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Ymorist [56]
3 years ago
15

(g) The mole fraction of O2 in atmospheric air is 0.21. Calculate the concentration of O2 in a sample of atmospheric air in a 10

L container at a pressure of 650 mmHg and temperature of 160 °C.
Chemistry
1 answer:
irinina [24]3 years ago
4 0

Answer:

The concentration of O₂ in the sample is 5,1x10⁻³ M (mol/L)

Explanation:

To obtain the moles of gas you should use ideal gas formula:

PV/RT = n

Where:

P is pressure: 650 mmHg or 650 mmHg* ( 1 atm / 760 mmHg) = 0,855 atm

V is volume: 10 L

R is gas constant: 0,082 atm·L/mol·K

T is temperature: 160°C or 160 + 273,15 = 433,15 K

And n is mol number

Thus, replacing bold values in ideal gas formula:

n =  0,24 mol

The mole fraction of O₂ in atmospheric air is 0,21. Thus, the moles of O₂ there are:

0,24 moles of atmospheric air ₓ 0,21 = 0,051 O₂ moles

There are many ways to express concentration but we will express it in molarity (mol of solute / L of solution) understanding solute as O₂ and solution as atmospheric air. So:

0,051 O₂ moles / 10 L = 5,1x10⁻³ M -<em>M is molarity</em>-

I hope it helps!

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An analytical chemist is titrating of a solution of nitrous acid with a solution of . The of nitrous acid is . Calculate the pH
Burka [1]

Answer:

pH = 2.69

Explanation:

The complete question is:<em> An analytical chemist is titrating 182.2 mL of a 1.200 M solution of nitrous acid (HNO2) with a solution of 0.8400 M KOH. The pKa of nitrous acid is 3.35. Calculate the pH of the acid solution after the chemist has added 46.44 mL of the KOH solution to it.</em>

<em />

The reaction of HNO₂ with KOH is:

HNO₂ + KOH → NO₂⁻ + H₂O + K⁺

Moles of HNO₂ and KOH that react are:

HNO₂ = 0.1822L × (1.200mol / L) = <em>0.21864 moles HNO₂</em>

KOH = 0.04644L × (0.8400mol / L) = <em>0.0390 moles KOH</em>

That means after the reaction, moles of HNO₂ and NO₂⁻ after the reaction are:

NO₂⁻ = 0.03900 moles KOH = moles NO₂⁻

HNO₂ = 0.21864 moles HNO₂ - 0.03900 moles = 0.17964 moles HNO₂

It is possible to find the pH of this buffer (<em>Mixture of a weak acid, HNO₂ with the conjugate base, NO₂⁻), </em>using H-H equation for this system:

pH = pKa + log₁₀ [NO₂⁻] / [HNO₂]

pH = 3.35 + log₁₀ [0.03900mol] / [0.17964mol]

<h3>pH = 2.69</h3>
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Answer:

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