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tatuchka [14]
3 years ago
5

What is the balanced NET ionic equation for the reaction when aqueous Cs₃PO₄ and aqueous AgNO₃ are mixed in solution to form sol

id Ag₃PO₄ and aqueous CsNO₃
Chemistry
1 answer:
rusak2 [61]3 years ago
7 0

Answer:

PO_4^{3-}(aq)+3Ag^+(aq)\rightarrow Ag_3PO_4(s)

Explanation:

Hello!

In this case, since the net ionic equation of a chemical reaction shows up the ionic species that result from the simplification of the spectator ions, which are those at both reactants and products sides, we take into account that aqueous species ionize into ions whereas liquid, solid and gas species remain unionized. In such a way, for the reaction of cesium phosphate and silver nitrate we can write the complete molecular equation:

Cs_3PO_4(aq)+3AgNO_3(aq)\rightarrow Ag_3PO_4(s)+3CsNO_3(aq)

Whereas the three aqueous salts are ionized in order to write the following complete ionic equation:

3Cs^+(aq)+PO_4^{3-}(aq)+3Ag^+(aq)+3NO_3^-(aq)\rightarrow Ag_3PO_4(s)+3Cs^+(aq)+3NO_3^-(aq)

In such a way, since the cesium and nitrate ions are the spectator ions because of the aforementioned, the net ionic equation turns out:

PO_4^{3-}(aq)+3Ag^+(aq)\rightarrow Ag_3PO_4(s)

Best regards!

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Which of the following is converted into chemical energy during photosynthesis?
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Calculate the gas constant, R, if 25.55 mL of hydrogen gas was collected at a barometric pressure of 0.987 atm and a temperature
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3 years ago
What volume of 6.9 M NaOH is needed to completely titrate 0.42 L of 2.39 M phosphoric acid according to
kirill115 [55]

Taking into account the definition of molarity and the stoichiometry of the reaction, the correct option is option C) 0.44 L of 6.9 M NaOH is needed to completely titrate 0.42 L of 2.39 M phosphoric acid.

The balanced reaction is:

H₃PO₄ (aq) + 3 NaOH (aq) → Na₃PO₄ (aq) + 3 H₂O(aq)

Then, by stoichiometry of the reaction (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:

  • H₃PO₄: 1 mole
  • NaOH: 3 moles
  • Na₃PO₄: 1 mole
  • H₂O: 3 moles

Molarity is the number of moles of solute that are dissolved in a given volume.

Molarity is determined by:

Molarity=\frac{number of moles of solute}{volume}

 Molarity is expressed in units \frac{moles}{liter}.

In this case, 0.42 L of 2.39 M phosphoric acid reacts. So, by definition of molarity, the number of moles that participate in the reaction is calculated as:

2.39 \frac{moles}{liter}=\frac{number of moles of phosphiric acid}{0.42 liters}

Solving:

number of moles of phosphiric acid= 2.39 \frac{moles}{liter}* 0.42 liters

number of moles of phosphiric acid= 1.0038 moles ≅ 1 mole

Approaching 1 mole of the amount of phosphoric acid required, then by stoichiometry of the reaction, 3 moles of NaOH are necessary to react with 1 mole of the acid.

Then by definition of molarity and knowing that 6.9 M NaOH is needed, you can calculate the necessary volume amount of NaOH by:

6.9 \frac{moles}{liter} =\frac{3 moles}{volume}

Solving:

6.9 \frac{moles}{liter}* volume= 3 moles

volume=\frac{3 moles}{6.9\frac{moles}{liter} }

volume= 0.44 L

The correct option is option C) 0.44 L of 6.9 M NaOH is needed to completely titrate 0.42 L of 2.39 M phosphoric acid.

Learn more about molarity with this example: <u>brainly.com/question/15406534?referrer=searchResults</u>

5 0
3 years ago
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