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Chapter 4: Problem 7

Consider separate aqueous solutions of \(\mathrm{HCl}\) and \(\mathrm{H}_{2} \mathrm{SO}_{4}\) with the same molar concentrations. You wish to neutralize an aqueous solution of \(\mathrm{NaOH}\). For which acid solution would you need to add more volume (in milliliters) to neutralize the base? a. the \(\mathrm{HCl}\) solution b. the \(\mathrm{H}_{2} \mathrm{SO}_{4}\) solution c. You need to know the acid concentrations to answer this question. d. You need to know the volume and concentration of the \(\mathrm{NaOH}\) solution to answer this question. e. \(c\) and \(\underline{d}\) Explain.

Short Answer

Expert verified
a. the \(\mathrm{HCl}\) solution

Step by step solution

01

Write balanced chemical equations for both reactions

We first need to write down the balanced chemical reactions for the neutralization of the sodium hydroxide solution by both \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\). These are: a. \(\mathrm{HCl} + \mathrm{NaOH} \rightarrow \mathrm{NaCl} + \mathrm{H}_{2}\mathrm{O}\) b. \(\mathrm{H}_{2}\mathrm{SO}_{4} + 2\mathrm{NaOH} \rightarrow \mathrm{Na}_{2}\mathrm{SO}_{4} + 2\mathrm{H}_{2}\mathrm{O}\)
02

Determine stoichiometric coefficients

Next, we identify the stoichiometric coefficients of the reactants in the balanced equations. We will consider the coefficients of \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\) in their respective reactions: a. In the \(\mathrm{HCl}\) reaction, there is a 1:1 ratio between \(\mathrm{HCl}\) and \(\mathrm{NaOH}\). It means one mole of \(\mathrm{HCl}\) reacts with one mole of \(\mathrm{NaOH}\). b. In the \(\mathrm{H}_{2}\mathrm{SO}_{4}\) reaction, there is a 1:2 ratio between \(\mathrm{H}_{2}\mathrm{SO}_{4}\) and \(\mathrm{NaOH}\). It means one mole of \(\mathrm{H}_{2}\mathrm{SO}_{4}\) reacts with two moles of \(\mathrm{NaOH}\).
03

Compare volumes of acid solutions needed for neutralization

Since the molar concentrations of \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\) solutions are the same, we can use the stoichiometric coefficients to compare the volumes required to neutralize the base: a. In the case of \(\mathrm{HCl}\), one mole of acid is needed to neutralize one mole of base. b. In the case of \(\mathrm{H}_{2}\mathrm{SO}_{4}\), one mole of acid is needed to neutralize two moles of base (twice as much base). Using this information, we can conclude that we would need to add more volume of the \(\mathrm{HCl}\) solution to neutralize the base, as it reacts with the base in a 1:1 ratio. On the other hand, since \(\mathrm{H}_{2}\mathrm{SO}_{4}\) reacts with twice as much base as \(\mathrm{HCl}\) in a 1:2 ratio, less volume of \(\mathrm{H}_{2}\mathrm{SO}_{4}\) solution is required to neutralize the same amount of base. So, the correct answer is a. the \(\mathrm{HCl}\) solution.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Stoichiometry
Stoichiometry is an essential concept in chemistry that helps us understand the quantitative relationships between the reactants and products in a chemical reaction. It involves using the balanced chemical equation to calculate the amount of each substance required or produced.

By analyzing the stoichiometric coefficients鈥攖he numbers in front of molecules in a balanced equation鈥攚e can figure out the proportions of reactants needed and products formed. For instance, in an acid-base reaction, these coefficients help determine how much acid is needed to completely neutralize a given volume of base.

Understanding stoichiometry allows us to tackle a wide range of problems, from finding the quantities of substances involved in reactions to making predictions about the yields of chemical processes.
Balanced Chemical Equation
A balanced chemical equation is crucial because it ensures that the law of conservation of mass is followed鈥攎eaning matter is neither created nor destroyed during a chemical reaction. This involves adjusting the coefficients in front of chemical formulas to make sure that the number of atoms for each element is the same on both sides of the equation.

For example, when hydrochloric acid (\(\mathrm{HCl}\)) reacts with sodium hydroxide (\(\mathrm{NaOH}\)), the balanced chemical equation is: \(\mathrm{HCl} + \mathrm{NaOH} \rightarrow \mathrm{NaCl} + \mathrm{H}_{2}\mathrm{O}\).

In this reaction, one mole of \(\mathrm{HCl}\) reacts with one mole of \(\mathrm{NaOH}\) to produce one mole of sodium chloride and water.

For sulfuric acid (\(\mathrm{H}_{2}\mathrm{SO}_{4}\)), the equation is: \(\mathrm{H}_{2}\mathrm{SO}_{4} + 2\mathrm{NaOH} \rightarrow \mathrm{Na}_{2}\mathrm{SO}_{4} + 2\mathrm{H}_{2}\mathrm{O}\). This shows that one mole of \(\mathrm{H}_{2}\mathrm{SO}_{4}\) can react with two moles of \(\mathrm{NaOH}\) to form different products.

