If a mixture of gases contained 78% nitrogen at a pressure of 984 torr and 22% carbon dioxide at 345 torr, what is the total pre
1 answer:
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Answer:
V = 11.2 L
Explanation:
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In this case, according to the ideal gas equation:
It is possible to compute the volume as shown below:
Whereas the moles are computed are computed given the mass and molar mass of oxygen:
Now, since the STP stands for a temperature of 273.15 K and a pressure of 1 atm, the resulting volume is:
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pH of 0.048 M HClO is 4.35.
<u>Explanation:</u>
HClO is a weak acid and it is dissociated as,
HClO ⇄ H⁺ + ClO⁻
We can write the equilibrium expression as,
Ka =
Ka = 4.0 × 10⁻⁸ M
4.0 × 10⁻⁸ M =
Now we can find x by rewriting the equation as,
x² = 4.0 × 10⁻⁸ × 0.048
= 1.92 × 10⁻⁹
Taking sqrt on both sides, we will get,
x = [H⁺] = 4.38 × 10⁻⁵
pH = -log₁₀[H⁺]
= - log₁₀[ 4.38 × 10⁻⁵]
= 4.35