1. This is a buffer solution. Use the Henderson-Hasselbalch equation.
2. This is made to look like a buffer solution but it isn't. Calculate OH from the Ba(OH)2 concn.
Post your work if you get stuck.
calculate [h3o] in solutions. 0.040 of HCl and 0.080 HOCl.
2. calculate OH for the solutions of 0.0063 ba (OH)2 and 0.0110 of BaCl2
5 answers
thank you. for #1, do i just get the PH and then covert that to H3O then?
but if HCL and HOCl are both strong acids, how can i use the equation? since its supposed to be an acid and base right?
No. I'm glad you asked the question because it made me look at the problem again. I gave you a bum way to go. This is not a buffered solution, it is the solution of a strong acid (HCl) and a weak acid (HOCl). What you do here is to calculate the H3O^+ from the strong acid, then the H3O^+ from the weak acid, add the moles together and divide by the volume to determine molarity. I suspect, however, that the contribution by HOCl will be very small, perhaps even negligible.
After reading your second response, HOCl is a weak acid. You can determine the Ka by looking in tables in your text or your notes.
1 answer