[johnnyjohn993123]

Given that I have 120mL  of 0.007M  Acetic acid what will be the pH if I were to add 20ml of 3M HCl?


Am I gonna do an ice tble for this if so here is what I'll do:
      HOAc             H⁺                    +    OAc^-
I     8.4x10^-3              0.06mol                     0       
C        -x                         +x                                +x

E    8.4x10^-3 -x      0.06+x                            x


Ka=1.75 x10^-5

Ka=  (0.06 +x)(x)/ (8.4x10^-5-x)

x= 2.45x10^-8
[H⁺] = 0.06+ 2.45x10^-8
                       =0.060 M
pH= -log[H⁺]
pH=1.22

Its this even correct>>>?

[AWK]

Forget acetic acid is present in calculation and take into account dilution of HCl.

[johnnyjohn993123]

Forget acetic acid is present in calculation and take into account dilution of HCl.

How can I start by doing that?
MV=MV thingy??

[AWK]

Just calculate H⁺ (H₃O⁺) after dilution of HCl.

[Borek]

How can I start by doing that?
MV=MV thingy??

Yes. That's how you deal with dilutions, don't you?

[johnnyjohn993123]

Mv =Mv

(3M)(0.02) * ( M) ( 0.120)
M = 5 ?? NOW what is this even correct ? The dilution of HCl

[AWK]

No, still wrong. You mix two solutions. What is a final volume?

[johnnyjohn993123]

No, still wrong. You mix two solutions. What is a final volume?

MV=MV

(3 M)(0.02)= (M)(0.02+0.120)

M=0.429 M   

pH= -log 0.429 
pH= 0.368  ? LIke that?

[AWK]

Perfectly