Saved Bookmarks
| 1. |
Calculate the pH of 0.001M HCl solution HCl_(0.001M) leftrightarrow^(H_2O)H_3O_(0.001M)^(+)+Cl_(0.001M)^(-) |
|
Answer» Solution :`H_3O^+` from the auto ionisation of `H_2O(10^-7M)` is negligible when compared from `10^-3 M HCL` HENCE `[H_3O^+]=0.001 MOL dm^-3` `pH=-log_10[H_3O^+]` `=-log_(10)(0.001)` `=-log_10(10^-3)=3` |
|