Ba(OH), (s) + _NH,SCN (s) → Observations:

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Balance the following chemical  equations 

**Chemical Reaction:**

\[ \_\_ \text{Ba(OH)}_2 (s) + \_\_ \text{NH}_4\text{SCN} (s) \rightarrow \]

**Observations:**

* [Text continues beyond the image and is not visible.]

This appears to be a partial chemical equation involving barium hydroxide (\(\text{Ba(OH)}_2\)) and ammonium thiocyanate (\(\text{NH}_4\text{SCN}\)), both in solid states. The substances likely react to form new products, which are not shown in the image. 

**Note:** The blanks suggest that coefficients for balancing the equation are required.
Transcribed Image Text:**Chemical Reaction:** \[ \_\_ \text{Ba(OH)}_2 (s) + \_\_ \text{NH}_4\text{SCN} (s) \rightarrow \] **Observations:** * [Text continues beyond the image and is not visible.] This appears to be a partial chemical equation involving barium hydroxide (\(\text{Ba(OH)}_2\)) and ammonium thiocyanate (\(\text{NH}_4\text{SCN}\)), both in solid states. The substances likely react to form new products, which are not shown in the image. **Note:** The blanks suggest that coefficients for balancing the equation are required.
**Reaction 1**

\[\underline{\hspace{1cm}} \, \text{Ba(OH)_2 (s)} + \underline{\hspace{1cm}} \, \text{HCl (aq)} \rightarrow \]

### Observations:

*(No observations provided in the image)*

**Explanation:**

The image shows a chemical equation that is not fully balanced. It involves the reactants barium hydroxide (\(\text{Ba(OH)_2}\)) in solid state and hydrochloric acid (\(\text{HCl}\)) in aqueous state. The reaction is producing unspecified products.

In a typical scenario, this reaction would result in barium chloride (\(\text{BaCl}_2\)) and water (\(\text{H}_2\text{O}\)):

\[ \text{Ba(OH)_2 (s)} + 2 \, \text{HCl (aq)} \rightarrow \text{BaCl}_2 (aq) + 2 \, \text{H}_2\text{O} (l) \] 

This is a type of acid-base reaction, wherein the acid (\(\text{HCl}\)) and the base (\(\text{Ba(OH)_2}\)) neutralize each other.
Transcribed Image Text:**Reaction 1** \[\underline{\hspace{1cm}} \, \text{Ba(OH)_2 (s)} + \underline{\hspace{1cm}} \, \text{HCl (aq)} \rightarrow \] ### Observations: *(No observations provided in the image)* **Explanation:** The image shows a chemical equation that is not fully balanced. It involves the reactants barium hydroxide (\(\text{Ba(OH)_2}\)) in solid state and hydrochloric acid (\(\text{HCl}\)) in aqueous state. The reaction is producing unspecified products. In a typical scenario, this reaction would result in barium chloride (\(\text{BaCl}_2\)) and water (\(\text{H}_2\text{O}\)): \[ \text{Ba(OH)_2 (s)} + 2 \, \text{HCl (aq)} \rightarrow \text{BaCl}_2 (aq) + 2 \, \text{H}_2\text{O} (l) \] This is a type of acid-base reaction, wherein the acid (\(\text{HCl}\)) and the base (\(\text{Ba(OH)_2}\)) neutralize each other.
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