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2 years ago

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Which of the following is acidic when dissolved in water? a. SO b. NO2 c. Na, d. Cao e. Two of these modern periodic table are a

rranged according to increase -- and group 7A elements of periodical

1 answer:

Zielflug [23.3K]2 years ago

4 0

Answer: e. Two of these

Explanation:

(a) $SO_2$

When $SO_2$ is dissolved in water. It reacts to form sulfurous acid. The chemical reaction is shown below:

$SO_2+H_2O\rightarrow H2SO_3$

Therefore, $SO_2$ is acidic when dissolved in water.

(b) $NO_2$

When $NO_2$ is dissolved in water. It reacts to form nitric acid. The chemical reaction is shown below:

$3NO_2+H_2O\rightarrow 2HNO_3+NO$

Therefore, $NO_2$ is acidic when dissolved in water.

(c) $Na$

Sodium is a metal. It gives sodium hydroxide on reaction with water. The chemical reaction is as follows:

$
Na+H_2O\rightarrow NaOH
+H_2$

Therefore, Na is basic when dissolved in water.

(d) $CaO
$

Calcium oxide is a metallic salt. It gives calcium hydroxide on reaction with water. The chemical reaction is as follows:

$CaO+H_2O\rightarrow Ca(OH)_2$ ,

Therefore, $CaO
$ is basic when dissolved in water.

(e) Two of these.

Since both $SO_2$ and $NO_2$ give acids when dissolved in water, both are acidic.

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II. Ionic Equations

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Answer:

Complete ionic: $\begin{aligned}& \rm 2\, Ag^{+}\, (aq) + 2\, {NO_3}^{-} \, (aq) + Ca^{2+}\, (aq) + 2\, Cl^{-}\, (aq) \\ & \rm \to 2\, AgCl\, (s) + Ca^{2+}\, (aq) + 2\, {NO_3}^{-}\, (aq)\end{aligned}$ .

Net ionic: $\begin{aligned}& \rm Ag^{+}\, (aq) + Cl^{-}\, (aq) \to AgCl\, (s)\end{aligned}$ .

Explanation:

Start by identifying species that exist as ions. In general, such species include:

Soluble salts.
Strong acids and strong bases.

All four species in this particular question are salts. However, only three of them are generally soluble in water: $\rm AgNO_3$ , $\rm CaCl_2$ , and $\rm Ca(NO_3)_2$ . These three salts will exist as ions:

Each $\rm AgNO_3\, (aq)$ formula unit will exist as one $\rm Ag^{+}$ ion and one $\rm {NO_3}^{-}$ ion.
Each $\rm CaCl_2$ formula unit will exist as one $\rm Ca^{2+}$ ion and two $\rm Cl^{-}$ ions (note the subscript in the formula $\rm CaCl_2\!$ .)
Each $\rm Ca(NO_3)_2$ formula unit will exist as one $\rm Ca^{2+}$ and two $\rm {NO_3}^{-}$ ions.

On the other hand, $\rm AgCl$ is generally insoluble in water. This salt will not form ions.

Rewrite the original chemical equation to get the corresponding ionic equation. In this question, rewrite $\rm AgNO_3$ , $\rm CaCl_2$ , and $\rm Ca(NO_3)_2$ (three soluble salts) as the corresponding ions.

Pay attention to the coefficient of each species. For example, indeed each $\rm AgNO_3\, (aq)$ formula unit will exist as only one $\rm Ag^{+}$ ion and one $\rm {NO_3}^{-}$ ion. However, because the coefficient of $\rm AgNO_3\, (aq)\!$ in the original equation is two, $\!\rm AgNO_3\, (aq)$ alone should correspond to two $\rm Ag^{+}\!$ ions and two $\rm {NO_3}^{-}\!$ ions.

Do not rewrite the salt $\rm AgCl$ because it is insoluble.

$\begin{aligned}& \rm 2\, Ag^{+}\, (aq) + 2\, {NO_3}^{-} \, (aq) + Ca^{2+}\, (aq) + 2\, Cl^{-}\, (aq) \\ & \rm \to 2\, AgCl\, (s) + Ca^{2+}\, (aq) + 2\, {NO_3}^{-}\, (aq)\end{aligned}$ .

Eliminate ions that are present on both sides of this ionic equation. In this question, such ions include one unit of $\rm Ca^{2+}$ and two units of $\rm {NO_3}^{-}$ . Doing so will give:

$\begin{aligned}& \rm 2\, Ag^{+}\, (aq) + 2\, Cl^{-}\, (aq) \to 2\, AgCl\, (s)\end{aligned}$ .

Simplify the coefficients:

$\begin{aligned}& \rm Ag^{+}\, (aq) + Cl^{-}\, (aq) \to AgCl\, (s)\end{aligned}$ .

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