Determining If A Solution Is Acidic Or Basic Based On [H+], PH, And POH

by THE IDEN 72 views

Introduction

In chemistry, understanding whether a solution is acidic, basic, or neutral is fundamental. The acidity or basicity of a solution is determined by the concentration of hydrogen ions (H+H^+) and hydroxide ions (OHβˆ’OH^-). The pH scale, ranging from 0 to 14, is used to quantify this property. A pH of 7 indicates neutrality, values below 7 indicate acidity, and values above 7 indicate basicity. Other related concepts include pOH, which measures the concentration of hydroxide ions, and the ion product of water (KwK_w), which relates the concentrations of H+H^+ and OHβˆ’OH^- in aqueous solutions. Determining whether a solution is acidic or basic is crucial in various fields, including environmental science, biology, and industrial chemistry. This article delves into the process of interpreting the given dataβ€”[H+][H^+], pH, and pOHβ€”to accurately classify a solution as acidic or basic.

Understanding the Given Data

To accurately determine the nature of a solution, it is crucial to analyze the provided data meticulously. Let's begin by examining the given values: [H+]=7.6imes10βˆ’12M[H^+] = 7.6 imes 10^{-12} M, pH=11.12pH = 11.12, and pOH=2.88pOH = 2.88. Each of these parameters provides valuable insights into the solution's characteristics. The concentration of hydrogen ions, denoted as [H+][H^+], indicates the molar concentration of H+H^+ ions in the solution. In this case, the concentration is 7.6imes10βˆ’12M7.6 imes 10^{-12} M, which is a relatively small value. This suggests that the solution has a low concentration of hydrogen ions. The pH value is a logarithmic scale that measures the acidity or basicity of a solution. It is defined as the negative logarithm (base 10) of the hydrogen ion concentration: pH=βˆ’log[H+]pH = -log[H^+]. The given pH value is 11.12, which falls in the higher range of the pH scale. The pOH value, on the other hand, measures the concentration of hydroxide ions (OHβˆ’OH^-) in the solution. It is defined as the negative logarithm (base 10) of the hydroxide ion concentration: pOH=βˆ’log[OHβˆ’]pOH = -log[OH^-]. The given pOH value is 2.88. Understanding these values and their relationships is essential for correctly classifying the solution as acidic, basic, or neutral. The pH and pOH scales are inversely related, and their sum at 25Β°C is always 14, reflecting the ion product of water (KwK_w). The KwK_w is a constant that represents the equilibrium between H+H^+ and OHβˆ’OH^- ions in water, and it equals 1.0imes10βˆ’141.0 imes 10^{-14} at 25Β°C. By analyzing the given [H+][H^+], pH, and pOH values, we can gain a comprehensive understanding of the solution's properties and accurately determine its nature.

Analyzing Hydrogen Ion Concentration ([H+][H^+])

The concentration of hydrogen ions ([H+][H^+]) is a fundamental indicator of a solution's acidity or basicity. A high concentration of H+H^+ ions signifies an acidic solution, while a low concentration indicates a basic solution. In the given data, the hydrogen ion concentration is [H+]=7.6imes10βˆ’12M[H^+] = 7.6 imes 10^{-12} M. This value is significantly lower than 1.0imes10βˆ’7M1.0 imes 10^{-7} M, which is the concentration of H+H^+ ions in pure water at 25Β°C (neutral condition). To put this into perspective, a neutral solution has an equal concentration of hydrogen and hydroxide ions, making the [H+][H^+] equal to 1.0imes10βˆ’7M1.0 imes 10^{-7} M. When the [H+][H^+] is lower than this value, it means there are fewer hydrogen ions compared to hydroxide ions, suggesting a basic environment. The fact that the given [H+][H^+] is 7.6imes10βˆ’12M7.6 imes 10^{-12} M strongly suggests that the solution is basic. This is because the concentration of hydrogen ions is substantially less than that in a neutral solution. In acidic solutions, the [H+][H^+] would be greater than 1.0imes10βˆ’7M1.0 imes 10^{-7} M, and in strongly acidic solutions, it would be much higher. For instance, a [H+][H^+] of 1.0imes10βˆ’2M1.0 imes 10^{-2} M indicates a highly acidic solution. The extremely low [H+][H^+] in our case points definitively towards a basic nature of the solution. This initial assessment based on hydrogen ion concentration is crucial and consistent with the other provided data, such as the pH and pOH values, which will be analyzed further to provide a comprehensive understanding of the solution’s characteristics.

