2.10 x 10^-10 M. Ans
pH + pOH = 14
Where, pOH is the power of hydroxide ion concentration and pH is the power of concetration of the H+ ion.
Now, pOH = 14 - 4.32
= 9.68
Now, the concentration of [H+] is 10-7 M, then pH is 7 and for [OH-] = 10-7 M, the pOH is also 7.
Now, pOH = -log[OH-]
[OH-] = 10^- pOH
= 10^-9.68
= 2.10 x 10^-10 M
Answer:
0.047 %
Explanation:
Step 1: Given data
- Partial pressure of ozone (pO₃): 0.33 torr
- Total pressure of air (P): 695 torr
Step 2: Calculate the %v/v of ozone in the air
Air is a mixture of gases. We can find the %v/v of ozone (a component) in the air (mixture) using the following expression.
<em>%v/v = pO₃/P × 100%</em>
%v/v = 0.33 torr/695 torr × 100%
%v/v = 0.047 %
Answer:
22.8 L
Step-by-step explanation:
We can use <em>Gay-Lussac's Law of Combining Volumes</em> to solve this problem:
Gases <em>at the same temperature and pressure</em> react in simple whole-number ratios.
1. Write the chemical equation.
Ratio: 2 L 1 L
Ca(s) + 2HCl(g) ⟶ CaCl₂(s) + H₂(g)
V/L: 11.4
2. Calculate the volume of HCl.
According to the law, 2 L of HCl form 1 L of H₂.
Then, the conversion factor is (2 L HCl/1 L H₂).
Volume of HCl = 11.4 L H₂ × (2 L HCl/1 L H₂)
= 22.8 L HCl
Answer:
Mole fraction N₂ = 0.336
Explanation:
Mole fraction of a gas can be determined in order to know the partial pressure of the gas, and the total pressure, in the mixture.
Total pressure in the mixture: Sum of partial pressure from all the gases
Total pressure = 183 mmHg + 443 mmHg + 693 mmHg =1319 mmHg
Mole fraction N₂ = Partial pressure N₂ / Total pressure
443 mmHg / 1319 mmHg = 0.336
Remember that mole fraction does not carry units
Gas particles spread out to fill a container evenly, unlike solids and liquids. Gas is a state of matter that has no fixed shape and no fixed volume. Gases have lower density than other states of matter, such as solids and liquids. Hence above statement is FALSE.