1) In the titration of a solution of weak monoprotic acid with a 0.1150 M soluti

Question

1) In the titration of a solution of weak monoprotic acid with a 0.1150 M solution of NaOH, the pH half way to the equivalence point was 4.46 . In the titration of a second solution of the same acid, exactly twice as much of a 0.1150 M solution of NaOH was needed to reach the equivalence point. what was the pH half way to the equivalence point in this titration? 2) Antacid tablets contain a variety of bases such as NaHCO3, MgCO3, CaCO3 and Mg(OH)2, Only NaHCO3 has appreciable solubility in water. write a net ionic equation for the reaction of each antacid with aqueous HCl. include the state of each species. a)MgCO3 b)CaCO3 c)Mg(OH)2

Explanation / Answer

pH = pka + log [salt]/[acid]  

HA + NaOH <------> NaA + H2O

at hafl way [salt]= [acid]

hence for solution 2 also pH = 4.46 at half way

2) a) 2H+(aq) + MgCO3(s) ------> Mg2+(aq) + H2O(l) + CO2(g)

b) 2H+ (aq) + CaCO3 (s) -----> Ca2+(aq) + H2O (l) + CO2(g)

c) 2H+(aq) + Mg(OH)2 (s)----------> 2H2O + Mg2+(aq)

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