Let's solve ~
Initial concentration of weak acid HA = 0.200 M
and dissociation constant (
) is :
Now, at initial stage :
At equilibrium :
Now, we know :
![\qquad \sf \dashrightarrow \: { K_a = \dfrac{[H+] [A-]}{[HA]}}](https://tex.z-dn.net/?f=%5Cqquad%20%5Csf%20%20%5Cdashrightarrow%20%5C%3A%20%7B%20K_a%20%3D%20%5Cdfrac%7B%5BH%2B%5D%20%5BA-%5D%7D%7B%5BHA%5D%7D%7D%20)
( big brackets represents concentration )
Answer:
A strong base, such as NaOH. The amount of OH added shouldn't exceed 0.35 mols (though i would stop at 0.30 mols)
Explanation:
a weakly basic salt can be turned into a buffer by the addition of a strong base, and a weakly acidic salt can be turned into a buffer with a strong acid
Answer:
The new temperature will be 2546 K or 2273 °C
Explanation:
Step 1: Data given
The initial temperature = 1000 °C =1273 K
The volume = 20L
The volume increases to 40 L
Step 2: Calculate the new temperature
V1/T1 = V2/T2
⇒with V1 = the initial volume = 20L
⇒with T1 = the initial temperature = 1273 K
⇒with V2 = the increased volume = 40L
⇒with T2 = the new temperature = TO BE DETERMINED
20L/ 1273 K = 40L / T2
T2 = 40L / (20L/1273K)
T2 = 2546 K
The new temperature will be 2546 K
This is 2546-273 = 2273 °C
Since the volume is doubled, the temperature is doubled as well
