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kotegsom [21]
3 years ago
9

An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of calcium nitrate. The net ionic equation

contains which of the following species (when balanced in standard form)
Chemistry
1 answer:
Veseljchak [2.6K]3 years ago
4 0

The complete question is:

An aqueous solution of ammonium sulfate is allowed to react with an aqueous solution of calcium nitrate.

The net ionic equation contains which of the following species (when balanced in standard form)?

a. 2NO3-(aq)

b. Ca2+(aq)

Answer:

b. Ca2+(aq)

Ca2+ (aq) + SO4^2-(aq) --------------> CaSO4(s)

Explanation:

The overall ionic equation is:

Ca2+(aq) + 2NO3-(aq) + 2NH4+(aq) + SO4^2-(aq) ---------------> CaSO4(s) + 2NH4NO3(aq)

The NO3- and NH4+ are spectator ions as they do not participate in the formation of the precipitate CaSO4.

The net ionic equation is:

Ca2+ (aq) + SO4^2-(aq) --------------> CaSO4(s)

The spectator ions form the soluble ammonium trioxonitrate V

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3 years ago
The mole fraction of a non-electrolyte (MM 40.0 g/mol) in a saturated aqueous solution is 0.310. What is the molality of the sol
jeka57 [31]

<u>Answer:</u> The molality of non-electrolyte is 24.69 m

<u>Explanation:</u>

We are given:

Mole fraction of saturated aqueous solution = 0.310

This means that 0.310 moles of non-electrolyte is present.

Moles of water (solvent) = 1 - 0.310 = 0.690 moles

To calculate the mass from given number of moles, we use the equation:

\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}

Moles of water = 0.690 moles

Molar mass of water = 18 g/mol

Putting values in above equation, we get:

0.690mol=\frac{\text{Mass of water}}{18g/mol}\\\\\text{Mass of water}=(0.690mol\times 18g/mol)=12.42g

To calculate the molality of solution, we use the equation:

\text{Molality}=\frac{n_{solute}\times 1000}{W_{solvent}\text{ (in grams)}}

Where,

n_{solute} = Moles of solute (non-electrolyte) = 0.310 moles

W_{solvent} = Mass of solvent (water) = 12.42 g

Putting values in above equation, we get:

\text{Molality of non-electrolyte}=\frac{0.310\times 1000}{12.42}\\\\\text{Molality of non-electrolyte}=24.96m

Hence, the molality of non-electrolyte is 24.69 m

4 0
3 years ago
How to balance this equation NH4OH+H3PO4=(NH4)3PO4+H2O with explainatio please ​
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Answer:

3 NH4OH (l) + H3PO4 (aq) → (NH4)3PO4 (aq) + 3 H2O (l)

Explanation:

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AfilCa [17]
Answer:
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Explanation
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