Answer: pH of resulting solution will be 13
Explanation:
pH is the measure of acidity or alkalinity of a solution.
Moles of 
ion = 
Moles of 
ion = 
For neutralization:
1 mole of ion will react with 1 mole of ion
0.01 mol of ion will react with =
of ion
Thus (0.012-0.01)= 0.002 moles of are left in 20 ml or 0.02 L of solution.
![[OH^-]=\frac{0.002}{0.02L}=0.1M](https://tex.z-dn.net/?f=%5BOH%5E-%5D%3D%5Cfrac%7B0.002%7D%7B0.02L%7D%3D0.1M)
![pOH=-log[OH^-]](https://tex.z-dn.net/?f=pOH%3D-log%5BOH%5E-%5D)
![pOH=-log[0.1]=1](https://tex.z-dn.net/?f=pOH%3D-log%5B0.1%5D%3D1)
Thus the pH of resulting solution will be 13
Answer:
C24H50
Explanation:
The empirical fomula's molar mass is 169.25 g/mol.
We know the molecular formula's molar mass is 338 g/mol.
338/169.25= 1.99 or approximately 2
Answer:
22.8 L
Explanation:
Step 1: Given data
- Moles of the gas (n): 1.35 mol
- Pressure of the gas (P): 1.30 atm
- Ideal gas constant (R): 0.0821 atm.L/mol.K
Step 2: Convert "T" to Kelvin
We will use the following expression.
K = °C + 273.15 = -6 + 273.15 = 267 K
Step 3: Calculate the volume of the gas
We will use the ideal gas equation.
P × V = n × R × T
V = n × R × T / P
V = 1.35 mol × (0.0821 atm.L/mol.K) × 267 K / 1.30 atm
V = 22.8 L
