Multiple Choice
At 60 °C, the value of KW is 1.3×10⁻¹³. What is the concentration of H₃O⁺ in a neutral solution at 60 °C?
17. Acid and Base Equilibrium
Auto-Ionization
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Calculate the Kw of pure water given the pH = 6.34.
A
4.57 × 10−7
B
6.76 × 10−4
C
2.09 × 10−13
D
4.57 × 10−14
Verified step by step guidance1
Understand that the pH of a solution is related to the concentration of hydrogen ions [H⁺] in the solution. The formula to find [H⁺] from pH is: \( [H^+] = 10^{-\text{pH}} \).
Substitute the given pH value into the formula: \( [H^+] = 10^{-6.34} \).
In pure water, the concentration of hydrogen ions [H⁺] is equal to the concentration of hydroxide ions [OH⁻]. Therefore, \( [OH^-] = [H^+] \).
The ion product of water, \( K_w \), is given by the product of the concentrations of hydrogen ions and hydroxide ions: \( K_w = [H^+][OH^-] \).
Substitute the value of \( [H^+] \) into the expression for \( K_w \): \( K_w = (10^{-6.34})(10^{-6.34}) \). Calculate this product to find the value of \( K_w \).
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