Welcome to Westonci.ca, where your questions are met with accurate answers from a community of experts and enthusiasts. Discover comprehensive answers to your questions from knowledgeable professionals on our user-friendly platform. Get precise and detailed answers to your questions from a knowledgeable community of experts on our Q&A platform.
Sagot :
Let's work through the question step-by-step:
1. Understanding Self-Ionization of Water:
Water (H₂O) can undergo self-ionization, which means that a small fraction of water molecules dissociate into hydrogen ions (H⁺) and hydroxide ions (OH⁻). This process is represented by the following chemical equation:
[tex]\[ 2H₂O (l) ⇌ H₃O⁺ (aq) + OH⁻ (aq) \][/tex]
However, for simplicity, we often write it as:
[tex]\[ H₂O (l) ⇌ H⁺ (aq) + OH⁻ (aq) \][/tex]
2. Concentration of H⁺ and OH⁻ ions in pure water:
In pure water at 25°C, the concentration of hydrogen ions [tex]\([H⁺]\)[/tex] and hydroxide ions [tex]\([OH⁻]\)[/tex] is [tex]\(1 \times 10^{-7}\)[/tex] moles per liter. This means that in one liter of pure water, there are [tex]\(1 \times 10^{-7}\)[/tex] moles of H⁺ ions and [tex]\(1 \times 10^{-7}\)[/tex] moles of OH⁻ ions.
3. Finding the Number of Moles of Self-Ionized Water Molecules:
Since each self-ionization event of a water molecule produces one H⁺ ion and one OH⁻ ion, the number of moles of self-ionized H₂O molecules is equal to the concentration of either H⁺ or OH⁻ ions. Therefore, in one liter of pure water, the number of moles of water molecules that self-ionize is also [tex]\(1 \times 10^{-7}\)[/tex] moles (or 0.0000001 moles).
4. Conclusion:
From the question, the concentration of self-ionized water molecules in one liter of water is indeed [tex]\(1 \times 10^{-7}\)[/tex] moles.
Therefore, the answer is:
c) 0.0000001 moles
1. Understanding Self-Ionization of Water:
Water (H₂O) can undergo self-ionization, which means that a small fraction of water molecules dissociate into hydrogen ions (H⁺) and hydroxide ions (OH⁻). This process is represented by the following chemical equation:
[tex]\[ 2H₂O (l) ⇌ H₃O⁺ (aq) + OH⁻ (aq) \][/tex]
However, for simplicity, we often write it as:
[tex]\[ H₂O (l) ⇌ H⁺ (aq) + OH⁻ (aq) \][/tex]
2. Concentration of H⁺ and OH⁻ ions in pure water:
In pure water at 25°C, the concentration of hydrogen ions [tex]\([H⁺]\)[/tex] and hydroxide ions [tex]\([OH⁻]\)[/tex] is [tex]\(1 \times 10^{-7}\)[/tex] moles per liter. This means that in one liter of pure water, there are [tex]\(1 \times 10^{-7}\)[/tex] moles of H⁺ ions and [tex]\(1 \times 10^{-7}\)[/tex] moles of OH⁻ ions.
3. Finding the Number of Moles of Self-Ionized Water Molecules:
Since each self-ionization event of a water molecule produces one H⁺ ion and one OH⁻ ion, the number of moles of self-ionized H₂O molecules is equal to the concentration of either H⁺ or OH⁻ ions. Therefore, in one liter of pure water, the number of moles of water molecules that self-ionize is also [tex]\(1 \times 10^{-7}\)[/tex] moles (or 0.0000001 moles).
4. Conclusion:
From the question, the concentration of self-ionized water molecules in one liter of water is indeed [tex]\(1 \times 10^{-7}\)[/tex] moles.
Therefore, the answer is:
c) 0.0000001 moles
We appreciate your time. Please come back anytime for the latest information and answers to your questions. Thanks for using our platform. We aim to provide accurate and up-to-date answers to all your queries. Come back soon. Thank you for visiting Westonci.ca, your go-to source for reliable answers. Come back soon for more expert insights.