Sulfuric acid (H 2 SO 4 ) accounts for as much as 80 percent of the acid in acid rain. Its first ionization is complete, producing H + and the hydrogen sulfate ion: H 2 SO 4 ( a q ) ⇄ H + ( a q )+HSO 4 − ( a q ) Its second ionization, which produces additional H + and the sulfate ion, has an ionization constant ( K a2 ) of 1.3 × 10 −2 . HSO 4 − ( a q ) ⇄ H + ( a q )+SO 4 2 − ( a q ) Calculate the concentration of all species m a raindrop in which the sulfuric acid concentration is 4 00 × 10 −5 M . Assume that sulfuric acid is the only acid present.
Sulfuric acid (H 2 SO 4 ) accounts for as much as 80 percent of the acid in acid rain. Its first ionization is complete, producing H + and the hydrogen sulfate ion: H 2 SO 4 ( a q ) ⇄ H + ( a q )+HSO 4 − ( a q ) Its second ionization, which produces additional H + and the sulfate ion, has an ionization constant ( K a2 ) of 1.3 × 10 −2 . HSO 4 − ( a q ) ⇄ H + ( a q )+SO 4 2 − ( a q ) Calculate the concentration of all species m a raindrop in which the sulfuric acid concentration is 4 00 × 10 −5 M . Assume that sulfuric acid is the only acid present.
Solution Summary: The author explains that sulphuric acid is the only acid present in rain drop. The concentration of hydrogen ion is measured using pH scale and the acidity of aqueous
Sulfuric acid (H2SO4) accounts for as much as 80 percent of the acid in acid rain. Its first ionization is complete, producing H+ and the hydrogen sulfate ion:
H
2
SO
4
(
a
q
)
⇄
H
+
(
a
q
)+HSO
4
−
(
a
q
)
Its second ionization, which produces additional H+ and the sulfate ion, has an ionization constant (Ka2) of 1.3 × 10−2.
HSO
4
−
(
a
q
)
⇄
H
+
(
a
q
)+SO
4
2
−
(
a
q
)
Calculate the concentration of all species m a raindrop in which the sulfuric acid concentration is 4 00 × 10−5M. Assume that sulfuric acid is the only acid present.
Calculate the pOH of the following solutions at 25 degrees Celsius. c. [H+] = 12 Md. [H+] = 5.4 x 10^-5 MNote: Add trailing zeros to complete your answer to the 2nd decimal place, if necessary.
HCl(aq)+NaOH(aq)→NaCl(aq)+H2O(l)
Calculate ΔHrxn for the reaction at 3 different concentrations of HCl as listed in the image provided. Please state how the concentration of acid affect the heat of reaction (ΔHrxn)between a strong acid (HCl) and a strong base(NaOH)?
In an analysis carried out with water (H2O) at 90 °C, a chemist found an amount of hydroniums (H3O+) equal to 5 x 10-7mol/L and hydroxides (OH-) equal to 5 x 10-7mol/L. What will be the value of the water ionization constant Kw at this temperature?
a.
25 x 10-7
b.
2.5 x 10-14
c.
25 x 10-14
d.
1 x 10-7
e.
25
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