Answer:
Endergonic reaction or nonspontaneous reaction.
Explanation:
Gibbs free energy is a state function that determines the spontaneity or feasibility of the given reversible chemical reaction, at fixed pressure and temperature. It is given by the equation:
ΔG = ΔH - TΔS
Here, ΔG - change in Gibbs free energy
ΔH- The change in enthalpy of reaction
ΔS - The change in entropy
T- Temperature
When the <u>change in the Gibbs free energy for a given reaction is positive</u> (ΔG > 0), then that chemical reaction is known as an endergonic reaction or nonspontaneous reaction.
They all have the same number of electrons in the electron cloud.
All chemicals can cause harm. When only a very large amount of the chemical can cause damage, the chemical is considered to be practically non-toxic. When a tiny amount is harmful, the chemical is considered to be highly toxic.
<u> </u> The pH of 0.035 M aqueous aspirin is 2.48
<u>Explanation:</u>
We are given:
Concentration of aspirin = 0.035 M
The chemical equation for the dissociation of aspirin (acetylsalicylic acid) follows:
<u>Initial:</u> 0.035
<u>At eqllm:</u> 0.035-x x x
The expression of 
for above equation follows:
![K_a=\frac{[C_9H_7O_4^-][H^+]}{[HC_9H_7O_4]}](https://tex.z-dn.net/?f=K_a%3D%5Cfrac%7B%5BC_9H_7O_4%5E-%5D%5BH%5E%2B%5D%7D%7B%5BHC_9H_7O_4%5D%7D)
We are given:
Putting values in above expression, we get:
Neglecting the value of x = -0.0037 because concentration cannot be negative
So, concentration of 
= x = 0.0033 M
- 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:
= 0.0033 M
Putting values in above equation, we get:
Hence, the pH of 0.035 M aqueous aspirin is 2.48
