The textbook said if you add dry ice (carbon dioxide) to lemonade or soda water, the pH of the substance (which is already acidic) will become even more acidic. Why?
Does the weak cabonic acid form in the process?It's actually CO2 + H2O <--> H3O+ + HCO3- (HCO3- is an ampholyte, however, I recall that essential chemistry is that of a base and sometimes employed to neutralize various types of acid solutions).
Carbon acid (H2CO3) is actually not a very weak acid (its Ka is not that small). The pH of carbonic acid is usually pretty low because (i) the solubility product for CO2 in water is low, and (ii) only a small fraction of the dissolved CO2 forms H2CO3. But among the H2CO3 that forms, a relatively significant fraction (nowhere near a majority, but a bigger fraction than HF) dissociates to H+ and (HCO3)- and a very tiny fraction of the (HCO3)- further dissociates into H+ and (CO3)2-.Does the weak cabonic acid form in the process?
ADD THE FOLLOWING REACTIONSSo this
H2CO3 + H2O ->HCO3- + H3O+ is more likely
H2CO3 -> CO2 + H2O
CO2 + H2O -> H2CO3 + H2O -> HCO3- + H3O+
This is not what I said. In fact, such a statement actually makes no sense from a chemistry point of view. The correct way to talk about reactions is to discuss the equilibrium conditions and the kinetics that lead to it. At equilibrium, the H2CO3 is as likely to make H2O + CO2 (in a given window of time) as the reverse reaction (by definition).BartDT, I haven't really learnt what you wrote but I will post what I have realised from what people like Gokul and GT have said:
It is more likely for H2CO3 to form H2O+CO2 than vice versa