Final answer:
All the options provided represent fundamental equations in acid-base chemistry and are correct. The relationships show how pH, pOH, and ion concentration interrelate in aqueous solutions, none is incorrect.
Step-by-step explanation:
The question asks which of the following relationships is incorrect:
- pH + pOH = 14
- [OH-] = 10^pOH
- pKw = -logKw
- [OH-][H₃O+] = 1 x 10⁻¹⁴
- pH = -log[H₃O+]
All the listed relationships are core concepts in acid-base chemistry. They describe how pH, pOH, and ion concentrations relate to each other in aqueous solutions.
pH and pOH are related by the equation pH + pOH = 14 at 25°C, which reflects the neutralization of hydronium (H₃O+) and hydroxide (OH⁻) ions in water. The relationship between the concentration of hydroxide ions ([OH⁻]) and pOH is given by [OH⁻] = 10^(-pOH). This allows us to calculate the concentration of OH⁻ from pOH. pH is calculated from the hydronium ion concentration [H₃O+] using the equation pH = -log[H₃O+]. The product of hydronium and hydroxide ion concentrations is always 1 x 10⁻¹⁴ at 25°C, represented by the equation [OH⁻][H₃O+] = 1 x 10⁻¹⁴. Finally, pKw is the negative log of the ionic product of water (Kw), hence pKw = -logKw.
Given the information, all relationships are correct as they are fundamental equations in acid-base chemistry and thus none of the relationships provided is incorrect.