Answer:
I think w but I don't know
Answer:
The ratio [A-]/[HA] increase when the pH increase and the ratio decrease when the pH decrease.
Explanation:
Every weak acid or base is at equilibrium with its conjugate base or acid respectively when it is dissolved in water.
⇄ 
This equilibrium depends on the molecule and it acidic constant (Ka). The Henderson-Hasselbalch equation,
![pH = pKa + Log \frac{[A^{-}]}{[HA]}](https://tex.z-dn.net/?f=pH%20%3D%20pKa%20%2B%20Log%20%5Cfrac%7B%5BA%5E%7B-%7D%5D%7D%7B%5BHA%5D%7D)
shows the dependency between the pH of the solution, the pKa and the concentration of the species. If the pH decreases the concentration of protons will increase and the ratio between A- and AH will decrease. Instead, if the pH increases the concentration of protons will decreases and the ratio between A- and AH will increase.
Answer:
Should be 0.6106 though i could be wrong
Explanation:
Answer:
E = 3 × 10¹⁰ J
Explanation:
Mass, m = 100 kg
We need to find energy made by the loss of 100 kg of mass. The formula between the mass and energy is given by :
E = mc²
Where c is speed of light
Putting all the values, we get :
E = 100 kg × (3×10⁸ m/s)²
= 3 × 10¹⁰ J
So, the required energy is 3 × 10¹⁰ J.
The physical explanation is that increasing temperature increases the kinetic energy of the gas molecules. Hence, their random motion breaks more intermolecular bonds and the gas is less dissolved in the solvent. In contrast, solid solutes in water have increased solubility with increased temperatures.