What is volumetric analysis.

a) What meant by the term titration?

b) Outline types of titration.

a) Give the meaning of standard solution

b) Mention types of standard solution

c) What are the characteristics of primary standard solution.

a) What is indicator?

b) Outline types of indicator.

Mention indicator required for

i) Strong acid with weak base
ii) Strong acid with strong base
iii) Weak acid with strong base
iv) Weak acid with weak acid

What volume concentrated sulphuric acid is required to prepare 0.4m of 750ml dilute sulphuric acid. (given; mw = 98, density= 1.84g/cm³). H = 1

a) What is the titre volume?

b) consider the table below then find the titre volume.

0.4 m of dilute sulphuric acid was reacted with sodium carbonate in the experimental done in chemistry laboratory



i) Work out mean volume
ii) Write the balance chemical equation
iii) What is the number of moles for?

a. Base reacted
b. Acid reacted

The experiment was done by reacting 25ml of 0.1 M sodium hydroxide with hydrochloric acid.
The product formed were sodium chloride and water.
The burette reading was 25ml.
Calculate the molarity of hydrochloric acid.

Define the following terms

a) End point
b) Secondary standard solution
c) Equivalent weight of an acid
d) Equivalent weight of a base
e) Basicity

a) what is basicity?

b) Classify the following compound basing on basicity

i. HCl
ii. H₂SO₄
iii. H₃PO₄

a) What do you mean by 0.4 M solution

b) Define the terms

i. concordant readings
ii. concentration

a) Molar mass means what?

b) Find the molar mass of the following

i. hydrochloric acid
ii. sodium hydroxide
iii. sulphuric acid
iv. carbon dioxide
v. Sulphur trioxide

How many grams in 99% pure sulphuric acid solution?

Calculate the percentage purity of the sample of the 12.0g sample acid with 11.57g of active acid in a sample.

Sodium chloride was prepared by neutralizing sodium hydroxide solution with dilute hydrochloric acid. The solution was gently heated to evaporate most of the water and allow the salt to crystallize. The crystals were separated from any remaining solution and dried on a father paper. However, the crystals are not necessarily completely dry. The salt may be required to be completely anhydrous, that is not containing any water. The prepared salt was analyzed for water by heating a sample in an oven at 110^OC to measure the evaporation of water residual. Calculate the percentage of purity of the salt.

What is the percentage purity of a sample of CaCO₃ if 150g of the sample gives out 44g of CO₂ on heating?

a) What meant by the following terms

i. hydrous
ii. anhydrous

b) 5g of hydrated magnesium sulphate was placed in crucible at 100^oC. After five (5) minutes, the 2g of water was evaporated.
Find:
i) mass of hydrous,
ii) mass of anhydrous salt,
iii) percentage of anhydrous.

a) A commercial sulphuric acid usually labeled as 98% of the acid by weight and having the density of 1.84g/cm³

i. Calculate the molarity of this industrial acid
ii. What volume of this acid that will be required to prepare 2dm³ of 0.5M Sulphuric acid?

b) Name the indicator you would choose for the following titraions.

i. Hydrochloric acid versus ammonia solution.
ii. Acetic acid versus sodium hydroxide.