The concentration of hydroxide ion is 5 10^
−
14 M.
<u>Explanation:</u>
Consider the equilibrium of this acid's dissociation,
H C l O 4 ⇌ H + + C l O 4 -
Moreover, let's assume that H C l O 4 is a strong acid and will fully dissociate.
Hence,
[ H + ] = 0.20 M
Now, recall,
K
w = [
H
+
]
[
O
H
−
] = 1.0 10
^−
14
Hence,
⇒
[
O
H
−
] = K
w / [
H
+
] = 5 10^
−
14 M.
Answer:
0.7457 g is the mass of the helium gas.
Explanation:
Given:
Pressure = 3.04 atm
Temperature = 25.0 °C
The conversion of T( °C) to T(K) is shown below:
T(K) = T( °C) + 273.15
So,
T₁ = (25.0 + 273.15) K = 298.15 K
Volume = 1.50 L
Using ideal gas equation as:
where,
P is the pressure
V is the volume
n is the number of moles
T is the temperature
R is Gas constant having value = 0.0821 L.atm/K.mol
Applying the equation as:
3.04 atm × 1.50 L = n × 0.0821 L.atm/K.mol × 298.15 K
<u>⇒n = 0.1863 moles</u>
Molar mass of helium = 4.0026 g/mol
The formula for the calculation of moles is shown below:
Thus,
<u>0.7457 g is the mass of the helium gas. </u>