Chemical Weathering & Soil Erosion a) How is carbonic acid (H2CO3) formed in nature? b) What...

Chemical Weathering & Soil Erosion

a) How is carbonic acid (H₂CO₃) formed in nature?
b) What controls the soil formation?
c) Is soil erosion a natural process or primarily the result of inappropriate land use by people? Explain.

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Amanda K answered 1 year ago

During chemical weathering, forsterite is dissolved by the carbonic acid in rainwater. The weathering reaction is:...

During chemical weathering, forsterite is dissolved by the carbonic acid in rainwater. The weathering reaction is: Mg2SiO4 forsterite + 4H2CO3 (aq) ? 2Mg2+ + 4HCO3- + H4SiO4 (aq) Use the thermodynamic data from Appendix II, source 2, for the following calculations. 4a. Calculate the Keq for this weathering reaction at 25 �C. 4b. If the reaction is at equilibrium, using Le Cha?telier�s principle, predict what would happen if Mg2+ ions were added to the solution 4c. Using Le Cha?telier�s principle,...

Carbonic acid (H2CO3) is a diprotic weak acid that undergoes the following dissociation reactions: H2CO3 ⇌...

Carbonic acid (H2CO3) is a diprotic weak acid that undergoes the following dissociation reactions: H2CO3 ⇌ H+ + HCO3− Ka1 = 4.3 x 10−7 HCO3− ⇌ H+ + CO32− Ka2 = 5.6 x 10−11 For a 0.020 M solution of carbonic acid in water, which of the following is true? [HCO3−] = [CO32−] [H+] = Ka1 [CO32−] = Ka2 Ka1 = Ka2 [H+] = Ka2

Carbonic acid, H2CO3, is a weak diprotic acid. In a 0.1 M solution of the acid,...

Carbonic acid, H2CO3, is a weak diprotic acid. In a 0.1 M solution of the acid, which of the following species is present in the largest amount? H2CO3. H3O+ HCO3

Acetaminophen is a weaker acid than carbonic acid (H2CO3), but aspirin is a stronger acid than...

Acetaminophen is a weaker acid than carbonic acid (H2CO3), but aspirin is a stronger acid than carbonic acid. prepare a flow diagram like the one in this experiment, showing a procedure that can be used to separate a mixture of sucrose, aspirin, and acetaminophen.

Match the following solutions to the best description. 0.14 M carbonic acid H2CO3 [...

Match the following solutions to the best description. 0.14 M carbonic acid H2CO3 [ Choose ] acidic and hypotonic neutral and hypotonic neutral and isotonic basic and isotonic basic and hypotonic acid and hypertonic basic and hypertonic acidic and isotonic neutral and hypertonic 0.14 M ammonium hydroxide NH4OH...

1.Explain how carbonic acid and bicarbonate are formed in the blood and the functions they serve....

1.Explain how carbonic acid and bicarbonate are formed in the blood and the functions they serve. 2. Define the terms acidosis and alkalosis, and explain how they relate to hypoventilation and hyperventilation. 3. Explain how ventilation is adjusted to help maintain acid-base balance.

With the titration of 281 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x...

With the titration of 281 mL of 0.501 M carbonic acid (H2CO3) (Ka1 = 4.3 x 10-7, Ka2 = 5.6 x 10-11) with 1.1 M NaOH. How many mL of the 1.1 M NaOH are needed to raise the pH of the carbonic acid solution to a pH of 6.019?

A. Calculate the hydronium ion concentration in an aqueous solution of 0.185 M carbonic acid, H2CO3...

A. Calculate the hydronium ion concentration in an aqueous solution of 0.185 M carbonic acid, H2CO3 (aq) B. Calculate the concentration of HCO3- in an aqueous solution of 0.1860 M carbonic acid, H2CO3 (aq).

Consider a the titration of 0.905 L of 0.679 M carbonic acid (H2CO3) with 1.65 M...

Consider a the titration of 0.905 L of 0.679 M carbonic acid (H2CO3) with 1.65 M NaOH. What is the pH at the second equivalence point of the titration?

Carbonic acid,H2CO3 , can be found in a wide variety of body fluids (from dissolved CO2...

Carbonic acid,H2CO3 , can be found in a wide variety of body fluids (from dissolved CO2 ). Calculate the hydronium ion concentration of a 4.65xten to the negative fourth M H2CO3 solution. What is the concentration of CO3 2- ? Ka1 equals 4.3 x 10 to the negative seventh Ka2 equals 4.8x10 to the negative eleventh

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