Sulfur oxides and nitrogen oxides are pollutants that are produced when fossil fuels are burned. Sulfur oxides and nitrogen oxides react with water in the atmosphere, which leads to the production of sulfuric acid and nitric acid, and thu naturally acidic and has a pH of approximately 5.6, but acid rain has a lower pH, sometimes below 4. One of the effects of acid rain is to increase the rate of deterioration of statues and buildings made of limestone and marble. Limes composed of calcium carbonate, CaCO3, which is not very soluble in pure water. The following equations can be written for the carbonate ion. Co2?- (ag) + H20(1) → HCO3 (ag) + OH¯(aq) co,?- (aq) + H3O*(aq) → HCO3¯(aq) + H2O(1) Which of the following correctly compares the H* concentration in acid rain with a pH of 4.6 to the H* concentration in rain that is naturally acidic and has a pH of 5.6? A The Ht concentration in the acid rain is a factor of () times shigh as the H* concentration in the rain that s naturally acidic. The Ht concentration in the acid rain is 2 times as high as the Ht concentration in the rain that is naturally acidic. C) The H* concentration in the acid rain is 4.6 times as high as the H concentration in the rain that is naturally acidic. D) The H+ concentration in the acid rain is 10 times as high as the Ht concentration in the rain that is naturally acidic.
Sulfur oxides and nitrogen oxides are pollutants that are produced when fossil fuels are burned. Sulfur oxides and nitrogen oxides react with water in the atmosphere, which leads to the production of sulfuric acid and nitric acid, and thu naturally acidic and has a pH of approximately 5.6, but acid rain has a lower pH, sometimes below 4. One of the effects of acid rain is to increase the rate of deterioration of statues and buildings made of limestone and marble. Limes composed of calcium carbonate, CaCO3, which is not very soluble in pure water. The following equations can be written for the carbonate ion. Co2?- (ag) + H20(1) → HCO3 (ag) + OH¯(aq) co,?- (aq) + H3O*(aq) → HCO3¯(aq) + H2O(1) Which of the following correctly compares the H* concentration in acid rain with a pH of 4.6 to the H* concentration in rain that is naturally acidic and has a pH of 5.6? A The Ht concentration in the acid rain is a factor of () times shigh as the H* concentration in the rain that s naturally acidic. The Ht concentration in the acid rain is 2 times as high as the Ht concentration in the rain that is naturally acidic. C) The H* concentration in the acid rain is 4.6 times as high as the H concentration in the rain that is naturally acidic. D) The H+ concentration in the acid rain is 10 times as high as the Ht concentration in the rain that is naturally acidic.
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Transcribed Image Text:nd nitrogen oxides are pollutants that are produced when fossil fuels are burned. Sulfur oxides and nitrogen oxides react with water in the atmosphere, which leads to the production of sulfuric acid and nitric acid, and thus acid rain. Rainwater is
and has a pH of approximately 5.6, but acid rain has a lower pH, sometimes below 4. One of the effects of acid rain is to increase the rate of deterioration of statues and buildings made of limestone and marble. Limestone and marble are
alcium carbonate, CaCO3, which is not very soluble in pure water.
quations can be written for the carbonate ion.
Нао() > нсо3 (ад) + Он (ад)
H30+(ag) → HCO3 (aq) + H20(1)
lowing correctly compares the H* concentration
acid rain with a pH of 4.6 to the HT concentration in rain that
naturally acidic and has a pH of 5.6?
H+ concentration in the acid rain is a factor of (2) times as high as the Ht concentration in the rain that is naturally acidic.
Ht concentration in the acid rain is 2 times as high as the H* concentration
the rain that is naturally acidic.
Ht concentration in the acid rain is 4.6 times as high as the Ht concentration in the rain that is naturally acidic.
Ht concentration in the acid rain is 10 times as high as the Ht concentration in the rain that is naturally acidic.
Transcribed Image Text:Sulfur oxides and nitrogen oxides are pollutants that are produced when fossil fuels are burned. Sulfur oxides and nitrogen oxides react with water in the atmosphere, which leads to the production of sulfuric acid and nitric acid, and thus
naturally acidic and has a pH of approximately 5.6, but acid rain has a lower pH, sometimes below 4. One of the effects of acid rain is to increase the rate of deterioration of statues and buildings made of limestone and marble. Limestor
composed of calcium carbonate, CaCO3, which is not very soluble in pure water.
The following equations can be written for the carbonate ion.
Соз (ад) + H2О() — нСОз (ад) + он (ад)
соз- (аq) + Hзot(ag) — нсоз (ag) + H20(0)
Which of the following correctly compares the H* concentration in acid rain with a pH of 4.6 to the Ht concentration in rain that is naturally acidic and has a pH of 5.6?
A
The Ht concentration in the acid rain is a factor of (2) times as high as the Ht concentration in the rain that is naturally acidic.
B
The Ht concentration in the acid rain is 2 times as high as the Ht concentration in the rain that is naturally acidic.
The Ht concentration in the acid rain is 4.6 times as high as the Ht concentration in the rain that is naturally acidic.
D) The H+ concentration in the acid rain is 10 times as high as the Ht concentration in the rain that is naturally acidic.
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