Calculae the mass of 0.1 mole of each of the following :
(a) $C a C O_{3}$ ,

(b) $N a_{2} S O_{4} . 10 H_{2} O,$
(c) $C a C l_{2},$

(d) Mg.

(Ca = 40, Na = 23, Mg = 24, S= 32, C= 12, Cl = 35.5, 0 = 16, H = 1 )

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Solution

(a) 0.1 mole of $C a C O_{3}$ has mass =100(molar mass) $\times$ 0.1=10 g
(b) 0.1 mole of $N a_{2} S O_{4} . 10 H_{2} O$ has mass = 322 $\times$ 0.1 = 32.2 g
(c) 0.1 mole of $C a C l_{2}$ has mass = 111 $\times$ 0.1 = 11.1g
(d) 0.1 mole of Mg has mass = 24 $\times$ 0.1 = 2.4 g

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Q. Calculate the molecular mass of the following:

(N H_{4})_{2} C O_{3}

Given: atomic mass of

N a = 23, H = 1, O = 16, C = 12, N = 14, M g = 24, S = 32

A water contains the following dissolved ions.
$[N a^{+}] = 56 m g / L; [C a^{2 +}] = 40 m g / L;$
$[M g^{2 +}] = 30 m g / L; [A l^{3 +}] = 3 m g / L;$
$[H C O_{3}^{-}] = 190 m g / L; [C l^{-}] = 165 m g / L;$
Water $p H$ is $7$ .
Atomic weights:
$C a = 40, M g = 24, A l = 27, H = 1, C = 12, O = 16, N a = 23, C l = 35.5$

The non-carbonate hardness of the sample in $m g / L$ as $C a C O_{3}$ is

Q. Ion concentrations obtained for a groundwater sample (having

p H = 8.10

) are given below.

Ion	$C a^{2 +}$	$M g^{2 +}$	$N a^{+}$	$H C O_{3}^{-}$	$S O_{4}^{2 -}$	$C l^{-}$
Ion concentration $(m g / L)$	$100$	$6$	$15$	$250$	$45$	$39$
Atomic weight	$C a = 40$	$M g = 24$	$N a = 23$	$H = 1$ $C = 12$ $O = 16$	$S = 32$ $O = 16$	$C l = 35.5$

Total hardness

(m g / L a s C a C O_{3})

present in the above water sample is

Q. Which of the following compound has formula mass of 322 u?

(H = 1, C = 12, 0 = 16, N a = 23, S = 32, C u = 63.5)

Calculate the relative molecular masses of (Use K = 39, Cl = 35.5, O = 16, C = 12, H = 1, Na = 23, N = 14, S = 32)
(a) potassium chlorate
(b) sodium acetate
(c) chloroform
(d) ammonium sulphate

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Calculae the mass of 0.1 mole of each of the following : (a) CaCO3 , (b) Na2SO4.10H2O, (c) CaCl2, (d) Mg. (Ca = 40, Na = 23, Mg = 24, S= 32, C= 12, Cl = 35.5, 0 = 16, H = 1 )

(a) 0.1 mole of CaCO3 has mass =100(molar mass) × 0.1=10 g (b) 0.1 mole of Na2SO4.10H2O​​​​​​​ has mass = 322 × 0.1 = 32.2 g (c) 0.1 mole of CaCl2​​​​​​​ has mass = 111 × 0.1 = 11.1g (d) 0.1 mole of Mg has mass = 24 × 0.1 = 2.4 g

Calculae the mass of 0.1 mole of each of the following :
(a) $C a C O_{3}$ ,

(b) $N a_{2} S O_{4} . 10 H_{2} O,$
(c) $C a C l_{2},$

(d) Mg.

(Ca = 40, Na = 23, Mg = 24, S= 32, C= 12, Cl = 35.5, 0 = 16, H = 1 )

(a) 0.1 mole of $C a C O_{3}$ has mass =100(molar mass) $\times$ 0.1=10 g
(b) 0.1 mole of $N a_{2} S O_{4} . 10 H_{2} O$ has mass = 322 $\times$ 0.1 = 32.2 g
(c) 0.1 mole of $C a C l_{2}$ has mass = 111 $\times$ 0.1 = 11.1g
(d) 0.1 mole of Mg has mass = 24 $\times$ 0.1 = 2.4 g