Practice Calculations:

Write out the known and unknown data first. Show all working and record answers to 3 significant figures.

1. An acid – base titration yielded the following information.

1.25.0 mL of a 0.250 molL-1solution of potassium hydroxide required 15.4 mL of sulfuric acid to be fully neutralised. Using the equation below calculate the concentration of the sulfuric acid in molL-1

2KOH + H2SO4 ® K2SO4 + 2H2O

2. An acid – base titration yielded the following information.

13.7ml of 0.250molL-1 HCl was required to fully neutralise 25ml of Ba(OH)2. Using the equation below calculate the concentration of the Ba (OH)2 in molL-1.

Ba(OH)2 + 2HCl ® BaCl2 + 2H2O

3. Aspirin, C9H8O4 , is made by reaction of:

Salicyclic Acid + Ethanoic anhydride à Aspirin + Ethanoic acid

C7H6O3 + C4H6O3 à C9H8O4 + C2H4O2

How many grams of ethanoic anhydride C4H6O3 are needed to make one aspirin tablet, which contains 0.33 g of aspirin?

4. When 4.78g of an oxide of lead are heated in a stream of hydrogen, 4.14g of lead are formed.

PbxOy + H2 à Pb + H2O

Determine the empirical formula of the lead oxide, PbxOy.

You need to work out the mass of the lead and oxygen so that you can determine the empirical formal of PbxOy

Help

The mass of lead, Pb in PbxOy = 4.14g

The mass of lead oxide, PbxOy = 4.78g

So mass of oxygen in PbxOy must be 4.78g - 4.14g = 0.64 g

n(Ba(OH)2) = 3.425 x 10‑3 mol = 1.7125 x 10-3 mol

c(Ba(OH)2) = = 0.0685molL-1

Q3)

M(C9H8O4) = 180 g mol-1

(i) n(C9H8O4) = m/M = 0.33 g / 180 g mol-1 = 1.83 x 10-3 mol

(ii) n(C4H6O3) = n(C9H8O4) = 1:1 mole ratio so

n(C4H6O3) 1.83 x 10-3 mol

(iii) m(C4H6O3) = 1.83 x 10-3 mol x 102 g mol-1 = 0.187 g

Q4)

Mass of lead oxide is 4.78g

Mass of lead is 4.14g

So mass of oxygen that is lost by the lead is worked out from

the mass of the PbO – mass of Pb

The mass of oxygen is 4.78g - 4.14g = 0.64 g

We don’t need the mass of H2 or H2O

i.e. PbO + H2 à Pb + H2O

(4.78g + 0.64 g) + H2 à 4.14g + H2O

i) n(Pb) = 4.14/207= 0.020 mol

(ii) m(O) = 4.78 - 4.14 = 0.64 g

(iii) n(O) = 0.64/16= 0.04 mol

(iv) Hence Pb : O = 1 : 2 and empirical formula is PbO2.

	Created by Bekky over 10 years ago

ncea level 3 chemistry (last internal/ titrations ) Note on practice calculations , created by Bekky on 23/08/2014.

practice calculations