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First, we write out a balanced equation.
HA <--> H(+) + A(-)
Next, we create an ICE table
HA <--> H+ + A-
[]i 0.40M 0M 0M
Δ[] -x +x +x
[]f 0.40-x x x
Next, we write out the Ka expression.
Ka = [H+][A-]/[HA]
Ka = x*x/(0.40-x)
However, because Ka is less than 10^-3, we can assume the amount of dissociation is negligible. Thus,
Assume 0.40-x ≈ 0.40
Therefore, 1.2x10^-6 = x^2/0.40
Then we solve for the [H+] concentration, or x
x=6.93x10^-4
Next, to find pH we do
pH = -log[H+]
pH = -log[6.93x10^-4]
pH = 3.2
HA <--> H(+) + A(-)
Next, we create an ICE table
HA <--> H+ + A-
[]i 0.40M 0M 0M
Δ[] -x +x +x
[]f 0.40-x x x
Next, we write out the Ka expression.
Ka = [H+][A-]/[HA]
Ka = x*x/(0.40-x)
However, because Ka is less than 10^-3, we can assume the amount of dissociation is negligible. Thus,
Assume 0.40-x ≈ 0.40
Therefore, 1.2x10^-6 = x^2/0.40
Then we solve for the [H+] concentration, or x
x=6.93x10^-4
Next, to find pH we do
pH = -log[H+]
pH = -log[6.93x10^-4]
pH = 3.2
A gas occupies 1.15 L at standard pressure and temperature and 1.56 L at 317 K and 650 mmHg, assuming ideal behavior.
<h3>What is an ideal gas?</h3>An ideal gas is a gas whose behavior can be explained through ideal gas laws. One of them is the combined gas law.
A gas occupies 1.15 L (V₁) at STP (T₁ = 273,15 K and P₁ = 760 mmHg). We can calculate the temperature (T₂) at which V₂ = 1.56 L and P₂ = 650 mmHg, using the combined gas law.
A gas occupies 1.15 L at standard pressure and temperature and 1.56 L at 317 K and 650 mmHg, assuming ideal behavior.
Learn more about ideal gases here: brainly.com/question/15634266
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