Determine the OH- of a solution that is 0.110M in F- [Solved]

Calculate [OH-]:

pH = 8.12

Supply(s): ChemTeam

Wed like the Ka of HF:

Supply(s): ChemTeam

Supply(s): ChemTeam

The reply on Mastering Chemistry was 1.8*10^-6=OH-

Maybe there was some rounding off that you just did otherwise or maybe the one who ready the reply used a special Kb than you probably did (or was supplied in the issue).

The reply on Mastering Chemistry was 1.8*10^-6=OH-

Calculate [OH-]:

The reply on Mastering Chemistry was 1.8*10^-6=OH-

Supply(s): ChemTeam

pH = 8.12

Maybe there was some rounding off that you just did otherwise or maybe the one who ready the reply used a special Kb than you probably did (or was supplied in the issue).

Kb = 1.5873 x 10^-11 (I will not hassle to spherical off but)

The proper reply is 1.7*10^-6M. First, write equilibrium F- H20 <=> HF H30 whole an ICE desk. Ka = 3.5*10^-4. However, have to make use of Kb price. To hunt out Kb use the connection Ka*Kb=Kw, the place Kw = 1.Zero*10^-14. Kb= 2.Eighty 5*10^-11. 2.Eighty 5*10^-11= x^2 / 0.10-x. Assume x is smaller than zero.100 (aka small x approximation). The OH- equals 1.Sixty eight*10^-6.

6.3 x 10^-4

This post is last updated on hrtanswers.com at Date : 1st of September – 2022

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