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A Solution Has A PH Of 3.4.What Is Its Hydrogen Ion Concentration?
![DrBob222](/images/users/0/1/128x128.jpeg)
pH = -log(H^+)
Substitute and solve.
![Emma](/images/users/0/1/128x128.jpeg)
45.1
![Emma](/images/users/0/1/128x128.jpeg)
0.000398
![Emma](/images/users/0/1/128x128.jpeg)
I put 45.1 as an answer to a different question. The real answer is 0.000398.
![Yo](/images/users/0/1/128x128.jpeg)
wsp
![Usman](/images/users/0/1/128x128.jpeg)
A solution has a pH 3.4 what is the hydrogen concentration
![Usman](/images/users/0/1/128x128.jpeg)
A solution has a pH of 3.4 whant is the hydrogen concentration
![precious](/images/users/0/1/128x128.jpeg)
pH =-log (h+
pH =-log (3.4)
pH = -(3.4)
pH =-3.4
![Isan](/images/users/0/1/128x128.jpeg)
The explanation is not clear
![C.R.7](/images/users/0/1/128x128.jpeg)
The pH of a given solution is 3.4. what's the ht
![Christabel](/images/users/0/1/128x128.jpeg)
4*10^-4
![Christabel](/images/users/0/1/128x128.jpeg)
Since pH is equal to _logbase10 (H +)
We have 3.4 =_log(h+)
There4 log [h+]=-3.4=-4.0+0.6=4.6
There4 [H+]= anti log 4.6
= 4*10^4 mol dm^-3
![Figbele](/images/users/0/1/128x128.jpeg)
How do you solve for the H+ that gave you4.0+0.6 that's confusing
![Ssam](/images/users/0/1/128x128.jpeg)
Did you just copy from New school chemistry, page 105? How did 3.4 become 4.6?
![Michael Ifeoluwa](/images/users/0/1/128x128.jpeg)
pH =-log (3.4)
Log10[H+]= -(3.4)
[H+] = antilog -3.4
= 0.000398 mol dm-3
![Catherine](/images/users/0/1/128x128.jpeg)