Calcium hypochlorite [Ca(OCl) 2 ] is used as a disinfectant for swimming pools. When dissolved in water it produces hypochlorous acid: Ca(OCl) 2 ( s ) + 2 H 2 O ( l ) ⇌ 2HClO ( a q ) + Ca(OH ) 2 ( s ) which ionizes as follows: HClO ( a q ) ⇌ H + ( a q ) + ClO − ( a q ) K a = 3.0 × 10 − 8 As strong oxidizing agents, both HClO and ClO − can kill bacteria by destroying their cellular components. However, too high a HClO concentration is irritating to the eyes of swimmers and too high a concentration of ClO − will cause the ions to decompose in sunlight. The recommended pH for pool water is 7.8. Calculate the percent of these species present at this pH.
Calcium hypochlorite [Ca(OCl) 2 ] is used as a disinfectant for swimming pools. When dissolved in water it produces hypochlorous acid: Ca(OCl) 2 ( s ) + 2 H 2 O ( l ) ⇌ 2HClO ( a q ) + Ca(OH ) 2 ( s ) which ionizes as follows: HClO ( a q ) ⇌ H + ( a q ) + ClO − ( a q ) K a = 3.0 × 10 − 8 As strong oxidizing agents, both HClO and ClO − can kill bacteria by destroying their cellular components. However, too high a HClO concentration is irritating to the eyes of swimmers and too high a concentration of ClO − will cause the ions to decompose in sunlight. The recommended pH for pool water is 7.8. Calculate the percent of these species present at this pH.
Solution Summary: The author explains the equilibrium expression for the reaction HA_(aq)stackrelto.
Calcium hypochlorite [Ca(OCl)2] is used as a disinfectant for swimming pools. When dissolved in water it produces hypochlorous acid:
Ca(OCl)
2
(
s
)
+
2
H
2
O
(
l
)
⇌
2HClO
(
a
q
)
+
Ca(OH
)
2
(
s
)
which ionizes as follows:
HClO
(
a
q
)
⇌
H
+
(
a
q
)
+
ClO
−
(
a
q
)
K
a
=
3.0
×
10
−
8
As strong oxidizing agents, both HClO and ClO− can kill bacteria by destroying their cellular components. However, too high a HClO concentration is irritating to the eyes of swimmers and too high a concentration of ClO− will cause the ions to decompose in sunlight. The recommended pH for pool water is 7.8. Calculate the percent of these species present at this pH.
The atmosphere contains 78% N2(g), 21% O2(g), and traces of other gases. These gases react at high temperature to form nitrogen monoxide, an important pollutant.
N2(g) + O2(g) = 2NO (g)
For this reaction at a certain temperature, Kc = 3.8 x 10^-5. If the initial concentration of N2(g) is 0.78 mol/L, and O2(g) is 0.21 mol/L, what will be the equilibrium concentration of NO(g) at this temperature?
Ozone is formed from oxygen. 3 O 2(g) 2 O 3(g) Calculate the value of K p at a temperature of 1.0 K, given that K c = 10.0 at that same temperature
Hemoglobin is the protein in red blood cells that transports oxygen to cells throughout your body. Each hemoglobin (Hb) molecule attaches to four oxygen molecules:
Hb(aq) + 4 O2(aq) ⇌ Hb(O2)4(aq)
In which direction does the above equilibrium shift in each of the following situations:
(a)At high elevations the air pressure is lowered reducing the [O2] in the blood.
(b)At high altitude, climbers sometimes breathe pressurized oxygen from a tank to increase the [O2] in the blood.
(c)People who live at higher altitudes produce more hemoglobin.
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Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell