Write a balanced chemical equation that represents the self-ionization of water. (Use the lowest possible coefficients. Include states-of-matter at 1 atm and 25°C in your answer.)
Well, the self-ionization of water is when water molecules split up into hydrogen ions (H+) and hydroxide ions (OH-). It's like water is having a mini identity crisis!
H2O(l) ⇌ H+(aq) + OH-(aq)
So, at 1 atm and 25°C, water molecules decide to split up and become ions, but don't worry, they'll still be friends – just different versions of themselves. It's like water's rebellious teenage phase!
The balanced chemical equation for the self-ionization of water is:
2 H2O(l) ⇌ H3O+(aq) + OH-(aq)
Please note that in this equation, H2O represents water in its liquid state, H3O+ represents the hydronium ion (an acid), and OH- represents the hydroxide ion (a base). The double arrows indicate a reversible reaction, meaning that the self-ionization is an equilibrium process.
To write the balanced chemical equation that represents the self-ionization of water, we first need to understand that water can donate and accept protons (H+ ions) to form the hydronium ion (H3O+) and the hydroxide ion (OH-).
The balanced chemical equation for the self-ionization of water is:
2 H2O(l) ⇌ H3O+(aq) + OH-(aq)
In this equation:
- "2 H2O" represents two water molecules.
- "(l)" represents the state of matter for water, which is liquid.
- "⇌" represents the equilibrium arrow, indicating that the reaction can occur in both directions.
- "H3O+" represents the hydronium ion, which has accepted a proton (H+) from water.
- "OH-" represents the hydroxide ion, which is left after water has donated a proton.
Note: The actual concentration of H3O+ and OH- ions in pure water is very low, indicating that the self-ionization of water is a very small reaction.