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Chapter 14: Problem 119

Complete and balance each of the following: (14.7) a. \(\mathrm{HCl}(a q)+\mathrm{LiOH}(s) \longrightarrow\) b. \(\mathrm{MgCO}_{3}(s)+\mathrm{H}_{2} \mathrm{SO}_{4}(a q) \longrightarrow\)

Short Answer

Expert verified
a. \( \mathrm{HCl} + \mathrm{LiOH} \longrightarrow \mathrm{LiCl} + \mathrm{H}_{2}\mathrm{O} \) b. \( \mathrm{MgCO}_{3} + \mathrm{H}_{2}\mathrm{SO}_{4} \longrightarrow \mathrm{MgSO}_{4} + \mathrm{H}_{2}\mathrm{O} + \mathrm{CO}_{2} \)

Step by step solution

01

Identify the Reactants

Identify the reactants given in the chemical equation. For part (a), the reactants are \( \mathrm{HCl}(aq) \) and \( \mathrm{LiOH}(s) \). For part (b), the reactants are \( \mathrm{MgCO}_{3}(s) \) and \( \mathrm{H}_{2}\mathrm{SO}_{4}(aq) \).
02

Predict the Products

Predict the products of the reaction. For part (a), \( \mathrm{HCl} \) and \( \mathrm{LiOH} \) react to form \( \mathrm{LiCl} \) and \( \mathrm{H}_{2}\mathrm{O} \). For part (b), \( \mathrm{MgCO}_{3} \) and \( \mathrm{H}_{2}\mathrm{SO}_{4} \) produce \( \mathrm{MgSO}_{4} \), \( \mathrm{H}_{2}\mathrm{O} \) and \( \mathrm{CO}_{2} \).
03

Write the Unbalanced Equations

Write the unbalanced chemical equations for both reactions: a. \( \mathrm{HCl}(aq) + \mathrm{LiOH}(s) \longrightarrow \mathrm{LiCl} + \mathrm{H}_{2}\mathrm{O} \) b. \( \mathrm{MgCO}_{3}(s) + \mathrm{H}_{2}\mathrm{SO}_{4}(aq) \longrightarrow \mathrm{MgSO}_{4} + \mathrm{H}_{2}\mathrm{O} + \mathrm{CO}_{2} \)
04

Balance the Equations

Ensure that the number of atoms for each element is the same on both sides of the equations. a. The equation for part (a) is already balanced as is: \( \mathrm{HCl}(aq) + \mathrm{LiOH}(s) \longrightarrow \mathrm{LiCl} + \mathrm{H}_{2}\mathrm{O} \) b. The equation for part (b) is also balanced correctly: \( \mathrm{MgCO}_{3}(s) + \mathrm{H}_{2}\mathrm{SO}_{4}(aq) \longrightarrow \mathrm{MgSO}_{4} + \mathrm{H}_{2}\mathrm{O} + \mathrm{CO}_{2} \)

