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Chapter 4: Problem 31

Which of the following solutions of strong electrolytes contains the largest number of moles of chloride ions: \(100.0 \mathrm{~mL}\) of \(0.30 \mathrm{M} \mathrm{AlCl}_{3}, 50.0 \mathrm{~mL}\) of \(0.60 \mathrm{M} \mathrm{MgCl}_{2}\), or \(200.0 \mathrm{~mL}\) of \(0.40 \mathrm{M} \mathrm{NaCl} ?\)

Short Answer

Expert verified
The 100.0 mL of 0.30 M AlCl3 solution has the largest number of moles of chloride ions with 0.09 mol.

Step by step solution

01

Analyzing each solution

For each of the three solutions, we need to find the number of moles of chloride ions: 1. AlCl3: This compound has 3 chloride ions for each aluminum ion (3 Cl- ions for each formula unit). 2. MgCl2: This compound has 2 chloride ions for each magnesium ion (2 Cl- ions for each formula unit). 3. NaCl: This compound has 1 chloride ion for each sodium ion (1 Cl- ion for each formula unit).
02

Calculate moles of Cl- ions in each solution

Now, we need to calculate the moles of chloride ions in all of the solutions: 1. For AlCl3 solution: Moles of AlCl3 = Volume (L) 脳 Molarity Moles of AlCl3 = \( 100.0 \times 10^{-3}L \times 0.30M \) Moles of AlCl3 = \( 0.03 mol \) Moles of Cl- ions = Moles of AlCl3 脳 Number of Cl- ions in AlCl3 Moles of Cl- ions = \( 0.03 mol \times 3 \) Moles of Cl- ions = \( 0.09 mol \) 2. For MgCl2 solution Moles of MgCl2 = Volume (L) 脳 Molarity Moles of MgCl2 = \( 50.0 \times 10^{-3} L \times 0.60 M \) Moles of MgCl2 = \( 0.03 mol \) Moles of Cl- ions = Moles of MgCl2 脳 Number of Cl- ions in MgCl2 Moles of Cl- ions = \( 0.03 mol \times 2 \) Moles of Cl- ions = \( 0.06 mol \) 3. For NaCl solution Moles of NaCl = Volume (L) 脳 Molarity Moles of NaCl = \( 200.0 \times 10^{-3} L \times 0.40 M \) Moles of NaCl = \( 0.08 mol \) Moles of Cl- ions = Moles of NaCl 脳 Number of Cl- ions in NaCl Moles of Cl- ions = \( 0.08 mol \times 1 \) Moles of Cl- ions = \( 0.08 mol \)
03

Compare the moles of Cl- ions in each solution

Now let's compare the moles of chloride ions in each solution: 1. AlCl3 solution: \( 0.09 \ mol \) of Cl- ions 2. MgCl2 solution: \( 0.06 \ mol \) of Cl- ions 3. NaCl solution: \( 0.08 \ mol \) of Cl- ions From the comparison, we can conclude that the 100.0 mL of 0.30 M AlCl3 solution has the largest number of moles of chloride ions with 0.09 mol.

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Most popular questions from this chapter

Consider reacting copper(II) sulfate with iron. Two possible reactions can occur, as represented by the following equations. copper(II) sulfate \((a q)+\operatorname{iron}(s)\) $$ \operatorname{copper}(s)+\text { iron(II) sulfate }(a q) $$ \(\operatorname{copper}(\) II \()\) sulfate \((a q)+\operatorname{iron}(s)\) $$ \operatorname{copper}(s)+\text { iron(III) sulfate }(a q) $$ You place \(87.7 \mathrm{~mL}\) of a \(0.500 M\) solution of copper(II) sulfate in a beaker. You then add \(2.00 \mathrm{~g}\) of iron filings to the copper(II) sulfate solution. After one of the above reactions occurs, you isolate \(2.27 \mathrm{~g}\) of copper. Which equation above describes the reaction that occurred? Support your answer.

A student titrates an unknown amount of potassium hydrogen phthalate \(\left(\mathrm{KHC}_{8} \mathrm{H}_{4} \mathrm{O}_{4}\right.\), often abbreviated \(\mathrm{KHP}\) ) with \(20.46 \mathrm{~mL}\) of a \(0.1000 M\) NaOH solution. KHP (molar mass \(=204.22\) \(\mathrm{g} / \mathrm{mol}\) ) has one acidic hydrogen. What mass of KHP was titrated (reacted completely) by the sodium hydroxide solution?

The concentration of a certain sodium hydroxide solution was determined by using the solution to titrate a sample of potassium hydrogen phthalate (abbreviated as KHP). KHP is an acid with one acidic hydrogen and a molar mass of \(204.22 \mathrm{~g} / \mathrm{mol}\). In the titration, \(34.67 \mathrm{~mL}\) of the sodium hydroxide solution was required to react with \(0.1082\) g KHP. Calculate the molarity of the sodium hydroxide.

Some of the substances commonly used in stomach antacids are \(\mathrm{MgO}, \mathrm{Mg}(\mathrm{OH})_{2}\), and \(\mathrm{Al}(\mathrm{OH})_{3}\) a. Write a balanced equation for the neutralization of hydrochloric acid by each of these substances. b. Which of these substances will neutralize the greatest amount of \(0.10 \mathrm{M} \mathrm{HCl}\) per gram?

The drawings below represent aqueous solutions. Solution A is \(2.00 \mathrm{~L}\) of a \(2.00 \mathrm{M}\) aqueous solution of copper(II) nitrate. Solution \(\mathrm{B}\) is \(2.00 \mathrm{~L}\) of a \(3.00 \mathrm{M}\) aqueous solution of potassium hydroxide. a. Draw a picture of the solution made by mixing solutions \(\mathrm{A}\) and \(\mathrm{B}\) together after the precipitation reaction takes place. Make sure this picture shows the correct relative volume compared to solutions \(\mathrm{A}\) and \(\mathrm{B}\), and the correct relative number of ions, along with the correct relative amount of solid formed. b. Determine the concentrations (in \(M\) ) of all ions left in solution (from part a) and the mass of solid formed.
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