In aqueous solutions, the concentration of hydrogen ions ([H+]) and hydroxide ions ([OH-]) dictates the acidity or basicity of the solution. At 25°C, pure water has a neutral pH where $[[H^+] = [OH^-] = 1.0 \times 10^{-7} M]$. Acids increase the $[H^+]$ concentration, while bases increase the $[OH^-]$ concentration. The ion product of water, $K_w$, is constant at a given temperature: $[K_w = [H^+][OH^-] = 1.0 \times 10^{-14}]$ at 25°C. Understanding these relationships is crucial for solving equilibrium problems and determining pH and pOH values.
Match the term with its correct definition:
| Term | Definition |
|---|---|
| 1. pH | A. A substance that increases the concentration of $OH^-$ ions in solution. |
| 2. Acid | B. The negative logarithm of the hydroxide ion concentration, $pOH = -log[OH^-]$. |
| 3. Base | C. The negative logarithm of the hydrogen ion concentration, $pH = -log[H^+]$. |
| 4. pOH | D. A substance that increases the concentration of $H^+$ ions in solution. |
| 5. $K_w$ | E. The ion product of water, $[K_w = [H^+][OH^-] = 1.0 \times 10^{-14}]$ at 25°C. |
Complete the following paragraph using the words: acidic, basic, neutral, $[H^+]$, $[OH^-]$, $1.0 \times 10^{-7}$, $1.0 \times 10^{-14}$.
A solution is considered _______ if the concentration of _______ is greater than the concentration of _______. A solution is _______ if the $[H^+]$ concentration equals the $[OH^-]$ concentration, which is _______ M at 25°C. A solution is _______ if the $[OH^-]$ concentration is greater. The ion product of water, $K_w$, equals _______.
Explain how changes in temperature can affect the $K_w$ value and how this, in turn, would impact the relationship between pH and pOH.
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