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Key Concepts

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

Chemical Reactions
Chemical reactions are processes where substances (reactants) transform into new substances (products). These changes at the molecular level involve the making and breaking of chemical bonds. For example, when hydrogen and oxygen react, they form water鈥攁 completely new substance. Chemical reactions can be classified in many ways, such as synthesis, decomposition, single replacement, double replacement, and combustion. Each type of reaction behaves in a predictable way, helping chemists understand and control chemical processes.
Reactants and Products
In a chemical reaction, starting materials are called reactants, while the substances formed are called products. For instance, in the reaction between hydrochloric acid (HCl) and lithium hydroxide (LiOH), these two compounds are the reactants. The resulting compounds鈥攍ithium chloride (LiCl) and water (H鈧侽)鈥攁re the products. Recognizing reactants and predicting the products are crucial steps in solving chemical equations. Remember, a chemical equation must always be balanced, meaning the number of atoms for each element is the same on both sides of the equation.
Stoichiometry
Stoichiometry is the calculation of reactants and products in chemical reactions. Using balanced chemical equations, stoichiometry allows chemists to determine the proportions of elements involved. It's like a recipe that tells you how much of each ingredient you need and how much product you鈥檒l get. For instance, in the reaction of magnesium carbonate (MgCO鈧�) with sulfuric acid (H鈧係O鈧�), the equation: MgCO鈧�(s) + H鈧係O鈧�(aq) 鈫� MgSO鈧� + H鈧侽 + CO鈧� tells us that one molecule of MgCO鈧� reacts with one molecule of H鈧係O鈧� to produce one molecule of MgSO鈧�, one molecule of H鈧侽, and one molecule of CO鈧�.
Acid-Base Reactions
Acid-base reactions occur when an acid reacts with a base to produce water and a salt. These reactions are also known as neutralization reactions. For example, in the reaction of hydrochloric acid (HCl) with lithium hydroxide (LiOH): HCl(aq) + LiOH(s) 鈫� LiCl + H鈧侽 HCl (the acid) donates a proton (H鈦�) to LiOH (the base), resulting in the formation of water (H鈧侽) and lithium chloride (LiCl). Understanding acid-base reactions is important for fields like chemistry, biology, environmental science, and medicine.
Precipitation Reactions
Precipitation reactions happen when two aqueous solutions react to form an insoluble solid called a precipitate. This solid separates from the solution. For example, if we mix solutions of silver nitrate (AgNO鈧�) and sodium chloride (NaCl), silver chloride (AgCl) precipitates out as a solid: AgNO鈧�(aq) + NaCl(aq) 鈫� AgCl(s) + NaNO鈧�(aq) The solid AgCl appears as a white, cloudy substance in the solution. Precipitation reactions are useful in various processes like wastewater treatment, mineral extraction, and in many laboratory procedures to isolate specific compounds.

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Most popular questions from this chapter

Balance each of the following neutralization reactions: a. \(\mathrm{HCl}(a q)+\mathrm{Mg}(\mathrm{OH})_{2}(s) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{MgCl}_{2}(a q)\) b. \(\mathrm{H}_{3} \mathrm{PO}_{4}(a q)+\mathrm{LiOH}(a q) \longrightarrow \mathrm{H}_{2} \mathrm{O}(l)+\mathrm{Li}_{3} \mathrm{PO}_{4}(a q)\)

Consider the buffer system of hydrofluoric acid, HF, and its salt, NaF. $$ \mathrm{HF}(a q)+\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}_{3} \mathrm{O}^{+}(a q)+\mathrm{F}^{-}(a q) $$ a. The purpose of this buffer system is to: 1\. maintain [HF] 2\. maintain [F ] 3\. maintain \(\mathrm{pH}\) b. The salt of the weak acid is needed to: 1\. provide the conjugate base 2\. neutralize added \(\mathrm{H}_{3} \mathrm{O}^{+}\) 3\. provide the conjugate acid c. If \(\mathrm{OH}^{-}\) is added, it is neutralized by: 1\. the salt 2\. \(\mathrm{H}_{2} \mathrm{O}\) 3\. \(\mathrm{H}_{3} \mathrm{O}^{+}\) d. When \(\mathrm{H}_{3} \mathrm{O}^{+}\) is added, the equilibrium shifts in the direction of the: 1\. reactants 2\. products 3\. does not change

If a base is added to pure water, why does the \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) decrease?

Determine each of the following for a \(0.025 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) solution: \((14.6,14.7,14.8)\) a. \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) b. \(\mathrm{pH}\) c. \(\mathrm{pOH}\) d. \(\left[\mathrm{OH}^{-}\right]\) e. the balanced equation for the reaction with \(\mathrm{CsOH}\)

A solution with a pH of 10 is 100 times more basic than a solution with \(\mathrm{pH}\) 8. Explain.
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