In: Chemistry
a) What is the final proudct of polyphosphonate hydrolysis?
b) HCl in natural water can react with solid CaCO3 and increase the hardness and alkalinity in water. What reaction shows how HCl increases the hardness of water and its alkalinity? If 1 mM HCl is present as an anthropogenic contaminant in water with solid CaCO3, what is the hardness of water after equilibration?
a) The end product of Hydrolysis of Polyphosphonates typically depends on the extent of Hydrolysis and lenght of the polyphosophonate chain.
Typically the end products are Ortho phosphates (PO4) if the hydrolysis is complete or it shall be condensed (smaller) polyphosphates if it is a long Polyphosphonate chain,.
Part B - Explaination
Part C Calculation
What is the hardness of Water after Equilibration:
To answer this part of question all the chemical equations that exist in equilibrium are to be solved:
1. Ca2+(aq) + CO32-(aq) <-> CaCO3(s)
2. CO32-(aq) + H+(aq) <-> HCO-3aq) + H+(aq) <-> H2CO3(aq) <-> H2O + CO2 (g)
For simplicity we ignore the equilibrium between H2CO3 (Aqueous) and CO2 (Gaseous phase) and the second equilibrium between HCO3-(aq) and H2CO3(aq) as the ka (10^-10.25) for the diprotic acid is very low.
If in the equilibrium concentration of CO32- is x and Concentration of HCO3- y
Concentration of Ca2+ in Solution = x+y
From chemical equation 2 y = 10^-3 moles (Total amount of bicarbonate produced = Total amount of acid consumed).
Ionic Product of CaCO3 in solution = x * (x+y)
= x * (10^-3+x)
Since the solution shall be saturated at equilibrium
Ionic Product = Solubility product (Ksp)
Ksp of CaCO3 = 6 X 10 ^-9
So total Calcium in the solution = x+y = 10^-3+ 6*10^-6
= 10^ -3 mol/lit(Approx.)
Hardness = 40 x 10^-3 *10^3 mg/lit as Cas
= 40 gm/lit as Ca
= 40/20*50 gm/lit as CaCO3
Hardness = 100 ppm as CaCO3