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Alika [10]
3 years ago
10

While investigating greenhouse gases, I measured 0.1875 grams of carbon dioxide in a 500-gram sample of the atmosphere. What is

the concentration of CO₂ in the atmospheric sample?
Chemistry
1 answer:
Harlamova29_29 [7]3 years ago
6 0

Answer:

[CO₂] = 375 ppm

Explanation:

We can determine the concentration in value of ppm

ppm = mass of solute (mg) / mass of solution (kg)

Solution: atmosphere

Solute: CO₂

We convert the mass of CO₂ from g to mg → 0.1875 g . 1000 mg / 1g = 187.5 mg

We convert the mass of the atmosphere from g to kg: 500 g . 1 kg/1000g = 0.500 kg

ppm = 187.5 mg / 0.500kg = 375

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For Na2HPO4:(( (Note that for H3PO4, ka1= 6.9x10-3, ka2 = 6.4x10-8, ka3 = 4.8x10-13 ) a) The active anion is H2PO4- b) The activ
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Check the explanation

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K_{a1}=6.9x10^8, K_{a2} = 6.2X10^8, and K_{a3}=4.8X10^{13}

The transformation of H_2PO_4- (aq) to HPO_4^2-(aq)is the second dissociation, so we need to use the Ka2 = 6.2x10-8 in the Henderson-Hasselbalch equation.

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First we need to calculate moles of each

Moles of KH2PO4 = 22.0 g / 136.08 g.mol-1

                             = 0.162 moles

Moles of Na2HPO4 = 32.0 g /141.96 g.mol-1

                             = 0.225 moles

[H2PO4-] = 0.162 moles / 1.00 L = 0.162 M

[HPO42-] = 0.225 moles / 1.00 L = 0.225 M

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pKa2 = -log Ka

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       = 7.21

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pH = pKa + log [conjugate base] / [acid]

pH = 7.21 + log 0.225 / 0.162

     = 7.35

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