People often take milk of magnesia to reduce the discomfort associated with acid stomach or heartburn. The recommended dose is 1 teaspoon, which contains 4.00×10 2 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 2.00×10 2 mL of pH 1.3 solution, is all the acid neutralized? If not, what fraction is neutralized?

Hello everyone today, we have been given the following scenario and asked to analyze it. So it says laboratory preparation of carbon dioxide gas is often carried out by reacting limestone with hydrochloric acid. The limestone dissolves completely into the acid solution and produces C. A. C. L. To water. And carbon dioxide were then asked to determine the volume. And middle leaders of the ph of 1.1 hydrochloric acid solution that could dissolve a 1.15 grand piece of limestone. Could the same piece of limestone neutralize a 350 sample of hcl solution with a ph of 1.1, if not what fraction can neutralize. And so the first thing we want to do is we want to denote, how can we find the hydro knee um concentration. So we can remember or recall that the hydrogen concentration is equal to 10 raised to the negative ph And so when we do this we have 10 raised to the negative ph or in other words negative 1.1. And this gives us a hydrogen concentration of 0.794 moller. And since hcl is a very strong acid, our hydrogen concentration is equal to how much a cl hcl that we have. And so the reaction equation in the situation here is CAC 03, a solid. And we're adding two equivalents of hcl in the acquis form. And this is going to give us a C a C. L. To acquis plus water in a liquid form of course plus C. +02 gas. And so now we have to determine the volume of hcl total. And so before we do that, we wanted to note that the molar mass of C a c 03 is 100.9 g per moller. And so to find the volume of Rh ceo. So to find the volume of hcl, we're going to take how many grams of C a c 03 that we have, which is 1.15 g. And then we're going to use the molar mass conversion factor. We're going to say one mole of this. C a C 03 is equal to 100. g. And then we're going to multiply by the multiple ratio. And we're going to say that for every one mole of c a c 03, we have two moles of H C L. Then we are going to say that for every 0.0794 moles of Hcl, we have one leader of hcl And then of course we have to convert to middle leaders. And by doing that, we say that for every one middle leader, we have 10 to the negative third leaders of Hcl. And once our units cancel out, we're going to end up with 289 mL as our volume. The other solution I stated in the question is 350 middle leaders. And so therefore it cannot be completely neutralized. Right? So therefore the fraction. So the fraction That is neutralized can be found by simply taking the 289 ml and dividing that by the 350 ml sample to give us 0.8-6 ml. And that is our final answer. I hope this helped until next time.

Ch.17 - Acids and Bases

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Tro 6th Edition

Ch.17 - Acids and Bases

Problem 135

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Chapter 17, Problem 135

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?

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Calculate the moles of Mg(OH)_2 in the recommended dose using its molar mass.

Write the balanced chemical equation for the neutralization reaction: Mg(OH)_2 + 2HCl -> MgCl_2 + 2H_2O.

Determine the moles of HCl that can be neutralized by the moles of Mg(OH)_2 using the stoichiometry from the balanced equation.

Calculate the concentration of HCl from the given pH using the formula: [H^+] = 10^{-pH}.

Determine the volume of HCl solution that can be neutralized by the moles of HCl calculated, and compare it to the given volume of stomach acid to find the fraction neutralized.

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Key Concepts

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

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, magnesium hydroxide (Mg(OH)2) acts as a base that neutralizes hydrochloric acid (HCl). The balanced chemical equation for this reaction is Mg(OH)2 + 2HCl → MgCl2 + 2H2O, which illustrates how the acid and base interact to reduce acidity.

pH and Concentration

pH is a measure of the hydrogen ion concentration in a solution, indicating its acidity or basicity. A pH of 1.3 corresponds to a high concentration of H+ ions, specifically 0.050 M HCl. Understanding pH is crucial for calculating how much acid can be neutralized by a given amount of base, as it directly relates to the concentration of the acid present in the solution.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on their molar ratios. In this scenario, stoichiometry is used to determine how many moles of HCl can be neutralized by the available moles of Mg(OH)2 from the milk of magnesia. This concept is essential for quantifying the extent of the neutralization and assessing whether all the acid in the stomach can be neutralized.

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