Determine the hydronium and hydroxide ion concentrations in a solution that is 2.0 × 10-2 M NaOH
For OH- I got 2.0*10^-2 M
and for H30+ I got 2.0*10^-2 M
Is this correct?
in an aqueous solution , what is the product of [H3O+] and [OH-] ?
No, OH^- is correct but that can't possible be the same as H3O^+.
(H3O^+)(OH^-) = Kw = 1E-14. Substitute your OH^- and solve for H3O^+.
To determine the hydronium (H₃O⁺) and hydroxide (OH⁻) ion concentrations in a solution of NaOH, you need to understand that NaOH is a strong base that dissociates completely in water.
The balanced equation for the dissociation of NaOH in water is:
NaOH → Na⁺ + OH⁻
From this equation, you can see that for every one mole of NaOH that dissociates, one mole of OH⁻ ions is produced.
Given that the concentration of NaOH is 2.0 × 10⁻² M, this concentration represents the concentration of Na⁺ ions in the solution, as NaOH completely dissociates into Na⁺ and OH⁻ ions. Therefore, the concentration of OH⁻ ions is also 2.0 × 10⁻² M.
Now, since water dissociates into H₃O⁺ and OH⁻ ions, the concentration of OH⁻ ions is equivalent to the concentration of H₃O⁺ ions. Thus, the concentration of H₃O⁺ ions in the solution is also 2.0 × 10⁻² M.
Therefore, the hydronium (H₃O⁺) ion concentration is 2.0 × 10⁻² M, and the hydroxide (OH⁻) ion concentration is also 2.0 × 10⁻² M.