concentrations associated with these pH value 7.35 is 
The hydrogen ion concentrations associated with these pH value 7.45 is
.
Explanation:
To calculate the pH of the solution, we use the equation:
![pH=-\log[H^+]](https://tex.z-dn.net/?f=pH%3D-%5Clog%5BH%5E%2B%5D)
We are given:
1) pH = 7.35
Putting values in above equation, we get:
![7.35=-\log[H^+]](https://tex.z-dn.net/?f=7.35%3D-%5Clog%5BH%5E%2B%5D)
![[H^+]=4.467\times 10^{-8} M\approx 4.5\times 10^{-8} M](https://tex.z-dn.net/?f=%5BH%5E%2B%5D%3D4.467%5Ctimes%2010%5E%7B-8%7D%20M%5Capprox%204.5%5Ctimes%2010%5E%7B-8%7D%20M)
The hydrogen ion concentrations associated with these pH value 7.35 is 
2) pH = 7.45
Putting values in above equation, we get:
![7.45=-\log[H^+]](https://tex.z-dn.net/?f=7.45%3D-%5Clog%5BH%5E%2B%5D)
![[H^+]=3.548\times 10^{-8}M \approx 3.6\times 10^{-8} M](https://tex.z-dn.net/?f=%5BH%5E%2B%5D%3D3.548%5Ctimes%2010%5E%7B-8%7DM%20%5Capprox%203.6%5Ctimes%2010%5E%7B-8%7D%20M)
The hydrogen ion concentrations associated with these pH value 7.45 is
.
Answer:
Magnesium oxide is a binary compound of magnesium and oxygen while magnesium ribbon consists only of magnesium atoms.
Explanation:
The burning of magnesium in oxygen is a chemical change. It produces magnesium oxide having greater mass than magnesium ribbon. The greater mass results from the fact that the chemical reaction has added another element to the sample- oxygen. The mass of magnesium ribbon is the mass of magnesium atoms alone but in magnesium oxide, we consider the masses of magnesium and oxygen atoms making magnesium oxide heavier than magnesium ribbon.
Riley can either change the surface area of the object or can change the slipperiness of the material.
The –OH+ group is most acidic proton in ln-OH as shown in figure (a). The proton is circled in the figure.
The stabilisation of the conjugate base produced is stabilises due to resonance factor. The possible resonance structures are shown in figure (b).
The acidity of a protonated molecule depends upon the stabilisation of the conjugate base produced upon deprotonation. The conjugate base of ln-OH is shown in figure (a).
The possible resonance structures are shown in figure (b). As the number of resonance structures of the conjugate base increases the stabilisation increases. Here the unstable quinoid (unstable) form get benzenoid (highly stable) form due to the resonance which make the conjugate base highly stabilise.
Thus the most acidic proton is assigned in ln-OH and the stability of the conjugate base is explained.