When excess lead nitrate solution was added to a solution of sodium sulphate, 15.15 g of lead sulphate were precipitated.

What mass of sodium sulphate was present in the original solution?

Na₂SO₄ + Pb(NO₃)₂ → PbSO₄ + 2NaNO₃

[Na = 23, S = 32, O = 16, Pb = 207, N = 14]

2.4 g

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7.1 g

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5.0 g

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4.8 g

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3.5 g

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Solution

The correct option is B
7.1 g

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Similar questions

(a) If 112 cm³ of hydrogen sulphide is mixed with 120 cm³ of chlorine at STP, what is the mass of sulphur formed?
H₂S + Cl₂ $\overset{}{\to}$ 2HCl + S
(b) Washing soda has the formula Na₂CO₃·10H₂O. What is the mass of anhydrous sodium carbonate left when all the water of crystallization is expelled by heating 57.2 g of washing soda?
(c) When excess lead nitrate solution was added to a solution of sodium sulphate, 15.1 g of lead sulphate was precipitated. What mass of sodium sulphate was present in the original solution?
Na₂SO₄ + Pb(NO₃)₂ $\overset{}{\to}$ PbSO₄ + 2NaNO₃
(H = 1; C = 12; O = 16; Na = 23; S = 32; Pb = 207)

Q. 10 g of a mixture of sodium chloride and anhydrous sodium sulphate is dissolved in water. An excess of barium chloride solution is added and 6.99 g. of barium sulphate is precipitated according to the equation :-

N a_{2} S O_{4} + B a C l_{2} ⟶ B a S O_{4} + 2 N a C l

.
The percentage of sodium sulphate in the original mixture is:

[N a = 23, O = 16, S = 32, B a = 132]

10 g of a mixture of barium chloride and anhydrous sodium sulphate is dissolved in water. An excess of barium chloride solution is added and 6.99 g of barium sulphate is precipitated according to the equation given below:

Na₂SO₄ + BaCl₂ → BaSO₄ +2NaCl

[O = 16, Na = 23, S = 32, Ba = 137]

Calculate the percentage of sodium sulphate in the original mixture.

Q. When 11.25 moles of lead nitrate are made to react with 2.5 moles of chromic sulphate, precipitation of lead sulphate takes place. Calculate the moles of

C r (N O_{3})_{3}

formed in the final solution. Assume that lead sulphate is completely insoluble.
(Molar mass of lead - 207 g/mol)

Q. Sodium hydroxide solution is added first in a small quantity, then in excess to the aqueous salt solution of copper (II) sulphate, zinc nitrate, lead nitrate, calcium chloride and iron (III) sulphate. Copy the following table and write the colour of the precipitate in (i) to (v) and the nature of the precipitate (soluble or insoluble) in (vi) to (x).

Aqueous salt solution	Colour of precipitate when NaOH is added in a small quantity	Nature of precipitate (soluble or insoluble) when NaOH is added in excess
Copper (II) sulphate Zinc nitrate Lead nitrate Calcium chloride Iron (III) sulphate	(i) (ii) (iii) (iv) (v)	(vi) (vii) (viii) (ix) (x)

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When excess lead nitrate solution was added to a solution of sodium sulphate, 15.15 g of lead sulphate were precipitated. What mass of sodium sulphate was present in the original solution? Na2SO4 + Pb(NO3)2 → PbSO4 + 2NaNO3 [Na = 23, S = 32, O = 16, Pb = 207, N = 14]

The correct option is B 7.1 g

When excess lead nitrate solution was added to a solution of sodium sulphate, 15.15 g of lead sulphate were precipitated.

What mass of sodium sulphate was present in the original solution?

Na₂SO₄ + Pb(NO₃)₂ → PbSO₄ + 2NaNO₃

[Na = 23, S = 32, O = 16, Pb = 207, N = 14]

The correct option is B
7.1 g