In s 0.30 mol/L HNO3(aq) solution.
a) what is the concentration of nitric acid molecules.
b)what is the hydroxide ion concentration?
Thank you! I am still confused about b)
NVM, i got it! thanks!
is it true that at 20ºC, 100g = 100mL （for water)
How do we determine the specific gravity of a solution? and what unit is it in?
How did you know that (H^+)(OH^-) = 1E-14?
And how did you know that (H^+) = 0.30 (Other than knowing that it was given from the questions, how would you know if that was the concentration of the hydrogen ion?)
To find the answers to these questions, we need to use the concept of dissociation of acids in water.
a) The concentration of nitric acid molecules can be calculated by assuming that all the HNO3 molecules dissociate completely into H+ and NO3- ions in water. This means that the concentration of HNO3 molecules will be equal to the concentration of H+ ions in the solution.
In a 0.30 mol/L HNO3(aq) solution, the concentration of HNO3 molecules is 0.30 mol/L.
b) To determine the hydroxide ion (OH-) concentration in this solution, we need to use the concept of the autoionization of water. Water molecules can self-ionize, forming equal concentrations of H+ and OH- ions. This means that in neutral water, the concentration of H+ ions is equal to the concentration of OH- ions.
Since HNO3 is an acid, it donates H+ ions to the solution. However, in this case, the concentration of HNO3 molecules is much higher (0.30 mol/L) compared to the autoionization of water. Therefore, the concentration of H+ ions from HNO3 can be considered negligible compared to the H+ ions from the autoionization of water.
Hence, in a 0.30 mol/L HNO3(aq) solution, the concentration of hydroxide ions (OH-) will be approximately equal to the concentration of hydroxide ions in pure water, which is 1.0 x 10^-7 mol/L.
(a) In aqueous solution there are no HNO3 molecules. Only ions are present.
(b) (H^+)(OH^-) = 1E-14
(H^+) = 0.30. Solve for (OH^-)