Calculate the pH of a 4.00 x 10^-2 mol dm^-3 solution of Ba(OH)2

The easiest way to answer this question is by using the equation pH + pOH = 14. 

Firstly, we need to work out the number of moles of OH- in the solution. As the formula for Ba(OH)2  shows that it has 2 moles of OH- for every 1 mole of Ba+ , the number of moles of OH- ions will be equal to twice the concentration of the solution. 

Therefore, there are 8.00 x 10-12 moles of OH- ions in the solution.

As pOH= -log (OH-), pOH = -log (8.00 x 10-12

Therefore pOH= 1.097

By rearranging the formula pH + pOH = 14, we get 14-pOH= pH

Therefore, 14-1.097= 12.9

The pH of the solution is 12.9

Answered by Chloe M. Chemistry tutor

12391 Views

See similar Chemistry IB tutors

Related Chemistry IB answers

All answers ▸

Please use the VSEPR theory to predict the shape of NH3 and the approximate bond angles


Which are four factors affecting the rate of a chemical reaction and how do these affect the rate constant of the reaction?


What is the intermolecular force involved in secondary protein structure?


How can we determine the molecular and electron geometry of H2O?


We're here to help

contact us iconContact usWhatsapp logoMessage us on Whatsapptelephone icon+44 (0) 203 773 6020
Facebook logoInstagram logoLinkedIn logo

© MyTutorWeb Ltd 2013–2025

Terms & Conditions|Privacy Policy
Cookie Preferences