If I add 1000 mg of CaCO3 to 25 ml of water, I achieve an experimental pH around 9, how can I prove this mathematically? If I then add 25 ml of 0.1 N HCl, I achieve a pH of about 7.5, how can I prove this mathematically?
The possible concentration of CO32- is 5.8x10-5 mol/L . CO32- + HOH = HCO3- + OH- [OH-] = 5.8x10-5 mol/L pOH = - lg[OH-] ≈ 4.3. pH = 14 – pOH = 14 – 4.3 ≈ 9.7
n (HCl) = 0.1 N ∙ 0.025 L = 0.0025 mol This quantity reacts completely with 1g of CaCO3. The salt is in excess! So if you wait till the end of the reaction the pH won’t change!
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