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Chapter 5: Problem 10

A solution is \(0.126 \mathrm{M} \mathrm{KCl}\) and \(0.148 \mathrm{M} \mathrm{MgCl}_{2} .\) What are \(\left[\mathrm{K}^{+}\right],\left[\mathrm{Mg}^{2+}\right],\) and \(\left[\mathrm{Cl}^{-}\right]\) in this solution?

Short Answer

Expert verified
The concentrations of the ions in the solution are: [K+] = 0.126 M, [Mg2+] = 0.148 M, [Cl-] = 0.422 M.

Step by step solution

01

Identify the ions and their ratios

When KCl is dissolved in water, it dissociates into K+ and Cl- ions in a 1:1 ratio. Therefore, the concentration of each ion will be equal to the molarity of KCl. Similarly, when MgCl2 is dissolved, it dissociates into Mg2+ ions and Cl- ions but in a 1:2 ratio because there are 2 chloride ions for each magnesium ion. This means that the concentration of Cl- ions from the MgCl2 will be twice the molarity of MgCl2.
02

Calculate the concentration of K+ and Mg2+ ions

Given that the solution is 0.126 M KCl and 0.148 M MgCl2, the concentration of K+ ions will be 0.126 M while the concentration of Mg2+ ions will be 0.148 M.
03

Calculate the concentration of Cl- ions

The concentration of Cl- ions will be the sum of the concentration of Cl- from KCl and twice the concentration from MgCl2 since it dissociates into two Cl- ions. Therefore, the concentration of Cl- ions will be 0.126 M + 2*0.148 M = 0.422 M.

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Most popular questions from this chapter

What are the oxidizing and reducing agents in the following redox reactions? (a) \(5 \mathrm{SO}_{3}^{2-}+2 \mathrm{MnO}_{4}^{-}+6 \mathrm{H}^{+} \longrightarrow\) \(5 \mathrm{SO}_{4}^{2-}+2 \mathrm{Mn}^{2+}+3 \mathrm{H}_{2} \mathrm{O}\) (b) \(2 \mathrm{NO}_{2}(\mathrm{g})+7 \mathrm{H}_{2}(\mathrm{g}) \longrightarrow 2 \mathrm{NH}_{3}(\mathrm{g})+4 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})\) (c) \(2\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{4-}+\mathrm{H}_{2} \mathrm{O}_{2}+2 \mathrm{H}^{+} \longrightarrow\) \(2\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]^{3-}+2 \mathrm{H}_{2} \mathrm{O}\)

A compound contains only Fe and O. A \(0.2729 \mathrm{g}\) sample of the compound was dissolved in \(50 \mathrm{mL}\) of concentrated acid solution, reducing all the iron to \(\mathrm{Fe}^{2+}\) ions. The resulting solution was diluted to \(100 \mathrm{mL}\) and then titrated with a \(0.01621 \mathrm{M} \mathrm{KMnO}_{4}\) solution. The unbalanced chemical equation for reaction between \(\mathrm{Fe}^{2+}\) and \(\mathrm{MnO}_{4}^{-}\) is given below. \(\begin{aligned} \mathrm{MnO}_{4}^{-}(\mathrm{aq})+& \mathrm{Fe}^{2+}(\mathrm{aq}) \longrightarrow \mathrm{Mn}^{2+}(\mathrm{aq})+\mathrm{Fe}^{3+}(\mathrm{aq}) \quad(\text { not balanced }) \end{aligned}\) The titration required \(42.17 \mathrm{mL}\) of the \(\mathrm{KMnO}_{4}\) solution to reach the pink endpoint. What is the empirical formula of the compound?

Select the (a) best and (b) poorest electrical conductors from the following solutions, and explain the reason for your choices: \(0.10 \mathrm{M} \mathrm{NH}_{3} ; 0.10 \mathrm{M} \mathrm{NaCl} ; 0.10 \mathrm{M}\) \(\mathrm{CH}_{3} \mathrm{COOH}\) (acetic acid); \(0.10 \mathrm{M} \mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}\) (ethanol).

A neutralization reaction between an acid and a base is a common method of preparing useful salts. Give net ionic equations showing how the following salts could be prepared in this way: (a) \(\left(\mathrm{NH}_{4}\right)_{2} \mathrm{HPO}_{4};\) (b) \(\mathrm{NH}_{4} \mathrm{NO}_{3} ;\) and \((\mathrm{c})\left(\mathrm{NH}_{4}\right)_{2} \mathrm{SO}_{4}\).

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