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Chapter 4: Problem 25

Calcium chloride is a strong electrolyte and is used to "salt" streets in the winter to melt ice and snow. Write a reaction to show how this substance breaks apart when it dissolves in water.

Short Answer

Expert verified
The dissolution of calcium chloride (CaCl₂) in water can be represented by the balanced chemical equation: \[ CaCl_{2}(s) \xrightarrow{H_2O} Ca^{2+}(aq) + 2Cl^-(aq) \] This equation shows the solid calcium chloride dissociating into its ions, calcium (Ca²⁺) and chloride (Cl⁻), in an aqueous solution.

Step by step solution

01

Understanding electrolytes

An electrolyte is a substance that produces ions when dissolved in water. These ions allow the solution to conduct electricity. In this case, calcium chloride is a strong electrolyte, which means it completely dissociates into its ions when dissolved in water.
02

Identifying the components of calcium chloride

Calcium chloride is made up of calcium ions (Ca²⁺) and chloride ions (Cl⁻). The chemical formula for calcium chloride is CaCl₂. This indicates that one calcium ion combines with two chloride ions to form one formula unit of calcium chloride.
03

Writing the balanced chemical equation for dissolution

Now, we can write the balanced chemical equation that shows the dissolution of calcium chloride in water. To do this, we will represent the reactants (calcium chloride and water) and the products (calcium ions and chloride ions) in the form of a balanced equation: \[ CaCl_{2}(s) \xrightarrow{H_2O} Ca^{2+}(aq) + 2Cl^-(aq) \] Here, "(s)" denotes the solid state of calcium chloride, "(aq)" indicates the aqueous state of the ions, and "H₂O" in the arrow represents the solvent in which the dissolution occurs. The balanced equation shows that one formula unit of calcium chloride dissociates into one calcium ion and two chloride ions when dissolved in water.

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Most popular questions from this chapter

Assign oxidation states for all atoms in each of the following compounds. a. \(\mathrm{UO}_{2}^{2+}\) b. \(\mathrm{As}_{2} \mathrm{O}_{3}\) c. \(\mathrm{NaBiO}_{3}\) d. As \(_{4}\) e. \(\mathrm{HAsO}_{2}\) f. \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7}\) g. \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) h. \(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\) i. \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\)

A \(10.00-\mathrm{g}\) sample consisting of a mixture of sodium chloride and potassium sulfate is dissolved in water. This aqueous mixture then reacts with excess aqueous lead(II) nitrate to form \(21.75 \mathrm{~g}\) of solid. Determine the mass percent of sodium chloride in the original mixture.

Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. a. \(0.100\) mole of \(\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}\) in \(100.0 \mathrm{~mL}\) of solution b. \(2.5\) moles of \(\mathrm{Na}_{2} \mathrm{SO}_{4}\) in \(1.25 \mathrm{~L}\) of solution c. \(5.00 \mathrm{~g}\) of \(\mathrm{NH}_{4} \mathrm{Cl}\) in \(500.0 \mathrm{~mL}\) of solution d. \(1.00 \mathrm{~g} \mathrm{~K}_{2} \mathrm{PO}_{4}\) in \(250.0 \mathrm{~mL}\) of solution

The unknown acid \(\mathrm{H}_{2} \mathrm{X}\) can be neutralized completely by \(\mathrm{OH}^{-}\) according to the following (unbalanced) equation: $$ \mathrm{H}_{2} \mathrm{X}(a q)+\mathrm{OH}^{-}(a q) \longrightarrow \mathrm{X}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(l) $$ The ion formed as a product, \(\mathrm{X}^{2-}\), was shown to have 36 total electrons. What is element \(\mathrm{X}\) ? Propose a name for \(\mathrm{H}_{2} \mathrm{X}\). To completely neutralize a sample of \(\mathrm{H}_{2} \mathrm{X}, 35.6 \mathrm{~mL}\) of \(0.175 \mathrm{M}\) \(\mathrm{OH}^{-}\) solution was required. What was the mass of the \(\mathrm{H}_{2} \mathrm{X}\) sample used?

A \(10.00-\mathrm{mL}\) sample of vinegar, an aqueous solution of acetic acid \(\left(\mathrm{HC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\right)\), is titrated with \(0.5062 \mathrm{M} \mathrm{NaOH}\), and \(16.58 \mathrm{~mL}\) is required to reach the equivalence point. a. What is the molarity of the acetic acid? b. If the density of the vinegar is \(1.006 \mathrm{~g} / \mathrm{cm}^{3}\), what is the mass percent of acetic acid in the vinegar?
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