What is the pH of a solution that has a [OH-] = 0.0033 M?

Question

6550 views around the world

You can reuse this answer
Creative Commons License

Answer 1 · 2018-04-19T01:31:49

#pH=11.52#

Here #[OH^-]=33xx 10^(-4)M#

#rArr pOH=-log_10[OH^-]#

#rArr pOH=-log_10[33xx10^(-4)]#

#rArr pOH=-log_10(33)-log_10(10^(-4))#

#rArr pOH=-1.52+4.00#

#rArr pOH=2.48#

We know that #pH+pOH=pK_w#............#{pK_w=14}#

#rArr pH+2.48=14#

#:.pH=11.52#