Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (c) a solution in which 3H+4 is 1000 times greater than 3OH-4.

Verified step by step guidance

1. Identify the relationship between \([H^+]\) and \([OH^-]\) in the solution. Given that \([H^+]\) is 1000 times greater than \([OH^-]\), express this as \([H^+] = 1000 \times [OH^-]\).
2. Recall the water dissociation constant at 25°C: \(K_w = [H^+][OH^-] = 1.0 \times 10^{-14}\).
3. Substitute \([H^+] = 1000 \times [OH^-]\) into the expression for \(K_w\): \((1000 \times [OH^-]) \times [OH^-] = 1.0 \times 10^{-14}\).
4. Solve for \([OH^-]\) by simplifying the equation: \(1000 \times [OH^-]^2 = 1.0 \times 10^{-14}\).
5. Determine the nature of the solution by comparing \([H^+]\) and \([OH^-]\). If \([H^+] > [OH^-]\), the solution is acidic.

Key Concepts

pH and pOH

pH is a measure of the hydrogen ion concentration in a solution, while pOH measures the hydroxide ion concentration. The relationship between pH and pOH is defined by the equation pH + pOH = 14 at 25°C. A solution is considered acidic if pH < 7, basic if pH > 7, and neutral if pH = 7.

Ion Concentration Ratio

The concentration of hydrogen ions (H+) and hydroxide ions (OH-) in a solution determines its acidity or basicity. If the concentration of H+ is significantly greater than that of OH-, the solution is acidic. Conversely, if OH- is more concentrated, the solution is basic. In this case, the problem states that [H+] is 1000 times greater than [OH-], indicating an acidic solution.

Logarithmic Scale of pH

The pH scale is logarithmic, meaning each whole number change on the scale represents a tenfold change in hydrogen ion concentration. Therefore, a solution with [H+] that is 1000 times greater than [OH-] corresponds to a pH of approximately 3, indicating a strongly acidic solution. Understanding this scale is crucial for interpreting the acidity or basicity of solutions.