Answer : The pH of solution at the half‑equivalence point is, 4.1
Explanation :
As we known that the titration takes place between strong base and weak acid.
So, at half‑equivalence point of a titration the pH of the solution is equal to the of weak acid.
As we are given:
Now we have to calculate the value of .
The expression used for the calculation of is,
Now put the value of in this expression, we get:
Thus,
Therefore, the pH of solution at the half‑equivalence point is, 4.1
Answer:
Anions or negatively-charged ions
Explanation:
The answer is ultraviolet
Answer:
<u>1092K</u>
Explanation:
We can use the combined gas law to answer this question:
P1V1/T1 = P2V2/T2,
where P, V and T are the Pressure, Volume, and Temperature for initial (1) and Final (2) conditions. Temperatures must be in Kelvin.
The problem states that V2 = 2V1 and P2 = 2P1.
Let's rearrange to solve for T2, which is the question:
T2 = T1(P2/P1)(V2/V1)
Note how the pressure and temperature values are written: as ratios. Enter the values:
T2 = (273K)(P2/P1)(V2/V1)
T2 = (273K)(2P1/P1)(2V1/V1) [Use the expressions for V2 and P2 from above]
T2 = (273K)(2)(2)
T2 = 1092K
1. c. 35
2. <span>d. 1.26 x 10^24 molecules
3. </span><span>d. 303.6 g</span>