have a few more questions..
1) ammonia is a weak bronsted lowry base of Kb value of 1.78x
10^-5 moldm-3
a 25.0cm3 sample of aqueous ammmonia was placed in a conical
flask, when titrated against the 0.200moldm-3 hydrochloric acid,
17.50cm3 of acid was required for complete neutralization.
how to calculate the pH at the equivalence pt of the
titration?
2) Solution X contains 0.100moldm-3 calcium chloride and 0.100
moldm-3 barium chloride. Predict and explain, with the aid of
relevant calculations, what would happen when equal volumes of
solution x and 0.00500moldm-3 sodium floride are mixed together
3) State and explain how the solubility of barium floride would
change if it is dissolved in an aqueous solution of KF
Tips :
Q1) Do ICF (Initial Change Final) and ICE (Initial Change
Equilibrium), then use Ka expresion (for proton dissociation from
the conjugate acid ammonium cation) to find [H+] and thus pH.
Q2) The question lacks Ksp data. But predictably, calcium
fluoride will be selectively precipitated over barium fluoride.
Support your answer with calculations involving ionic and
solubility products for both ionic compounds.
Q3) Explani using Le Chatelier's principle and common ion
effect. Molar/Mass solubility of barium fluoride will decrease.
