From the molarity and volume of HClO4, we can determine how many moles of H+ we initially have:
0.18 M HClO4 * 0.100 L HClO4 = 0.018 moles H+
We can determine how many moles of OH- we have from the molarity and volume of LiOH:
0.27 M LiOH * 0.030 L LiOH = 0.0081 moles OH-
When the HClO4 and LiOH neutralize each other, the remaining will be
0.018 moles H+ - 0.0081 moles OH- = 0.0099 moles of excess H+
This means that the molarity [H+] will be
[H+] = 0.0099 moles H+ / (0.100 L + 0.030 L) = 0.07615 M
The pH of the solution will therefore be
pH = -log [H+] = -log 0.07615 = 1.12
Answer:
The answer is: 22, 4 liters
Explanation:
We use the formula PV=nRT
At STP: 1 atm of pressure and 273 K of temperature.
PV=nRT
V=nRT/P =1 mol x 0,082 l atm/L mol x 273 K /1 atm
V=22, 386 l
Answer:
a liquid
Explanation:
I'm not for sure but I just looked it up
The anwser to this question you have to do the work...
7+8+9+0
2-3=3112+4+6^4
78326-090+12^4567=3
#0380-90128+9328=3
so the awnser is cat.