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Chapter 8: Problem 11

Evaporating ocean water leaves a mixture of salts. Is this a chemical change? Explain.

Short Answer

Expert verified
No, the evaporation of ocean water leaving a mixture of salts is not a chemical change. It is a physical change because the water and the salt retain their chemical identities throughout the process.

Step by step solution

01

Define Chemical Change

Initially, define what constitutes a chemical change. A chemical change, also known as a chemical reaction, involves a process that transforms one or more substances into new substances. These changes are commonly associated with changes in the chemical identity of the substances involved.
02

Evaluate the Given Scenario

Next, examine the process in question, which is the evaporation of ocean water leaving behind a mixture of salts. When water evaporates, it changes from a liquid state to a gaseous state. The salt, which was dissolved in the water, is left behind. Both the water and the salt retain their chemical identities throughout this process, even though the physical state of the water changes.
03

Conclude Based on Understanding

Finally, it can be concluded that the evaporation of ocean water leaving a mixture of salts is not a chemical change. This is because neither the water nor the salt undergo a transformation into new substances. They remain chemically the same before and after the evaporation process, despite the physical change of state in the water.

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Most popular questions from this chapter

Graphing Calculator Least Common Multiples When writing chemical formulas or balancing a chemical equation, being able to identify the least com- mon multiple of a set of numbers can often help. Your graphing calculator has a least common multiple function that can compare two numbers. On a TI-83 Plus or similar graphing calculator, press MATH 8 . The screen should read "lcm(." Next, enter one number and then a comma followed by the other number and a closing parenthesis. Press ENTER, and the calculator will show the least common multiple of the pair you entered. Use this function as needed to find the answers to the following questions. $$\begin{array}{l}{\text { a. Tin(IV) sulfate contains } \mathrm{Sn}^{4+} \text { and } \mathrm{SO}_{4}^{2-}} \\ {\text { ions. Use the least common multiple of } 2} \\ {\text { and } 4 \text { to determine the empirical formula }} \\ {\text { for this compound. }}\end{array}$$ $$ \begin{array}{l}{\text { b. Aluminum ferrocyanide contains } \mathrm{Al}^{3+} \text { ions }} \\ {\text { and } \mathrm{Fe}(\mathrm{CN})_{6}^{4} \text { ions. Use the least common }} \\ {\text { multiple of } 3 \text { and } 4 \text { to determine the empiri- }} \\ {\text { cal formula for this compound. }}\end{array} $$ $$\text{c. Balance the following unbalanced equation}.$$$$ \text{___}\mathrm{P}_{4} \mathrm{O}_{10}(s)+\text{___}\mathrm{H}_{2} \mathrm{O}(g) \rightarrow\text{___}\mathrm{H}_{3} \mathrm{PO}_{4}(a q)$$ $$\text{d. Balance the following unbalanced equation}.$$ $$ \text{___}\mathrm{KMnO}_{4}(a q)+\text{___}\mathrm{MnCl}_{2}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\text{___}\mathrm{MnO}_{2}(s)+4 \mathrm{HCl}(a q)+2 \mathrm{KCl}(a q) $$

The following equations are incorrect in some way. Identify and correct each error, and then balance each equation. $$\begin{array}{l}{\text { a. } \mathrm{Li}+\mathrm{O}_{2} \rightarrow \mathrm{LiO}_{2}} \\ {\text { b. } \mathrm{MgCO}_{3} \rightarrow \mathrm{Mg}+\mathrm{C}+3 \mathrm{O}_{2}} \\ {\text { c. } \mathrm{NaI}+\mathrm{Cl}_{2} \rightarrow \mathrm{NaCl}+\mathrm{I}} \\ {\text { d. } \mathrm{AgNO}_{3}+\mathrm{CaCl}_{2} \rightarrow \mathrm{Ca}\left(\mathrm{NO}_{3}\right)+\mathrm{AgCl}_{2}} \\ {\text { e. } 3 \mathrm{Mg}+2 \mathrm{FeBr}_{3} \rightarrow \mathrm{Fe}_{2} \mathrm{Mg}_{3}+3 \mathrm{Br}_{2}}\end{array}$$

Predict the products for each of the following reactions. Write a total ionic equation and a net ionic equation for each reaction. If no reaction occurs, write "no reaction." $$\begin{array}{l}{\text { a. } \mathrm{Li}_{2} \mathrm{CO}_{3}(a q)+\mathrm{BaBr}_{2}(a q) \longrightarrow} \\ {\text { b. } \mathrm{Na}_{2} \mathrm{SO}_{4}(a q)+\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q) \rightarrow} \\ {\text { c. } \mathrm{Al}(s)+\mathrm{NiCl}_{2}(a q) \rightarrow} \\ {\text { d. } \mathrm{K}_{2} \mathrm{CO}_{3}(a q)+\mathrm{FeCl}_{3}(a q) \rightarrow}\end{array}$$

Balance the following equations. $$\text{a}. \mathrm{CaH}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow\mathrm{Ca}(\mathrm{OH})_{2}(a q)+\mathrm{H}_{2}(g)$$ $$\text{b}. \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CCH}(g)+\mathrm{Br}_{2}(l) \longrightarrow\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CBr}_{2} \mathrm{CHBr}_{2}(l)$$ $$\text{c} \cdot \mathrm{Pb}^{2+}(a q)+\mathrm{OH}^{-}(a q) \rightarrow \mathrm{Pb}(\mathrm{OH})_{2}(s)$$ $$\text{d} . \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \rightarrow \mathrm{HNO}_{3}(a q)+\mathrm{NO}(g)$$

Describe the relationship between a synthesis reaction and a decomposition reaction.
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