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Anton [14]
3 years ago
7

If 0.500 mol of each of the following solutes is dissolved in 2.0 L of water, which will cause the greatest increase in the boil

ing point of the solution? A. NaCl B. KI C. CO2 D. Na2SO4
Chemistry
2 answers:
serious [3.7K]3 years ago
8 0

Answer is: D. Na2SO4.

b(solution) = 0.500 mol ÷ 2.0 L.

b(solution) = 0.250 mol/L.

b(solution) = 0.250 m; molality of the solutions.

ΔT = Kf · b(solution) · i.

Kf - the freezing point depression constant.

i - Van 't Hoff factor.

Dissociation of sodium sulfate in water: Na₂SO₄(aq) → 2Na⁺(aq) + SO₄²⁻(aq).

Sodium sulfate dissociates on sodium cations and sulfate anion, sodium sulfate has approximately i = 3.

Sodium chloride (NaCl) and potassium iodide (KI) have Van 't Hoff factor approximately i = 2.

Carbon dioxide (CO₂) has covalent bonds (i = 1, do not dissociate on ions).

Because molality and the freezing point depression constant are constant, greatest freezing point lowering is solution with highest Van 't Hoff factor.

arlik [135]3 years ago
7 0

Answer: D. Na_2SO_4

Explanation:

\Delta T_b=i\times K_b\times m

\Delta T_b = change in boiling point

i= vant hoff factor = no of ions produced on complete dissociation

K_b = boiling point constant

m= molality =\frac{\text{moles of solute}}{\text{weight of solvent in kg}}=\frac{0.5}{2kg}=0.25m =same for all solutes

1. For NaCl:

NaCl\rightarrow Na^++Cl^-

i=2

2. For KI ,

KI\rightarrow K^++I^-

i=2

3. CO_2 , i= 1 as it does not dissociate

4. For Na_2SO_4 ,

Na_2SO_4\rightarrow 2Na^++SO_4^{2-}

i=3

Thus elevation in boiling point will be highest in Na_2SO_4 solution.

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Liters of a 2.40 M
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Answer:

1.42 L

Explanation:

Step 1:

The following data were obtained from the question :

Molarity of KBr = 2.40 M

Mole of KBr = 3.40 moles

Volume of solution =?

Step 2:

Determination of the volume of the solution.

Molarity of solution is simply the mole of the solute per unit volume the of solution. It is given as :

Molarity = mole /Volume

Volume = mole /Molarity

Volume = 3.4/2.4

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Write out a balanced, molecular equation, total ionic equation, and net ionic equation for each:
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How many atoms does 2.0 moles of He represent
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We use the following formula to calculate the number of atoms:

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In a certain electrolysis experiment, 1.24 g of Ag were deposited in one cell (containing an aqueous AgNO3 solution), while 0.65
eduard

Answer:

The correct answer is 169.56 g/mol.

Explanation:

Based on the given information, the mass of Ag deposited is 1.24 g, and the mass of unknown metal X deposited in another cell is 0.650 g. The number of moles of electrons can be determined as,

= 1.24 g Ag * 1mol Ag/107.87 g/mol Ag * 1 mol electron/1 mol Ag ( the molecular mass of Ag is 107.87 g/mol)

= 0.0115 mole of electron

The half cell reaction for the metal X is,  

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From the reaction, it came out that 3 faraday will reduce one mole of X^3+.  

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3 years ago
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