0

Guest

Courses New

Determine the pH of solution that results from the addition of 20 ml, 0.01 M ca(0H)2 to 30ml of 0.01M HCl.

Determine the pH of solution that results from the addition of 20 ml, 0.01 M ca(0H)2 to 30ml of 0.01M HCl. 
 

Grade:12

1 Answers

Arun
25750 Points
5 years ago
Ca(OH)is a strong  base and HCL is a strong acid,therefore it is a strong acid reaction.The reaction will be
H+(aq)+OH-(aq)→H2O(l)
The original no. of moles of H+ in the solution is
30×10^-3 L×0.01M HCL=3×10^-4Mole
The number of moles of OH- added is 20×10^-3L×0.01M HCL=2×10^-4 moles
the resultant moles of H+ is 
3×10^-4-2×10^-4 moles H+(aq)
the total volume of solution=20ml+30ml=50ml=5×10^-3L
(H+)=1×10^-4/5×10^-3=0.02
pH=-log(H+)
=-Log(0.02)
=1.698
 

Think You Can Provide A Better Answer ?

Other Related Questions on Physical Chemistry

View all Questions »

ASK QUESTION

Get your questions answered by the expert for free

Answer and earn gift vouchers

Win Gift vouchers upto Rs 500/-

View courses by askIITians

Design classes One-on-One in your own way with Top IITians/Medical Professionals

Click Here Know More

Complete Self Study Package designed by Industry Leading Experts

Click Here Know More

Live 1-1 coding classes to unleash the Creator in your Child

Click Here Know More

a Complete All-in-One Study package Fully Loaded inside a Tablet!

Click Here Know More