50 mL of 2.0 M of 
and 25 mL of 2.0 M of 
were mixed to make a solution
Final volume of the solution after dilution = 200 mL (given)
Final concentration of , [] = 
Final concentration of , [] = 
Using Hasselbach- Henderson equation:
![pH = pK_a+ log \frac{[salt]}{[acid]}](https://tex.z-dn.net/?f=pH%20%3D%20pK_a%2B%20log%20%5Cfrac%7B%5Bsalt%5D%7D%7B%5Bacid%5D%7D)
Substituting the values:
Hence, the 
of the final solution is 7.15.
Answer:
Mass of KOH = 497.78 g
Explanation:
Given data
mass of KOH = ?
number of KOH molecules = 5.34 × 10²⁴
molar mass of KOH = 56.12 g/mol
Solution
1st we find out the number of moles of KOH
<em>number of moles = number of molecules given / Avogadro number
</em>
number of moles of KOH = 5.34 × 10²⁴ / 6.022 × 10²³
number of moles of KOH = 8.87 mol
Now we find out the mass of KOH
<em>Mass of KOH = moles × molar mass</em>
Mass of KOH = 8.87 mol × 56.12 g/mol
Mass of KOH = 497.78 g
K.E. = 1/2 mv2
m= mass
v= volume
and since its measured in Joules, 1 Joule is equal to 1 kilogram-meters squared per second squared.
~Hope that helped!~
~Izzy~
It beaded up and rolls off
I did it myself
