Textbook Question
The average pH of normal arterial blood is 7.40. At normal body temperature 137 °C2, Kw = 2.4 * 10-14. Calculate 3H+4, 3OH-4, and pOH for blood at this temperature.
17. Acid and Base Equilibrium
Auto-Ionization
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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?
A
1.0×10⁻⁷ M
B
1.1×10⁻⁷ M
C
1.3×10⁻⁷ M
D
1.3×10⁻⁶ M
Verified step by step guidance1
Understand that in a neutral solution, the concentration of hydronium ions \( [\text{H}_3\text{O}^+] \) is equal to the concentration of hydroxide ions \( [\text{OH}^-] \).
Recall the expression for the ion product of water \( K_w \), which is given by \( K_w = [\text{H}_3\text{O}^+][\text{OH}^-] \).
At 60 °C, the value of \( K_w \) is provided as \( 1.3 \times 10^{-13} \).
Since the solution is neutral, set \( [\text{H}_3\text{O}^+] = [\text{OH}^-] = x \). Substitute into the \( K_w \) expression: \( x^2 = 1.3 \times 10^{-13} \).
Solve for \( x \) by taking the square root of both sides: \( x = \sqrt{1.3 \times 10^{-13}} \). This value of \( x \) will give you the concentration of \( [\text{H}_3\text{O}^+] \) in a neutral solution at 60 °C.
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