Calculate the pH of a 0.10 M solution of NaOH. Express your answer numerically using two decimal places. • View Available Hint(s) 1ν ΑΣφ ? pH = Submit - Part C Calculate the pH of a 0.10 M solution of hydrazine, N2H4. K, for hydrazine is Express your answer numerically using two decimal places. • View Available Hint(s) ?
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19 Please answer B and C part
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Part B
The pH of a solution is the negative logarithm of the molar
concentration of hydronium ion, that is,
Calculate the pH of a 0.10 M solution of NaOH.
Express your answer numerically using two decimal places.
pH = -log[H3O+]
In neutral solutions at 25 ° C, [H30+] = 10-7 M and
pH = 7. As [H3O+] increases, pH decreases, so acidic
solutions have a pH of less than 7. Basic solutions have a pH
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greater than 7.
?
The hydroxide and hydronium ion concentrations are related
by the the ion-product constant of water, Ku , as follows:
pH =
1.0 × 10-14
Kw
= [H3O+][OH¯]
Submit
In the same way as the pH, we can define the pOH as
pOH = -log[OH ]. It follows from the Kw expression that
pH+ pОН — 14.
Part C
Calculate the pH of a 0.10 M solution of hydrazine, N2H4. K, for hydrazine is 1.3 × 10-0.
Express your answer numerically using two decimal places.
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Nνα ΑΣφ
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