How do you get Kw=1.0×10×−14 at 25° in no 1 question

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ScanSolve AI Tutor · Accepted Answer

The value of K_w = 1.0 × 10⁻¹⁴ at 25° C comes from the autoionization of water. Step 1: Water undergoes a slight autoionization, meaning it reacts with itself to form hydronium ions (H₃O^+ or simply H^+) and hydroxide ions (OH^−). H₂O(l) + H₂O(l) H₃O^+(aq) + OH^−(aq) This can be simplified as: H₂O(l) H^+(aq) + OH^−(aq) Step 2: The equilibrium constant for this reaction is called the ion product of water, K_w. K_w = [H^+][OH^−] Step 3: In pure water at 25° C, the concentrations of H^+ and OH^− ions are equal because they are produced in a 1:1 ratio. Through experimental measurements (e.g., conductivity), it's found that the concentration of each ion is 1.0 × 10⁻⁷ M. [H^+] = 1.0 × 10⁻⁷ M; [OH^−] = 1.0 × 10⁻⁷ M Step 4: Substitute these concentrations into the K_w expression. K_w = (1.0 × 10⁻⁷)(1.0 × 10⁻⁷); K_w = 1.0 × 10⁽⁻⁷⁾⁺⁽⁻⁷⁾; K_w = 1.0 × 10⁻¹⁴; Thus, at 25° C, the ion product of water is K_w = 1.0 × 10⁻¹⁴.

How do you get Kw=1.0×10*-14 at 25° in no 1 question

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Step-by-step solution

Water undergoes a slight autoionization, meaning it reacts with itself to form hydronium ions ( $\text{H}_3\text{O}^+$ or simply $\text{H}^+$ ) and hydroxide ions ( $\text{OH}^-$ ).

The equilibrium constant for this reaction is called the ion product of water, $K_w$ .

In pure water at $25^\circ \text{C}$ , the concentrations of $\text{H}^+$ and $\text{OH}^-$ ions are equal because they are produced in a 1:1 ratio.

Substitute these concentrations into the $K_w$ expression.

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