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Ch.18 - Chemistry of the Environment
Chapter 18, Problem 42

The Ogallala aquifer described in the Closer Look box in Section 18.3, provides 82% of the drinking water for the people who live in the region, although more than 75% of the water that is pumped from it is for irrigation. Irrigation withdrawals are approximately 18 billion gallons per day. (a) Assuming that 2% of the rainfall that falls on an area of 600,000 km2 recharges the aquifer, what average annual rainfall would be required to replace the water removed for irrigation?

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Aquifer Recharge

Aquifer recharge refers to the process by which water from precipitation or surface water infiltrates into the ground and replenishes underground water reserves. In the context of the Ogallala aquifer, understanding how much rainfall contributes to this recharge is crucial for assessing the sustainability of water resources, especially when a significant portion is used for irrigation.
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Water Balance

Water balance is a hydrological concept that accounts for the inputs and outputs of water in a given system. It involves calculating the total amount of water entering (through precipitation and recharge) and leaving (through evaporation, transpiration, and withdrawals) the system. For the Ogallala aquifer, maintaining a positive water balance is essential to ensure that the aquifer can sustain its water supply for both drinking and irrigation.
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Irrigation Water Use

Irrigation water use refers to the amount of water extracted from sources like aquifers for agricultural purposes. In the case of the Ogallala aquifer, understanding the scale of irrigation withdrawals (18 billion gallons per day) is vital for calculating the necessary rainfall to replenish the aquifer. This concept highlights the significant impact of agricultural practices on water resources and the need for effective management strategies.
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Related Practice
Textbook Question

Phosphorus is present in seawater to the extent of 0.07 ppm by mass. Assuming that the phosphorus is present as dihydrogenphosphate, H2PO4-, calculate the correspond-ing molar concentration of H2PO4- in seawater.

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Textbook Question

The enthalpy of evaporation of water is 40.67 kJ/mol. Sunlight striking Earth's surface supplies 168 W per square meter (1 W = 1 watt = 1 J/s). (a) Assuming that evaporation of water is due only to energy input from the Sun, calculate how many grams of water could be evaporated from a 1.00 square meter patch of ocean over a 12-h day

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Textbook Question

The enthalpy of fusion of water is 6.01 kJ/mol. Sunlight striking Earth's surface supplies 168 W per square meter (1 W = 1 watt = 1 J/s). (b) The specific heat capacity of ice is 2.032 J/g°C. If the initial temperature of a 1.00 square emter patch of ice is -5.0°C, what is its final temperature after being in sunlight for 12 h, assuming no phase changes and assuming that sunlight penetration uniformly to a depth of 1.00 cm?

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Textbook Question

The organic anion

is found in most detergents. Assume that the anion under-goes aerobic decomposition in the following manner: C18H29SO3- + 51 O2 → 36 CO2(aq) + 28 H2O (l) + 2 H+(aq) + 2 SO42-(aq) What is the total mass of O2 required to biodegrade 10.0 g of this substance?

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Textbook Question

Magnesium ions are removed in water treatment by the addition of slaked lime, Ca(OH)2. Write a balanced chemical equation to describe what occurs in this process

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Textbook Question

In the lime soda process once used in large scale munici-pal water softening, calcium hydroxide prepared from lime and sodium carbonate are added to precipitate Ca2+ as CaCO3(s) and Mg2+ as Mg(OH)2(s): Ca2+(aq) + CO32-(aq) → CaCO3(s) Mg2+(aq) + 2 OH-(aq) → MgOH2(aq) How many moles of Ca(OH)2 and Na2CO3 should be added to soften (remove the Ca2+ and Mg2+) 1200 L of water in which [Ca2+] = 5.0x10-4 M and [Mg2+] = 7.0x10-4 M?

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