Determine the hydronium ion concentration in a solution that is 0.00042M HCL Answer in units of M.
pH = -log (H3O^+) and since HCl is a strong acid and ionizes 100%, then
pH = -log(HCl). In very weak acid solutions it is necessary to take into account the H^+ contribution of the H^+ in water but I don't think that will be necessary in this concentration.
Determine the hydroxide ion concentration in a solution that is 0.0027 M Ca(OH)2. Answer in units of M
Ca(OH)2 ==> Ca^2+ + 2OH^-
SO, if [Ca(OH)2] = 0.0027 M then (OH^-) must be twice that. Right?
To determine the hydronium ion concentration in a solution of 0.00042 M HCl (hydrochloric acid), we need to understand that HCl is a strong acid that completely dissociates in water to form H+ ions (protons) and Cl- ions.
The balanced chemical equation for this process is:
HCl(aq) → H+(aq) + Cl-(aq)
Since HCl fully dissociates, the concentration of hydronium ions (H3O+) is equal to the concentration of H+ ions. Therefore, in our case, the hydronium ion concentration is also 0.00042 M.
Thus, the hydronium ion concentration in the solution is 0.00042 M.