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Chapter 4: Problem 36

Which of the following solutions of strong electrolytes contains the largest number of ions: 100.0 \(\mathrm{mL}\) of 0.100\(M \mathrm{NaOH}\) , 50.0 \(\mathrm{mL}\) of \(0.200 \mathrm{M} \mathrm{BaCl}_{2},\) or 75.0 \(\mathrm{mL}\) of 0.150 \(\mathrm{M} \mathrm{Na}_{3} \mathrm{PO}_{4} ?\)

Short Answer

Expert verified
The solution containing the largest number of ions is 75.0 mL of 0.150 M Na3PO4, with a total of 0.0450 mol of ions.

Step by step solution

01

Determine moles of each electrolyte in the given solution

First, let's find the moles of each electrolyte in the solution. We can use the formula: Moles of electrolyte = Molarity × Volume (in liters) For the NaOH solution: Moles of NaOH = 0.100 M × 100.0 mL × (1L/1000mL) = 0.0100 mol For the BaCl2 solution: Moles of BaCl2 = 0.200 M × 50.0 mL × (1L/1000mL) = 0.0100 mol For the Na3PO4 solution: Moles of Na3PO4 = 0.150 M × 75.0 mL × (1L/1000mL) = 0.01125 mol
02

Identify ions produced by electrolytes and their corresponding numbers

When the strong electrolytes dissociate in water, they release their respective ions. Let's identify the ions produced by each electrolyte and their corresponding numbers. For NaOH: 1 Na⁺ ion and 1 OH⁻ ion Total ions = 1 + 1 = 2 For BaCl2: 1 Ba²⁺ ion and 2 Cl⁻ ions Total ions = 1 + 2 = 3 For Na3PO4: 3 Na⁺ ions and 1 PO₄³⁻ ion Total ions = 3 + 1 = 4
03

Calculate the total number of ions produced in each solution

Now that we have the moles of each electrolyte and the total ions produced per mole, we can calculate the total number of ions produced in each solution using the following formula: Total ions in solution = Moles of electrolyte × Total ions produced per mole of electrolyte For the NaOH solution: Total ions = 0.0100 mol × 2 = 0.0200 mol of ions For the BaCl2 solution: Total ions = 0.0100 mol × 3 = 0.0300 mol of ions For the Na3PO4 solution: Total ions = 0.01125 mol × 4 = 0.0450 mol of ions
04

Compare the total number of ions and determine the solution with the largest number of ions

Now that we have the total number of ions produced in each solution, let's compare them to find out which solution contains the largest number of ions. NaOH solution: 0.0200 mol of ions BaCl2 solution: 0.0300 mol of ions Na3PO4 solution: 0.0450 mol of ions We can see that the Na3PO4 solution contains the largest number of ions (0.0450 mol). Therefore, the solution containing the largest number of ions is 75.0 mL of 0.150 M Na3PO4.

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Most popular questions from this chapter

A sample may contain any or all of the following ions: \(\mathrm{Hg}_{2}^{2+}\) \(\mathrm{Ba}^{2+}\) and \(\mathrm{Mn}^{2+}\) a. No precipitate formed when an aqueous solution of NaCl was added to the sample solution. b. No precipitate formed when an aqueous solution of $\mathrm{Na}_{2} \mathrm{SO}_{4}$ was added to the sample solution. c. A precipitate formed when the sample solution was made basic with NaOH. Which ion or ions are present in the sample solution?

In the spectroscopic analysis of many substances, a series of standard solutions of known concentration are measured to generate a calibration curve. How would you prepare standard solutions containing 10.0, 25.0, 50.0, 75.0, and 100. ppm of copper from a commercially produced 1000.0-ppm solution? Assume each solution has a final volume of 100.0 mL. (See Exercise 135 for definitions.)

When organic compounds containing sulfur are bumed, sulfur dioxide is produced. The amount of \(\mathrm{SO}_{2}\) formed can be determined by the reaction with hydrogen peroxide: $$\mathrm{H}_{2} \mathrm{O}_{2}(a q)+\mathrm{SO}_{2}(g) \longrightarrow \mathrm{H}_{2} \mathrm{SO}_{4}(a q)$$ The resulting sulfuric acid is then titrated with a standard NaOH solution. A 1.302 -g sample of coal is burned and the \(\mathrm{SO}_{2}\) is collected in a solution of hydrogen peroxide. It took 28.44 \(\mathrm{mL}\) of a $0.1000-M \mathrm{NaOH}$ solution to titrate the resulting sulfuric acid. Calculate the mass percent of sulfur in the coal sample. Sulfuric acid has two acidic hydrogens.

What mass of solid AgBr is produced when 100.0 \(\mathrm{mL}\) of 0.150 \(\mathrm{MAgNO}_{3}\) is added to 20.0 \(\mathrm{mL}\) of 1.00 $\mathrm{M} \mathrm{NaBr} ?$

A 500.0-mL sample of 0.200 M sodium phosphate is mixed with 400.0 mL of 0.289 M barium chloride. What is the mass of the solid produced?
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