Interpreting the pH Value

The pH value is a widely used measure to determine the acidity or basicity of a solution. It is defined as the negative logarithm (base 10) of the hydrogen ion concentration (pH=βˆ’log[H+]pH = -log[H^+]). The pH scale ranges from 0 to 14, where pH 7 is considered neutral, pH values less than 7 indicate acidity, and pH values greater than 7 indicate basicity. In this case, the given pH value is 11.12. This value falls significantly above 7, placing it firmly in the basic range of the pH scale. A pH of 7 is characteristic of pure water at 25Β°C, where the concentrations of hydrogen ions (H+H^+) and hydroxide ions (OHβˆ’OH^-) are equal. Solutions with a pH less than 7 have a higher concentration of H+H^+ ions than OHβˆ’OH^- ions, making them acidic. The lower the pH value, the higher the acidity. For example, a solution with a pH of 2 is strongly acidic. Conversely, solutions with a pH greater than 7 have a lower concentration of H+H^+ ions than OHβˆ’OH^- ions, making them basic or alkaline. The higher the pH value, the stronger the basicity. A pH of 11.12 indicates a considerably basic solution. To put this into context, common household substances such as baking soda (pH around 8.3) and ammonia (pH around 11) are basic. A pH of 11.12 suggests that the solution is more basic than baking soda and is comparable to the basicity of ammonia. Thus, the pH value of 11.12 provides strong evidence that the solution is basic, reinforcing the conclusion drawn from the low hydrogen ion concentration ([H+]=7.6imes10βˆ’12M[H^+] = 7.6 imes 10^{-12} M). The interpretation of the pH value is a critical step in accurately classifying the nature of a solution.

Analyzing the pOH Value

The pOH value is another important parameter for determining the acidity or basicity of a solution. While pH measures the concentration of hydrogen ions (H+H^+), pOH measures the concentration of hydroxide ions (OHβˆ’OH^-). The relationship between pOH and [OHβˆ’][OH^-] is defined as pOH=βˆ’log[OHβˆ’]pOH = -log[OH^-]. The pOH scale, like the pH scale, ranges from 0 to 14, but the interpretation is reversed: a pOH less than 7 indicates basicity, a pOH of 7 indicates neutrality, and a pOH greater than 7 indicates acidity. The sum of pH and pOH at 25Β°C is always 14 (pH+pOH=14pH + pOH = 14), reflecting the ion product of water (Kw=[H+][OHβˆ’]=1.0imes10βˆ’14K_w = [H^+][OH^-] = 1.0 imes 10^{-14}). In this case, the given pOH value is 2.88. Since this value is less than 7, it strongly suggests that the solution is basic. A low pOH indicates a high concentration of hydroxide ions, which is characteristic of basic solutions. To understand this further, let's consider the relationship between pH and pOH. Given that pH+pOH=14pH + pOH = 14, a pOH of 2.88 corresponds to a pH of 14βˆ’2.88=11.1214 - 2.88 = 11.12, which is consistent with the given pH value. This consistency between the pOH and pH values reinforces the conclusion that the solution is basic. In acidic solutions, the pOH would be greater than 7, indicating a lower concentration of hydroxide ions. For instance, a pOH of 10 would correspond to a pH of 4, which is indicative of an acidic solution. The low pOH value of 2.88 definitively points towards a high concentration of hydroxide ions, confirming the basic nature of the solution. This analysis of the pOH value provides an additional layer of evidence, complementing the information obtained from the hydrogen ion concentration and the pH value, to accurately classify the solution.

Conclusion: Solution Classification

After a thorough analysis of the given data, including the hydrogen ion concentration ([H+]=7.6imes10βˆ’12M[H^+] = 7.6 imes 10^{-12} M), the pH value (11.12), and the pOH value (2.88), it is definitively clear that the solution is basic. Each of these parameters independently points to the same conclusion, reinforcing the accuracy of the classification. The low hydrogen ion concentration indicates a scarcity of H+H^+ ions relative to hydroxide ions, a hallmark of basic solutions. The pH value of 11.12, significantly above the neutral pH of 7, confirms the basic nature of the solution. Similarly, the pOH value of 2.88, which is less than 7, further supports this conclusion by indicating a high concentration of hydroxide ions. The consistency across all three indicators provides a comprehensive understanding of the solution's properties. In summary, the integration of evidence from [H+][H^+], pH, and pOH values leaves no doubt that the solution under consideration is basic. This determination is crucial in various applications, including chemical reactions, environmental monitoring, and biological processes, where the acidity or basicity of a solution can significantly impact the outcome.