Experimentally it was found that a metal oxide has formula M_0.98O. Metal M, present as M²⁺ and M³⁺ in its oxide.Fraction of the metal which exists as M³⁺ would be :

7.01%
4.08%
6.05%
5.08%

Solution

A gaseous hydrocarbon gives upon combustion 0.72 g of water and 3.08 g. of CO₂. The empirical formula of the hydrocarbon is :

C₂H₄
C₃H₄
C₆H₅
C₇H₈

Solution

Consider a titration of potassium dichromate solution with acidified Mohr’s salt solution using diphenylamine as indicator. The number of moles of Mohr’s salt required per mole of dichromate is

Solution

The molality of a urea solution in which 0.0100 g of urea,[(NH₂)₂CO] is added to 0.3000 dm3 of water at STP is:

45.55 × 10⁴m
33.3 m
3.33 × 10^–2 m
0.555 m

Solution

The density (in g mL–1) of a 3.60 M sulphuric acid solution that is 29% H₂SO₄(molar mass = 98 g mol^–1) by mass will be

1.45
1.64
1.88
1.22

Solution

Since molarity of solution is 3.60 M. It means 3.6 moles of H₂SO₄ is present in its 1 litre solution.
Mass of 3.6 moles of H₂SO₄ = Moles × Molecular mass= 3.6× 98 g = 352.8g
∴ 1000 ml solution has 352.8 g of H₂SO₄
29% H₂SO₄ by mass means 29g of H₂SO₄ is present in 100 g of solution.
∴ 352.8 g of H₂SO₄ is present in
\(\frac{100}{29}\) = 352.8 g of solution = 1216 g of solution

Density = \(\frac{Mass}{Volume}\) = \(\frac{1216}{1000}\) = 1.216 g/ml = 1.22 g/ml