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Chapter 16: Problem 77

One drop of \(1 \mathrm{M} \mathrm{OH}^{-}\)ion is added to a \(1 M\) solution of \(\mathrm{HNO}_{2}\). What will be the effect of this addition on the equilibrium concentration of the following? $$ \mathrm{HNO}_{2}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{NO}_{2}^{-}(a q) $$ (a) \(\left[\mathrm{OH}^{-}\right]\) (c) \(\left[\mathrm{NO}_{2}^{-}\right]\) (b) \(\left[\mathrm{H}^{+}\right]\) (d) \(\left[\mathrm{HNO}_{2}\right]\)

Short Answer

Expert verified
The addition of OH鈦� will decrease [H鈦篯, increase [NO鈧傗伝], and decrease [HNO鈧俔. [OH鈦籡 will fluctuate but generally increase initially.

Step by step solution

01

- Understand the Addition of OH鈦�

When a drop of 1 M OH鈦� is added to a 1 M solution of HNO鈧�, the OH鈦� ions will react with H鈦� ions in the solution. The reaction is: \[ \text{OH}^{-} + \text{H}^{+} \rightarrow \text{H}_2\text{O} \] This will remove H鈦� ions from the solution.
02

- Le Chatelier鈥檚 Principle

According to Le Chatelier鈥檚 Principle, if the concentration of H鈦� is decreased, the system will shift to the right to produce more H鈦� ions and NO鈧傗伝 ions. The equilibrium shift can be represented as: \[ \text{HNO}_2 \rightleftharpoons \text{H}^{+} + \text{NO}_2^{-} \]
03

- Effect on Equilibrium Concentrations

- (a) The concentration of OH鈦� will initially increase due to the addition but will subsequently decrease as it reacts with H鈦� to form water.- (b) The concentration of H鈦� will also decrease as it reacts with OH鈦�.- (c) The concentration of NO鈧傗伝 will increase as the system shifts to the right to replace the H鈦� ions.- (d) The concentration of HNO鈧� might decrease as it dissociates to replace the H鈦� ions.
04

- Summarizing the Changes

Summarizing the changes in equilibrium concentrations:(a) [OH鈦籡 will generally increase initially but will tend to decrease, approaching the initial concentration.(b) [H鈦篯 will decrease.(c) [NO鈧傗伝] will increase.(d) [HNO鈧俔 will decrease.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Le Chatelier's Principle
Le Chatelier's Principle is a fundamental concept in chemical equilibrium. It states that when a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust itself to counteract that change and restore a new balance. In the given problem, adding OH鈦� ions to the HNO鈧� solution reduces the H鈦� ion concentration. According to Le Chatelier's Principle, the equilibrium shifts to produce more H鈦� ions and NO鈧傗伝 ions. This is a way for the system to 'fight against' the disturbance caused by adding OH鈦�.
Acid-Base Reaction
An acid-base reaction involves the transfer of protons (H鈦� ions) between the reactants. In our example, HNO鈧� (nitrous acid) dissociates into H鈦� ions and NO鈧傗伝 ions. Here is the balanced equation: $$\text{HNO}_2 \rightleftharpoons \text{H}^{+} + \text{NO}_2^{-}$$ When OH鈦� ions are added to the solution, they react with H鈦� ions to form water (\text{H}_2\text{O}). This reduces the concentration of H鈦� ions, driving the equilibrium to the right, dissociating more HNO鈧� and increasing the concentration of NO鈧傗伝 ions.
Equilibrium Shift
An equilibrium shift occurs when a system at equilibrium responds to an external change. In our case, adding OH鈦� ions to the HNO鈧� solution shifts the equilibrium. Initially, the OH鈦� ions react with H鈦� ions, reducing their concentration. According to Le Chatelier's Principle, the system compensates by shifting the equilibrium to the right, increasing the concentration of NO鈧傗伝 ions. This shift aims to balance the reduced H鈦� ions by dissociating more HNO鈧�.
HNO鈧� Dissociation
HNO鈧�, or nitrous acid, is a weak acid that partially dissociates in water. The dissociation can be expressed as: $$\text{HNO}_2 \rightleftharpoons \text{H}^{+} + \text{NO}_2^{-}$$ When OH鈦� ions are added to this system, they react with H鈦� ions, forming water and causing the H鈦� concentration to decrease. As a result, the equilibrium shifts, leading to further dissociation of HNO鈧�. This balances the decreased H鈦� ions and increases the concentration of NO鈧傗伝. Over time, the system reaches a new equilibrium, with adjusted concentrations of all species involved.

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Most popular questions from this chapter

Calculate the ionization constant for the given acids. Each acid ionizes as follows: \(\mathrm{HA} \rightleftharpoons \mathrm{H}^{+}+\mathrm{A}^{-}\). $$ \begin{array}{|l|c|c|} \hline \text { Acid } & \begin{array}{c} \text { Acid } \\ \text { concentration } \end{array} & {\left[\mathrm{H}^{+}\right]} \\ \hline \text { Hypochlorous, } \mathrm{HOCl} & 0.10 M & 5.9 \times 10^{-5} \mathrm{~mol} / \mathrm{L} \\ \hline \text { Propanoic, } \mathrm{HC}_{3} \mathrm{H}_{5} \mathrm{O}_{2} & 0.15 M & 1.4 \times 10^{-3} \mathrm{~mol} / \mathrm{L} \\ \hline \text { Hydrocyanic, } \mathrm{HCN} & 0.20 M & 8.9 \times 10^{-6} \mathrm{~mol} / \mathrm{L} \\ \hline \end{array} $$

(a) Would you expect a reaction to take place between \(\operatorname{HCN}(a q)\) and \(\operatorname{AgNO}_{3}(a q)\) $$ \left(K_{\mathrm{sp}} \text { for } \mathrm{AgCN}=5.97 \times 10^{-17}\right) \text { ? } $$ Explain, and if a reaction occurs, write the net ionic equation. (b) If \(\mathrm{NaCN}\) is added to distilled water, would you expect the solution to be acidic, basic, or neutral? Explain using any chemical equations that may be appropriate.

For the following equations, tell in which direction, left or right, the equilibrium will shift when these changes are made: The temperature is increased, the pressure is increased by decreasing the volume of the reaction vessel, and a catalyst is added. (a) \(2 \mathrm{SO}_{3}(g)+197 \mathrm{~kJ} \rightleftharpoons 2 \mathrm{SO}_{2}(g)+\mathrm{O}_{2}(g)\) (b) \(4 \mathrm{NH}_{3}(g)+3 \mathrm{O}_{2}(g) \rightleftharpoons 2 \mathrm{~N}_{2}(g)+6 \mathrm{H}_{2} \mathrm{O}(g)+1531 \mathrm{~kJ}\) (c) \(\mathrm{OF}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(g) \rightleftharpoons \mathrm{O}_{2}(g)+2 \mathrm{HF}(g)+318 \mathrm{~kJ}\)

What effect will increasing the \(\left[\mathrm{H}^{+}\right]\)of a solution have on (a) \(\mathrm{pH}\), (b) \(\mathrm{pOH}\), (c) \(\left[\mathrm{OH}^{-}\right]\), and (d) \(K_{\mathrm{w}}\) ?

Write the solubility product expression, \(K_{\mathrm{sp}}\), for these substances: (a) \(\mathrm{AgCl}\) (c) \(\mathrm{Zn}(\mathrm{OH})_{2}\) (b) \(\mathrm{PbCrO}_{4}\) (d) \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)
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