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3 years ago

What net ionic equation describes the reaction when these solutions are mixed?

Chemistry

2 answers:

Aleksandr-060686 [28]3 years ago

8 0

Answer:

$2PO_{4}^{-3} (aq) + 3Ca^{+2}(aq)-->Ca_{3}(PO_{4})_{2}(s)$

Explanation:

In net ionic equation we remove the spectator ions. The ions which are present on both the side and are not forming any solid compound.

Let us write the balanced reaction first:

$2Na_{3}PO_{4}(aq)+3CaCl_{2}(aq)-->3Ca_{3}(PO_{4})_{2}+6NaCl(aq)$

The ionic reaction is:

$6Na^{+}(aq)++6Cl^{-}(aq)+2PO_{4}^{-3} (aq) + 3Ca^{+2}(aq)-->Ca_{3}(PO_{4})_{2}(s)+6Na^{+}(aq)+6Cl^{-}(aq)$

Thus net ionic reaction is

$2PO_{4}^{-3} (aq) + 3Ca^{+2}(aq)-->Ca_{3}(PO_{4})_{2}(s)$

almond37 [142]3 years ago

7 0

I think the correct answer from the choices listed above is option D. The net ionic equation that will describe the reaction of the reactants when mixed is expressed as:

<span>2PO43–(aq) + 3Ca2+(aq) → Ca3(PO4)2(s)
</span>
Hope this answers the question. Have a nice day.

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Use the following balanced equation to answer the questions below.

Blababa [14]

Answer:

A. 4.5 mol Mg(OH)₂

B. 6 mol NaOH

Explanation:

Let's consider the following balanced equation.

Mg(NO₃)₂ + 2 NaOH ⇒ Mg(OH)₂ + 2 NaNO₃

PART A

The molar ratio of NaOH to Mg(OH)₂ is 2:1. The moles of Mg(OH)₂ produced from 9 moles of NaOH are:

9 mol NaOH × 1 mol Mg(OH)₂/2 mol NaOH = 4.5 mol Mg(OH)₂

PART B

The molar ratio of NaOH to NaNO₃ is 2:2. The moles of NaOH needed to produce 6 moles of NaNO₃ are:

6 mol NaNO₃ × 2 mol NaOH/2 mol NaNO₃ = 6 mol NaOH

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2 years ago

WILL GIVE 50 POINTS AND BRAINLIEST Describe the properties of alkaline earth metals. Based on their electronic arrangement, expl

Arisa [49]

Alkaline earth metals are metals of group two. They are divalent metals and they have a highly negative reduction potential hence the metals are mostly extracted by electrolysis.

They are highly reactive metals. They react with water but do so less readily than alkali earth metals.

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1 year ago

Which statement accurately describes dark matter?

Mandarinka [93]

Answer:

C. It does not emit electromagnetic radiation.

Explanation:

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2 years ago

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Select the compounds from the list below which are insoluble in water

natulia [17]

Answer:

Insoluble in water:

BaSO4

PbCl2

Cu2O

AgBr

Explanation:

Water turns out to be a good solvent for ionic substances, or in general, polarized covalent substances. On the other hand, it is not a good solvent for non-polar substances, these being the vast majority of covalent substances.

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3 years ago

EXTRA POINTSSS 1. A solution at 25 degrees Celsius is 1.0 × 10–5 M H3O+. What is the concentration of OH– in this solution?

AlekseyPX

Answer:

Concentration of OH⁻:

1.0 × 10⁻⁹ M.

Explanation:

The following equilibrium goes on in aqueous solutions:

$\text{H}_2\text{O}\;(l)\rightleftharpoons \text{H}^{+}\;(aq) + \text{OH}^{-}\;(aq)$ .

The equilibrium constant for this reaction is called the self-ionization constant of water:

$K_w = [\text{H}^{+}]\cdot[\text{OH}^{-}]$ .

Note that water isn't part of this constant.

The value of $K_w$ at 25 °C is $10^{-14}$ . How to memorize this value?

The pH of pure water at 25 °C is 7.
$[\text{H}^{+}] = 10^{-\text{pH}} = 10^{-7}\;\text{mol}\cdot\text{dm}^{-3}$
However, $[\text{OH}^{-}] = [\text{H}^{+}]=10^{-7}\;\text{mol}\cdot\text{dm}^{-3}$ for pure water.
As a result, $K_w = [\text{H}^{+}] \cdot[\text{OH}^{-}] = (10^{-7})^{2} = 10^{-14}$ at 25 °C.

Back to this question. $[\text{H}^{+}]$ is given. 25 °C implies that $K_w = 10^{-14}$ . As a result,

$\displaystyle [\text{OH}^{-}] = \frac{K_w}{[\text{H}^{+}]} = \frac{10^{-14}}{1.0\times 10^{-5}} = 10^{-9} \;\text{mol}\cdot\text{dm}^{-3}$ .

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3 years ago