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OlgaM077 [116]
3 years ago
5

Sodium carbonate (NaCO3) is sometimes used as a water-softening agent. Suppose that a worker prepares a 0.730 M solution of NaCO

3 and water. The volume of the solution is 1.421 liters. What is the mass of solute in the solution?
Chemistry
2 answers:
sergey [27]3 years ago
5 0

The molarity of a solution is the number of moles of a substance divided by the volume in liters prepared.

molarity=\frac{n}{V}, where n is number of moles and V is the volume in liters.

In order to calculate the mass of solute we need to convert the volume and molarity to moles

1.421 L solution \times\frac{0.0730 moles}{1 Lsolution}= 1.037 mol NaCO_3

Now that we have moles we use the relative formula mass of NaCO₃, We have 1 Na atom, 1 C atom and 3 O atoms, thus

M_r= (1\times 22.99) + (1\times 12.00) + (3\times 16.00)= 82.99g/mol

1.037 \times\frac{82.99g}{mol} = 86.1g

Luda [366]3 years ago
5 0

Answer is: the mass of solute in the solution is 110 grams.

c(Na₂CO₃) = 0.730 M; molarity of sodium carbonate solution.

V(Na₂CO₃) = 1.421 L; volume of solution.

n(Na₂CO₃) = c(Na₂CO₃) · V(Na₂CO₃).

n(Na₂CO₃) = 0.73 mol/L · 1.421 L.

n(Na₂CO₃) = 1.037 mol; amount of solute.

M(Na₂CO₃) = 106 g/mol; molar mass of sodium carbonate.

m(Na₂CO₃) = n(Na₂CO₃) · M(Na₂CO₃).

m(Na₂CO₃) = 1.037 mol · 106 g/mol.

m(Na₂CO₃) = 110 g; mass of sodium carbonate.

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\large \boxed{\text{-827.4 kJ}}

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2. S(s, rhombic)  + O₂(g)   ⟶ SO₂(g);                                 ∆H = -296.8 kJ

3. PbO(s)             + H₂S(g) ⟶ PbS(s)               + SO₂(g);    ∆H =  -104.3 kJ

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When you reverse an equation, you reverse the sign of its ΔH.

When you double an equation, you double its ΔH.

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Equation 5 has 2H₂O on the left. That is not in the target equation.

You need an equation with 2H₂O on the right, so you copy Equation 1.  

6. 2H₂S(g) + O₂(g) ⟶ 2S(s, rhombic) + 2H₂O(g) ; ∆H = -442.4 kJ  

Equation 6 has 2S(s, rhombic) on the right. That is not in the target equation.

You need an equation with 2S(s, rhombic) on the left, so you double Equation 2.  

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When you add equations, you add their ΔH values.

You get the target equation 4:

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4 . 2PbS(s) + 3O₂(g)      ⟶ 2PbO(s) + 2SO₂(g); ΔH = -827.4 kJ

\Delta H \text{ for the reaction is $ \large \boxed{\textbf{-827.4 kJ}}$}

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