Problem 28 - Algebra 2

Question

The pH of each food is given. Find the concentration of hydrogen ions \(\left[\mathrm{H}^{+}\right] .\) egg white, 8.0

Step-by-Step Solution

Answer

The concentration of hydrogen ions [\([H^{+}]\)] in the egg white is \(0.00000001 \, M\).

Step 1: Understanding the pH Scale

The pH scale is a measure of the acidity or alkalinity of a solution. It is defined as the negative logarithm of the concentration of hydrogen ions in a solution. In simple terms, the lower the pH, the more acidic the solution, and the higher the pH, the more alkaline (or less acidic) the solution. The pH scale ranges from 0 to 14.

Step 2: Applying the Formula

Given the pH value as 8.0 for the egg white we will use the formula for calculating the concentration of hydrogen ions which is: \([H^{+}] = 10^{-pH}\). So, this will be: \([H^{+}] = 10^{-8.0}\).

Step 3: Calculation

By using a calculator to find the power of 10 we get: \([H^{+}] = 10^{-8.0} = 0.00000001 \, M\). This is the concentration of hydrogen ions in the egg white.

Key Concepts

Hydrogen Ion Concentration

The concentration of hydrogen ions, noted as \( [H^+] \), is a critical concept in understanding the acidity of solutions. It represents the amount of hydrogen ions present in a given volume of a solution. Hydrogen ions are positively charged, and their concentration directly influences how acidic or basic a solution is.

In chemical terms, a higher concentration of \( [H^+] \) means a solution is more acidic, while a lower concentration indicates a more basic (or alkaline) solution.

• A very high hydrogen ion concentration would correspond to strong acidic solutions like lemon juice or vinegar.
• Conversely, a low concentration is typical for basic solutions like baking soda in water.

To calculate \( [H^+] \) from a pH value, a logarithmic relationship is utilized, specifically the formula \([H^{+}] = 10^{-pH}catch \). This formula shows that pH is inversely and logarithmically related to hydrogen ion concentration, making it easier to manage a wide range of acidity levels.

pH Scale

The pH scale is a measurement system used to specify the acidity or alkalinity of an aqueous solution. It is one of the most common indicators in chemistry for determining how acidic or basic a solution is. The pH scale ranges from 0 to 14, with each step on the scale representing a tenfold change in hydrogen ion concentration.

On the pH scale:

• pH 7 is neutral, which is the pH of pure water.
• pH values less than 7 indicate acidic solutions.
• pH values greater than 7 indicate alkaline (or basic) solutions.

The pH scale is logarithmic, meaning each whole number change corresponds to a factor of ten change in the concentration of hydrogen ions. For example, a solution with a pH of 3 is ten times more acidic than one with a pH of 4.

This scale is crucial for many fields, including biology, chemistry, medicine, and environmental science, as it helps in understanding chemical conditions and processes.

Acidity and Alkalinity

Acidity and alkalinity refer to the chemical properties of substances that determine their reaction with other substances, specifically their potential to donate or accept hydrogen ions. These properties are often described using the pH scale and are essential in many chemical and biological processes.

Acidity refers to the level at which a solution can donate hydrogen ions. Acids contribute hydrogen ions when dissolved in water. Examples include lemon juice and vinegar, which have pH values below 7.

• Acids are generally sour in taste and can corrode metals.
• They play significant roles in various industrial and biological functions.

Alkalinity, on the other hand, refers to a solution's ability to accept hydrogen ions. Alkaline substances, or bases, reduce the concentration of hydrogen ions in solution. Baking soda in water is an example of an alkaline solution with a pH above 7.

• Bases are usually bitter and slippery to the touch.
• They are essential in many cleaning and neutralizing processes.

Both acidity and alkalinity are vital for maintaining environmental balance and are inherently linked to the pH scale.