Question

Could you use the p-notation for the concentration of a very dilute solution of chloride ion for a solution made when a tablespoon of water is added to a gallon of water? How would it be defined?

Short answer

p-Notation could be used for a very dilute solution of chloride ions if the concentration is within a range where a logarithmic scale is meaningful. It would be defined as pCl = -log[Cl-], where [Cl-] is the molarity of chloride ions.

Step-by-step solution

Understanding p-Notation

The p-notation is commonly used to express small quantities of substances, such as the concentration of ions in a solution. It is used in chemistry for various scales like pH or pOH, which represent the negative logarithm of hydrogen and hydroxide ion concentrations respectively. The general formula is represented as pX, where pX = -log[X], and [X] is the concentration of the ion of interest.

Assessing the Concentration Scale

To determine if p-notation is suitable for expressing the concentration of chloride ions in the very dilute solution, we need to know if the chloride concentration is within a range where the logarithmic scale provides a meaningful and convenient representation. For extremely dilute solutions, such as a tablespoon of water in a gallon, the concentration of chloride ions (if present) is typically very low and may fall into the range where p-notation is sensible.

Defining p-Notation for Chloride Concentration

If the concentration of chloride ions is suitable for p-notation, it would be defined as pCl = -log[Cl-], where [Cl-] represents the molarity of chloride ions in the solution. However, to use this notation, one must know the specific concentration of chloride ions in moles per liter. Without this information, the pCl cannot be calculated directly.

Key concepts

Ion Concentration

When we talk about ion concentration in chemistry, we're discussing the amount of ions present in a particular volume of solution. In the context of dilute solutions, such as adding a tablespoon of water to a gallon of water, the concentration of any dissolved ions like chloride (Cl⁻) will be quite small. Assuming we know the exact amount of chloride present, we express this in units of molarity, which is the number of moles of ions per liter of solution (moles/L). This measurement is crucial because it allows chemists to predict and control the reactions that depend on the presence of specific ions.

Logarithmic Concentration Scale

A logarithmic concentration scale is used to simplify the expression of ion concentrations, especially when dealing with very small numbers. Such a scale is proportional to the logarithm of the ion concentration, making it easier to work with values that span several orders of magnitude. In simple terms, on a logarithmic scale, each step or number represents a tenfold change in concentration. This is particularly useful in chemistry for capturing the wide range of ion concentrations that can be present in solutions.

Molarity

Molarity is a central concept in solution chemistry and represents the concentration of a solute in a solution. It’s defined as the number of moles of solute divided by the volume of solution in liters (mol/L). For instance, if a solution has one mole of solute in one liter of water, its molarity is 1 M. Working with molarity is essential when preparing solutions for reactions and when discussing concentrations in a consistent and standardized manner. It's especially important because reactions often depend on the molarity of reactants for the reaction to proceed correctly.

pH and pOH

pH and pOH are specific applications of p-notation in chemistry. The pH is a measure of the acidity or basicity of an aqueous solution. It is defined as the negative base-10 logarithm of the hydrogen ion (H⁺) concentration:
\[-\log[H^{+}]\].
Conversely, pOH gives the negative logarithm of the hydroxide ion (OH⁻) concentration:
\[-\log[OH^{-}]\].
Pure water has a pH of 7, which is considered neutral. Solutions with a pH less than 7 are acidic, and those with a pH greater than 7 are basic. The pH and pOH values are related through the ion product of water, which is always 1 x 10⁻¹⁴ at 25°C. Therefore, pH + pOH always equals 14 in aqueous solutions. Understanding these concepts is critical in fields ranging from biochemistry to environmental science, as they influence the behavior and stability of molecules in various environments.