6B.5d

Moderators: Chem_Mod, Chem_Admin

Alicia Lin 2F
Posts: 83
Joined: Wed Sep 18, 2019 12:17 am

6B.5d

Postby Alicia Lin 2F » Mon Jan 13, 2020 9:53 pm

Calculate the pH and pOH of each of the following aqueous solutions of a strong acid or base:
(d) 2.00 mL of 0.175M KOH(aq) after dilution to 0.500 L

I'm not really sure how to approach this problem.

Isha_Maniyar_Dis2E
Posts: 110
Joined: Thu Jul 11, 2019 12:16 am

Re: 6B.5d

Postby Isha_Maniyar_Dis2E » Mon Jan 13, 2020 10:05 pm

First find the number of moles of KOH in 2 mL of 0.175M solution. Then, divide by 0.500 L to find the concentration of KOH. The concentration of KOH equals the concentration of OH- in the solution because KOH is a strong base and will dissociate completely into K+ and OH- ions. So, you can find pOH by simply calculating the following: -log[OH-]

Once you have found this value, subtract it from 14 to find pH (pH + pOH = 14, so pH = 14 - pOH).

Hope this helped!

805422680
Posts: 103
Joined: Sat Sep 14, 2019 12:16 am

Re: 6B.5d

Postby 805422680 » Mon Jan 13, 2020 11:26 pm

find moles of OH- ions in 2ml of 0.175M KOH. Divide this value to obtain concentration of OH- ions. use the formula of pOH to calculate the pOH of solution and then subtract by 14 to calculate the pH


Return to “Equilibrium Constants & Calculating Concentrations”

Who is online

Users browsing this forum: No registered users and 2 guests