*fixed.It's because they react further with water.
Example one - the neutral salt NaCl
It is neutral because the salt does not further react of water in solution.
Na+ + H20 --> Na+ + H20
Cl- + H20 --> Cl- + H20 ---> No Hydronium/Hydroxide ions produced, therefore neutral
Example two - the basic salt NaCH3COO or CH3COONa (doesn't matter which way you write it)
Na+ + H20 --> Na+ + H20
CH3COO- + H20 --> CH3COOH + OH- ---> Hydroxide ions produced, therefore basic
Example three - the acidic salt NH4Cl
NH4+ + H20 --> NH3 + H30+
Cl- + H20 --> Cl- + H20 ---> Hydronium ions produced, therefore *acidic
Hehe, thanks for the pick up*fixed.
ThanksAmmonium nitrate methinks.
Thanks. Understand now. Much appreciated.It's because they react further with water.
Example one - the neutral salt NaCl
It is neutral because the salt does not further react of water in solution.
Na+ + H20 --> Na+ + H20
Cl- + H20 --> Cl- + H20 ---> No Hydronium/Hydroxide ions produced, therefore neutral
Example two - the basic salt NaCH3COO or CH3COONa (doesn't matter which way you write it)
Na+ + H20 --> Na+ + H20
CH3COO- + H20 --> CH3COOH + OH- ---> Hydroxide ions produced, therefore basic
Example three - the acidic salt NH4Cl
NH4+ + H20 --> NH3 + H30+
Cl- + H20 --> Cl- + H20 ---> Hydronium ions produced, therefore acidic
It's because they react further with water.
Example one - the neutral salt NaCl
It is neutral because the salt does not further react of water in solution.
Na+ + H20 --> Na+ + H20
Cl- + H20 --> Cl- + H20 ---> No Hydronium/Hydroxide ions produced, therefore neutral
Example two - the basic salt NaCH3COO or CH3COONa (doesn't matter which way you write it)
Na+ + H20 --> Na+ + H20
CH3COO- + H20 --> CH3COOH + OH- ---> Hydroxide ions produced, therefore basic
Example three - the acidic salt NH4Cl
NH4+ + H20 --> NH3 + H30+
Cl- + H20 --> Cl- + H20 ---> Hydronium ions produced, therefore acidic
Acetic acid is indeed a weak acid, but its degree of ionisation is extremely low (< 2%), so low that the hydroxide ions produced still make the solution much more basic than the small concentration of hydronium ions produced by the acetic acid would make it acidic. Therefore it's still acidic.i'm a bit confused. isn't CH3COOH acetic acid so it would be acidic
oh i just realised is it because u have Na+ and OH- which is a strong base so strong base plus weak acid gives weak base
Um yeh, there is 1.68 grams of KOH.....1)
[H+][OH-]=10^-14, but we know [H+]=100[OH-]
Thus we have 2 equations in 2 unknowns, which can be solved by substitution:
{100[OH-]}[OH-]=10^-14
100[OH-]^2=10^-14
[OH-]^2=10^-16
[OH-]=(10^-16)^0.5=10^-8
[H+]=10^-14/[OH-]=10^-14/10^-8=10^-6
pH=-log_10{[H+]}=-log_10{10^-6}=(-6)(-log_10{10})=(-6)(-1)(1)=6 I think...
2)
I think some words are missing:
"1.68 [missing word - 'grams' perhaps?] KOH..."