In this item, I supposed, that we are determine the molar fraction of oxygen and carbon dioxide in the sample. This can be done by dividing their respective partial pressures by the total pressure of the sample.
O2 : mole fraction = (100.7 mmHg) / (763.00 mmHg) = 0.13
CO2 : mole fraction = (33.57 mmHg) / (763.00 mmHg) = 0.044
Answers: O2 = 0.13
CO2 = 0.044
A homogenous mixture is that mixture in which the components mix with each other and its composition is uniform throughout the solution. A heterogenous mixture is that mixture in which the composition is not uniform throughout and different components are observed.
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Total volume required = 100mL
The concentration of carbonic acid = 0.025
Let concentration of sodium bi carbonate = [NaHCO3]
From Hendersen Hassalbalch's equation for buffers
pH = pKa + log [salt] / [acid]
pKa of carbonic acid = 6.35
7.25 = 6.35 + log [NaHCO3] / 0.025
0.9 = log [NaHCO3] / 0.025
Taking antilog
7.943 = [NaHCO3] / 0.025
[NaHCO3] = 7.943 X 0.025
[NaHCO3] = 0.199 M
Volume is 100mL
Moles of NaHCO3 = molarity X volume (L) = 0.199 X 0.1 = 0.0199
Mass of NaHCO3 = moles X molar mass = 0.0199 X 84 = 1.672 g
moles of H2CO3 = molarity X volume (L) = 0.025 X 0.1 = 0.0025
Mass of H2CO3 = moles X molar mass = 0.0025 X 62 = 0.155 g
Answer:
7.86 g/cm³
Explanation:
11.0 kg = 11,000 g
The density in g/cm³ is ...
(11,000 g)/(1,400 cm³) = 7.86 g/cm³