Properly balanced equations are essential for making accurate calculations in stoichiometry and understanding reaction dynamics.
Molarity
Molarity is a way to express concentration, specifically the concentration of a solution. It鈥檚 defined as the number of moles of a solute per liter of solution and is often represented by the symbol \(M\).

Knowing the molarity of an acid solution, like \(\mathrm{HCl}\) or \(\mathrm{H}_{2}\mathrm{SO}_{4}\), helps us determine how many moles of the acid are present in a given volume of the solution.

The concentration of these solutions is crucial for calculating the correct volume needed during a neutralization reaction. The more precise the molarity, the more accurately we can predict how much of the acid is needed to react with a base.
  • Formula for molarity: \(M = \frac{\text{moles of solute}}{\text{liters of solution}}\).
  • This concept helps us relate the stoichiometry of reactions directly to the practical measurements taken in the lab.
Understanding molarity is fundamental in preparing solutions and determining their strengths in laboratory settings.
HCl vs H2SO4 Neutralization
Neutralization is a chemical reaction in which an acid and a base react to form water and, often, a salt. In the context of \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\), this process varies due to their different chemical properties and stoichiometric ratios.

Hydrochloric acid (\(\mathrm{HCl}\)) neutralizes sodium hydroxide (\(\mathrm{NaOH}\)) in a simple 1:1 molar ratio, meaning one mole of \(\mathrm{HCl}\) reacts with one mole of \(\mathrm{NaOH}\).

Sulfuric acid (\(\mathrm{H}_{2}\mathrm{SO}_{4}\)), however, reacts differently, with a 1:2 molar ratio. One mole of \(\mathrm{H}_{2}\mathrm{SO}_{4}\) has the ability to neutralize two moles of \(\mathrm{NaOH}\). Thus, if both \(\mathrm{HCl}\) and \(\mathrm{H}_{2}\mathrm{SO}_{4}\) are present at the same molarity, it will take less sulfuric acid to neutralize the same amount of sodium hydroxide.

This illustrates why \(\mathrm{H}_{2}\mathrm{SO}_{4}\) is often considered a more potent acid per mole compared to \(\mathrm{HCl}\) in neutralization reactions: it can neutralize more base per mole of acid.

Understanding these differences helps in choosing the correct acid for chemical processes requiring specific neutralization capacities.

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Most popular questions from this chapter

Saccharin \(\left(\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{NO}_{3} \mathrm{~S}\right)\) is sometimes dispensed in tablet form. Ten tablets with a total mass of \(0.5894 \mathrm{~g}\) were dissolved in water. The saccharin was oxidized to convert all the sulfur to sulfate ion, which was precipitated by adding an excess of barium chloride solution. The mass of \(\mathrm{BaSO}_{4}\) obtained was \(0.5032 \mathrm{~g}\). What is the average mass of saccharin per tablet? What is the average mass percent of saccharin in the tablets?

What volume of \(0.0200 M\) calcium hydroxide is required to neutralize \(35.00 \mathrm{~mL}\) of \(0.0500 M\) nitric acid?

How would you prepare \(1.00 \mathrm{~L}\) of a \(0.50 M\) solution of each of the following? a. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) from "concentrated" \((18 M)\) sulfuric acid b. \(\mathrm{HCl}\) from "concentrated" \((12 \mathrm{M})\) reagent c. \(\mathrm{NiCl}_{2}\) from the salt \(\mathrm{NiCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) d. HNO \(_{3}\) from "concentrated" (16 M) reagent e. Sodium carbonate from the pure solid

Zinc and magnesium metal each react with hydrochloric acid according to the following equations: $$ \begin{array}{l} \mathrm{Zn}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{ZnCl}_{2}(a q)+\mathrm{H}_{2}(g) \\ \mathrm{Mg}(s)+2 \mathrm{HCl}(a q) \longrightarrow \mathrm{MgCl}_{2}(a q)+\mathrm{H}_{2}(g) \end{array} $$ A \(10.00-\mathrm{g}\) mixture of zinc and magnesium is reacted with the stoichiometric amount of hydrochloric acid. The reaction mixture is then reacted with \(156 \mathrm{~mL}\) of \(3.00 M\) silver nitrate to produce the maximum possible amount of silver chloride. a. Determine the percent magnesium by mass in the original mixture. b. If \(78.0 \mathrm{~mL}\) of \(\mathrm{HCl}\) was added, what was the concentration of the \(\mathrm{HCl}\) ?

A stock solution containing \(\mathrm{Mn}^{2+}\) ions was prepared by dissolving \(1.584 \mathrm{~g}\) pure manganese metal in nitric acid and diluting to a final volume of \(1.000 \mathrm{~L}\). The following solutions were then prepared by dilution: For solution A. \(50.00 \mathrm{~mL}\) of stock solution was diluted to \(1000.0 \mathrm{~mL}\) For solution \(B, 10.00 \mathrm{~mL}\) of solution \(A\) was diluted to \(250.0 \mathrm{~mL}\). For solution \(C, 10.00 \mathrm{~mL}\) of solution \(B\) was diluted to \(500.0 \mathrm{~mL}\). Calculate the concentrations of the stock solution and solutions \(A, B\), and \(C\).
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