Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO 3 ). How much limestone (in kg) is required to completely neutralize a 4.3 billion liter lake with a pH of 5.5?

Hello everyone today, we're giving the following scenario and asked to find the mass of a statue that's lost. So the question says acid rain is a serious environmental problem that damages the ecosystem, destroys materials and has a negative has negative effects on human health. A limestone made buddhist statue in India has endured damaged caused by acid rain. If 1.546 times 10 to the seventh liter of rain water with a ph of 4.5 completely reacts with the statues. What mass of the statue is lost? So the first thing we have to do is calculate the concentration of hcl from its ph and so we can say that the concentration of our H. Plus is equal to 10 to the negative ph and this situation that ph is 4. And this is going to give us 3.16 times 10 to the -5 molar. Next we want to determine what the reaction equation is. And so we have our limestone which is C. A. C. 03 solid. It's going to react with two equivalence is of H. Plus and the acquis form that's gonna give us calcium two plus in the acquis form plus water in the liquid form plus C. +02 in the gas form. And so before we determine the mass of C. C. A. C. +03 lost, we have to include the molar mass of limestone which of C. A C. +03 which is 100.9 g per mole. And now we can solve for the mass of C. A. C. 03 that is lost or that has reacted. And so first we're going to start off with our leaders. So we have 1.546 times 10 to the seventh leaders. And then we're going to use a conversion factor that says that for every one liter of rainwater we have 3.16 times 10 to the negative five moles of H plus. We're then going to use a multiple ratio of H plus ions and calcium carbonate. So we can say that for every one mole or for every two moles of H plus ions, we have one mole of C A C +03. And then finally we want to determine the moles and grams. So therefore we have to use the molar mass. We say one mole of this, C a C +03 is equal to 100. g. And that's why we use the molar mass earlier. And so we need this answer in kilograms. And so to go from grams to kilograms, we can say that for every one kg that's equal to 10 to the third grams. And so this is going to give us our final answer of 24.4 kg lost. I hope this helped. And until next time

Ch.17 - Acids and Bases

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Tro 5th Edition

Ch.17 - Acids and Bases

Problem 132

Chapter 17, Problem 132

Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO₃). How much limestone (in kg) is required to completely neutralize a 4.3 billion liter lake with a pH of 5.5?

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Determine the concentration of hydrogen ions \([H^+]\) in the lake using the pH value: \([H^+] = 10^{-pH}\).

Calculate the total moles of \([H^+]\) in the lake by multiplying the concentration of \([H^+]\) by the volume of the lake in liters.

Write the balanced chemical equation for the neutralization reaction: \(CaCO_3 + 2H^+ \rightarrow Ca^{2+} + CO_2 + H_2O\).

Use stoichiometry to find the moles of \(CaCO_3\) needed, knowing that 1 mole of \(CaCO_3\) neutralizes 2 moles of \(H^+\).

Convert the moles of \(CaCO_3\) to mass in kilograms using the molar mass of \(CaCO_3\) (100.09 g/mol).

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Key Concepts

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

pH and Acidity

pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or alkalinity. A pH of 7 is neutral, while values below 7 indicate acidity. In this case, a pH of 5.5 suggests the lake is acidic, which can harm aquatic life. Understanding pH is crucial for determining how much limestone is needed to neutralize the lake.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt, effectively reducing the acidity of the solution. In this scenario, limestone (CaCO3) acts as a base that reacts with the hydrogen ions in the acidic lake water, raising the pH towards neutrality. Knowing the stoichiometry of this reaction is essential for calculating the amount of limestone required.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. To determine how much limestone is needed, one must use the molar mass of CaCO3 and the volume of the lake to find the total moles of hydrogen ions present. This allows for the precise calculation of limestone required to achieve neutralization.

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Stoichiometry Concept

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Textbook Question

The binding of oxygen by hemoglobin in the blood involves the equilibrium reaction: HbH⁺(aq) + O₂(aq) ⇌ HbO₂(aq) + H⁺(aq) In this equation, Hb is hemoglobin. The pH of normal human blood is highly controlled within a range of 7.35 to 7.45. Given the above equilibrium, why is this important? What would happen to the oxygen-carrying capacity of hemoglobin if blood became too acidic (a dangerous condition known as acidosis)?

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Textbook Question

Carbon dioxide dissolves in water according to the equations:

CO₂(g) + H₂O(l) ⇌ H₂CO₃(aq)

H₂CO₃(aq) + H₂O(l) ⇌ HCO₃^–(aq) + H₃O⁺(aq)

Carbon dioxide levels in the atmosphere have increased about 20% over the last century. Given that Earth's oceans are exposed to atmospheric carbon dioxide, what effect might the increased CO₂ be having on the pH of the world's oceans? What effect might this change be having on the limestone structures (primarily CaCO₃) of coral reefs and marine shells?

Textbook Question

People often take milk of magnesia to reduce the discomfort associated with acid stomach or heartburn. The recommended dose is 1 teaspoon, which contains 4.00×10² mg of Mg(OH)₂. What volume of an HCl solution with a pH of 1.3 can be neutralized by one dose of milk of magnesia? If the stomach contains 2.00×10² mL of pH 1.3 solution, is all the acid neutralized? If not, what fraction is neutralized?

Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO3). How much limestone (in kg) is required to completely neutralize a 4.3 billion liter lake with a pH of 5.5?

Verified video answer for a similar problem:

Key Concepts

pH and Acidity

Neutralization Reaction

Stoichiometry

Lakes that have been acidified by acid rain can be neutralized by liming, the addition of limestone (CaCO₃). How much limestone (in kg) is required to completely neutralize a 4.3 billion liter lake with a pH of 5.5?