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Eduardwww [97]
3 years ago
5

Write a net ionic equation for the overall reaction that occurs when aqueous solutions of phosphoric acid (h3po4) and potassium

hydroxide are combined.assume excess base. use the pull-down boxes to specify states such as (aq) or (s).
Chemistry
1 answer:
shusha [124]3 years ago
7 0
Firstly, we have to show molecular equation (all compounds are showed as neutral molecules) for the reaction:

H₃PO₄(aq) + 3KOH(aq)  ⇒ K₃PO₄(aq) + 3H₂O(l) 

Then, the reaction has to be written as an ionic equation:

3H⁺(aq) + PO₄³⁻(aq) + 3K⁺(aq)+ 3OH⁻(aq) +   ⇒  3K⁺(aq) + PO₄³⁻(aq)  + 3H₂O(l) 

The molecule of water does not dissociate and it is shown as a molecule. Soluble ionic compounds H₃PO₄ and KOH are shown as dissociated ions.
Since there are not spectator ions (ions that do not participate in the reaction) the equation is at the same time and net ionic equation (ions and molecules involved in the reaction).

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Explain the reason potassium was visible when using the cobalt glass. Describe what occured.
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Explanation:

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What type of organic compound has the empirical formula CH2O and can serve as energy storage or the starting material for fats a
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4 0
3 years ago
Se hace reaccionar 4,00 g de aluminio y 42,00 g de bromo, según la reacción: Al(s)+Br2(l)⟶AlBr3(s) Calcular las moles de AlBr3(s
NeX [460]

Answer:

0.145 moles de AlBr3.

Explanation:

¡Hola!

En este caso, al considerar la reacción química dada:

Al(s)+Br2(l)⟶AlBr3(s)

Es claro que primero debemos balancearla como se muestra a continuación:

2Al(s)+3Br2(l)⟶2AlBr3(s)

Así, calculamos las moles del producto AlBr3 por medio de las masas de ambos reactivos, con el fin de decidir el resultado correcto:

n_{AlBr_3}^{por\ Al}=4.00gAl*\frac{1molAl}{27gAl} *\frac{2molAlBr_3}{2molAl}=0.145mol AlBr_3\\\\n_{AlBr_3}^{por\ Br_2}=42.00gr*\frac{1molr}{160g Br_2} *\frac{2molAlBr_3}{3molBr_2}=0.175mol AlBr_3

Así, inferimos que el valor correcto es 0.145 moles de AlBr3, dado que viene del reactivo límite que es el aluminio.

¡Saludos!

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