What is the #pH# of a mass of #4.66mg# of barium hydroxide dissolved in a #1L# volume of water?

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Answer 1 · 2016-10-26T19:23:10

#pH=9.74#

We need to find (i), #[HO^-]# #=# #(2xx4.66xx10^-3g)/(171.34*g*mol^-1)xx1/L# #=# #5.44xx10^-5mol*L^-1#.

And (ii), #pOH# #=# #-log_10[HO^-]# #=# #-log_10(5.44xx10^-5)# #=# #4.26.#

And since (iii) #pH+pOH=14, pH=14-4.26=9.74#.

What is the #pH# of a mass of #4.66*mg# of barium hydroxide dissolved in a #1*L# volume of water?