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Chapter 13: Problem 95

Is a saline ( \(\mathrm{NaCl}\) ) solution at \(80^{\circ} \mathrm{C}\) acidic, basic, or neutral?

Short Answer

Expert verified
A saline solution (NaCl) at 80°C is neutral. This is because the ions produced when NaCl dissolves in water do not alter the acidity or basicity of the solution. Additionally, the increased temperature does not affect the pH of the solution since the ionization of water at higher temperatures affects both acidic and basic ions equally, maintaining the pH of the solution at a neutral value.

Step by step solution

01

Understand the properties of NaCl

Sodium chloride (NaCl) is a salt formed from the neutralization reaction between a strong acid (hydrochloric acid, HCl) and a strong base (sodium hydroxide, NaOH). When NaCl is dissolved in water, it dissociates into its constituent ions, Na\(^+\) and Cl\(^-\).
02

Observe the behavior of Na\(^+\) and Cl\(^-\) ions in water

When NaCl dissociates in water, the Na\(^+\) and Cl\(^-\) ions interact with water molecules. However, since both ions come from strong acid (HCl) and strong base (NaOH), they do not react with water to form either hydronium (H\(_3\)O\(^+\)) ions or hydroxide (OH\(^-\)) ions. This means that they do not alter the acidity or basicity of the solution.
03

Consider the effect of temperature

In this scenario, the saline solution is at \(80^{\circ} \mathrm{C}\). The effect of temperature on the ionization of water should be considered. At higher temperatures, the ionization of water increases, which results in an increase in the concentration of both H\(_3\)O\(^+\) and OH\(^-\) ions in the solution. However, since the concentration of both ions increases equally, the overall pH of the solution remains neutral (pH = 7).
04

Conclusion

A saline solution (NaCl) at \(80^{\circ} \mathrm{C}\) is neutral, as the ions produced when NaCl dissolves in water do not alter the acidity or basicity of the solution. The increased temperature doesn't affect the conclusion since the increase in ionization of water at higher temperatures affects both acidic and basic ions equally, maintaining the pH of the solution at a neutral value.

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Most popular questions from this chapter

Calculate \(\left[\mathrm{H}^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) in solutions with the following \(\mathrm{pH}\). (a) \(4.0\) (b) \(8.52\) (c) \(0.00\) (d) \(12.60\)

Milk of Magnesia has a pH of \(10.5\). (a) Calculate \(\left[\mathrm{H}^{+}\right]\). (b) Calculate the ratio of the \(\mathrm{H}^{+}\) concentration of gastric juice, \(\mathrm{pH} 1.5\), to that of Milk of Magnesia.

Using the Brønsted-Lowry model, write an equation to show why each of the following species produces a basic aqueous solution. (a) \(\mathrm{NH}_{3}\) (b) \(\mathrm{NO}_{2}^{-}\) (c) \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\) (d) \(\mathrm{CO}_{3}{ }^{2-}\) (e) \(\mathrm{F}^{-}\) (f) \(\mathrm{HCO}_{3}^{-}\)

The \(\mathrm{pH}\) of a household ammonia cleaning solution is \(11.68\). How many grams of ammonia are needed in a 1.25-L solution to give the same pH?

The solubility of \(\mathrm{Ca}(\mathrm{OH})_{2}\) at \(25^{\circ} \mathrm{C}\) is \(0.153 \mathrm{~g} / 100 \mathrm{~g} \mathrm{H}_{2} \mathrm{O}\). Assuming that the density of a saturated solution is \(1.00 \mathrm{~g} / \mathrm{mL}\), calculate the maximum \(\mathrm{pH}\) one can obtain when \(\mathrm{Ca}(\mathrm{OH})_{2}\) is dissolved in water.
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