Approximately how much greater in mass is a d2o molecule than an h2o molecule? (assume the oxygen atoms have a mass number of 16
2 answers:
The deuteriuoted water that is consists of an isotope of hydrogen in place of hydrogen from the normal water. The approximate mass of deuteriuoted water and normal water can be calculated as {(2×2)+16} = 20. However the exact mass of
is 20.027 g/mole, whereas the mass of water can also be calculated as- {(1×2)+16}=18, however the exact mass of (
) molecule is 18.015 g/mole. Thus the difference between the mass of the molecules are (20.027 - 18.015) = 2.01 2g/mole.
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Answer:
pH after the addition of 10 ml NaOH = 4.81
pH after the addition of 20.1 ml NaOH = 8.76
pH after the addition of 25 ml NaOH = 8.78
Explanation:
(1)
Moles of butanoic acid initially present = 0.1 x 20 = 2 m moles = 2 x 10⁻³ moles,
Moles of NaOH added = 10 x 0.1 = 1 x 10⁻³ moles
CH₃CH₂CH₂COOH + NaOH ⇄ CH₃CH₂CH₂COONa + H₂O
Initial conc. 2 x 10⁻³ 1 x 10⁻³ 0
Equilibrium 1 x 10⁻³ 0 1 x 10⁻³
Final volume = 20 + 10 = 30 ml = 0.03 lit
So final concentration of Acid =
Final concentration of conjugate base [CH₃CH₂CH₂COONa]
Since a buffer solution is formed which contains the weak butanoic acid and conjugate base of that acid .
Using Henderson Hasselbalch equation to find the pH
