1. What is the (i) Molarity, (ii) Normality and (iii) % w/v of a solution containing 13.5 mL of conc. H2SO4 (98% w/w; sp

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1. What is the (i) Molarity, (ii) Normality and (iii) % w/v of a
solution containing 13.5 mL of conc. H2SO4 (98% w/w; sp.gr 1.8)
dissolved in and made up to 750ml with distilled water?
2. A solution was prepared by dissolving 45.0g of solid KOH and
diluting to 1.0L with distilled water. A 25 mL aliquot of the above
H2SO4 solution required 27 mL of the KOH solution to titrate it to
the phenolphthalein end point. Assuming the H2SO4 concentration to
be exactly as calculated in (B) above, calculate the purity (% w/w)
of the solid KOH
3. Show that for a solution of a weak acid, that [H+ ] =
√(𝐾𝑎.𝐶) where Ka is the acid dissociation constant and C is the
concentration of acid in mol/L.
Calculate the concentration of lactic acid in a solution having
a pH value of 2.73 (pKa for lactic acid = 3.86). If the solution is
titrated with a NaOH solution of the same concentration what will
be the pH value at the equivalence point.
4. What weights of which of the K-salts of H3PO4 are
required to prepare 1.0 L of a K- phosphate buffer, pH 7.0 and
ionic strength of 0.025 M.
H3PO4 K1 = 7.52x10-3
K2 = 6.23x10-8
K3 = 5.0x10-13