How do the isotopes hydrogen-1 and hydrogen-2 differ?
2 answers:
<u>Answer:</u> They differ by the number of neutrons
<u>Explanation:</u>
Isotopes are defined as the chemical species which have same number of protons but differ in the number of neutrons.
The general isotopic representation is
where,
Z = Atomic number of the atom
A = Mass number of the atom
X = Symbol of the atom
Atomic number is defined as the number of protons or electrons that are present in a neutral atom.
Atomic number = number of protons = number of electrons
Mass number is defined as the sum of number of protons and number of neutrons present in an atom.
Mass number = Number of neutrons + Number of protons.
We are given two isotopes:
- <u>For
isotope:</u>
Number of protons = 1
Mass number = 1
Number of neutrons = 1 - 1 = 0
- <u>For
isotope:</u>
Number of protons = 1
Mass number = 2
Number of neutrons = 2 - 1 = 1
Hence, they differ by the number of neutrons
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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
