Calculate the \(\left[\mathrm{H}^{+}\right]\)for (a) pure water (b) lemon lime soda with a \(\mathrm{pH}\) of \(4.3\) (c) root beer with a \(\mathrm{pH}\) of \(5.8\) (d) window cleaner with a \(\mathrm{pH}\) of \(10.3\)

Acid-base chemistry is all about understanding the properties of acids and bases, and how they interact with each other. An acid is a substance that can donate a proton (\(\text{H}^+\) ion), while a base is a substance that can accept a proton. In water, acids increase the concentration of \(\text{H}^+\) ions, making the solution more acidic. Bases, on the other hand, reduce the concentration of \(\text{H}^+\) ions by providing more hydroxide ions (\(\text{OH}^-\)).To study acid-base chemistry, we use the pH scale. This scale ranges from 0 to 14 and tells us how acidic or basic a solution is. A pH less than 7 indicates an acidic solution, a pH of 7 is neutral (like pure water), and a pH above 7 is basic.- Acid is a proton donor- Base is a proton acceptor- pH scale ranges from 0 to 14

The concentration of hydrogen ions (\(\text{H}^+\)) in a solution is crucial for determining its acidity or basicity. In pure water, \(\text{H}^+\) and hydroxide ions (\(\text{OH}^-\)) exist in equal amounts. This balance makes the water neutral with a pH of 7, creating a concentration of \(\text{H}^+\) ions of \(1 \times 10^{-7}\) M.To calculate the \(\text{H}^+\) ion concentration in other solutions, we use the formula: \[ [\text{H}^+] = 10^{-\text{pH}} \] Therefore, we can find \(\text{H}^+\) for any given pH value by plugging it into the formula.- Pure water has \(\text{H}^+ = 1 \times 10^{-7}\) M- Use \([\text{H}^+] = 10^{-\text{pH}}\) to find \(\text{H}^+\) for other solutions

Logarithmic functions are a special way of expressing numbers, and they are particularly useful in acid-base chemistry. The pH scale is logarithmic, which means every unit change in pH represents a tenfold change in \(\text{H}^+\) concentration.Using the pH formula: \[ \text{pH} = -\text{log}[\text{H}^+] \] When you need to find \(\text{H}^+\), you take the inverse log (or antilog). This inverse operation is written as: \[ [\text{H}^+] = 10^{-\text{pH}} \] Logarithmic scales make it easier to handle the very large or very small numbers typically encountered in chemistry.- pH = -log[H\(^+\)]- \([\text{H}^+] = 10^{-\text{pH}}\)

The pH of a solution reveals how acidic or basic it is. To calculate it, we first determine the \(\text{H}^+\) concentration. For example, if the pH is 4.3, use the formula: \[ [\text{H}^+] = 10^{-4.3} \] Applying this formula helps us find the \(\text{H}^+\) concentration in various solutions:- For a pH of 7 (pure water): \([\text{H}^+] = 1 \times 10^{-7}\) M- For a pH of 4.3 (lemon lime soda): \([\text{H}^+] = 5.01 \times 10^{-5}\) M- For a pH of 5.8 (root beer): \([\text{H}^+] = 1.58 \times 10^{-6}\) M- For a pH of 10.3 (window cleaner): \([\text{H}^+] = 5.01 \times 10^{-11}\) MKnowing the pH and \(\text{H}^+\) concentration helps us better understand the properties and behavior of various solutions.