Question

question 1
indicate which reactants will result in an neutralization reaction.
□ hcl and nac₂h₃o₂
□ naoh and nh₄cl
□ h₂so₄ and sr(oh)₂
□ hcl and nh₄oh

Explanation:

Step1: Recall neutralization reaction

A neutralization reaction is between an acid and a base to form salt and water.

Step2: Analyze each option

- \( \text{HCl (acid)} \) and \( \text{NaC}_2\text{H}_3\text{O}_2 \) (salt of weak acid and strong base, not a base) → Not neutralization.
- \( \text{NaOH (base)} \) and \( \text{NH}_4\text{Cl} \) (salt, not an acid) → Not neutralization.
- \( \text{H}_2\text{SO}_4 \) (acid) and \( \text{Sr(OH)}_2 \) (base) → Acid - base reaction, forms \( \text{SrSO}_4 \) (salt) and \( \text{H}_2\text{O} \) → Neutralization.
- \( \text{HCl (acid)} \) and \( \text{NH}_4\text{OH} \) (base) → Acid - base reaction, forms \( \text{NH}_4\text{Cl} \) (salt) and \( \text{H}_2\text{O} \) → Neutralization. Wait, but let's re - check. \( \text{NH}_4\text{OH} \) is a weak base, \( \text{HCl} \) is strong acid. Also, \( \text{H}_2\text{SO}_4 \) (strong acid) and \( \text{Sr(OH)}_2 \) (strong base) is a classic neutralization. Also, \( \text{HCl} \) and \( \text{NH}_4\text{OH} \): \( \text{HCl}+\text{NH}_4\text{OH}=\text{NH}_4\text{Cl}+\text{H}_2\text{O} \), which is neutralization. But let's check the options again. Wait, maybe the intended correct ones are \( \text{H}_2\text{SO}_4 \) and \( \text{Sr(OH)}_2 \), and \( \text{HCl} \) and \( \text{NH}_4\text{OH} \), and also let's check \( \text{NaOH} \) and \( \text{NH}_4\text{Cl} \): \( \text{NaOH}+\text{NH}_4\text{Cl}=\text{NaCl}+\text{NH}_3+\text{H}_2\text{O} \), this is a reaction between a base and a salt, not acid - base (neutralization in the strict sense? Wait, \( \text{NH}_4\text{Cl} \) is an acidic salt (since \( \text{NH}_4^+ \) is acidic). So \( \text{NaOH} \) (base) and \( \text{NH}_4\text{Cl} \) (acidic salt) react, but is this a neutralization? Neutralization is acid + base. So \( \text{H}_2\text{SO}_4 \) (acid) and \( \text{Sr(OH)}_2 \) (base) is a clear acid - base (neutralization). \( \text{HCl} \) (acid) and \( \text{NH}_4\text{OH} \) (base) is acid - base. \( \text{NaOH} \) (base) and \( \text{NH}_4\text{Cl} \) (salt, \( \text{NH}_4^+ \) is acidic, so it can act as an acid? Wait, \( \text{NH}_4^+ \) is a weak acid, so \( \text{NaOH} \) (base) and \( \text{NH}_4^+ \) (acid) reaction: \( \text{OH}^-+\text{NH}_4^+=\text{NH}_3+\text{H}_2\text{O} \), which is also an acid - base reaction (neutralization). And \( \text{HCl} \) and \( \text{NaC}_2\text{H}_3\text{O}_2 \): \( \text{HCl}+\text{NaC}_2\text{H}_3\text{O}_2=\text{NaCl}+\text{HC}_2\text{H}_3\text{O}_2 \), this is a reaction between acid and salt (conjugate base of weak acid), it's a displacement reaction, not neutralization.

So the correct options are \( \text{H}_2\text{SO}_4 \) and \( \text{Sr(OH)}_2 \), \( \text{HCl} \) and \( \text{NH}_4\text{OH} \), and \( \text{NaOH} \) and \( \text{NH}_4\text{Cl} \)? Wait, maybe I made a mistake. Let's re - define neutralization: reaction between acid and base to form salt and water.

- \( \text{H}_2\text{SO}_4 \) (acid) + \( \text{Sr(OH)}_2 \) (base) → \( \text{SrSO}_4 \) (salt) + \( \text{H}_2\text{O} \) (water) → Neutralization.
- \( \text{HCl} \) (acid) + \( \text{NH}_4\text{OH} \) (base) → \( \text{NH}_4\text{Cl} \) (salt) + \( \text{H}_2\text{O} \) (water) → Neutralization.
- \( \text{NaOH} \) (base) + \( \text{NH}_4\text{Cl} \) (salt, but \( \text{NH}_4^+ \) is a weak acid) → \( \text{NaCl} \) (salt) + \( \text{NH}_3 \) + \( \text{H}_2\text{O} \). Here, \( \text{NH}_4^+ \) acts as an acid (donates \( \text{H}^+ \) to \( \text{OH}^- \)), so it is an acid - base reaction (neutralization).
- \( \text{HCl} \) and \( \text{NaC}_2\text{H}_3\text{O}_2 \): \( \text{HCl} \) (acid) + \( \text{NaC}_2\text{H}_3\text{O}_2 \) (conjugate base of \( \text{HC}_2\text{H}_3\text{O}_2 \)) → \( \text{NaCl} \) + \( \text{HC}_2\text{H}_3\text{O}_2 \). This is a reaction between an acid and a conjugate base (a salt), not a base, so not neutralization.

So the correct options are \( \text{H}_2\text{SO}_4 \) and \( \text{Sr(OH)}_2 \), \( \text{NaOH} \) and \( \text{NH}_4\text{Cl} \), \( \text{HCl} \) and \( \text{NH}_4\text{OH} \). But let's check standard neutralization: acid (proton donor) and base (proton acceptor) to form salt and water.

\( \text{H}_2\text{SO}_4 \) (acid) + \( \text{Sr(OH)}_2 \) (base) → salt + water: yes.

\( \text{NaOH} \) (base) + \( \text{NH}_4\text{Cl} \) (acidic salt, \( \text{NH}_4^+ \) is acid) → acid - base reaction: yes.

\( \text{HCl} \) (acid) + \( \text{NH}_4\text{OH} \) (base) → acid - base reaction: yes.

But maybe the question considers only strong acid - strong base or acid - base (including weak). So the correct check - boxes are for \( \text{H}_2\text{SO}_4 \) and \( \text{Sr(OH)}_2 \), \( \text{NaOH} \) and \( \text{NH}_4\text{Cl} \), \( \text{HCl} \) and \( \text{NH}_4\text{OH} \). But let's confirm with the definition. A neutralization reaction is when an acid and a base react to form a salt and water. So:

1. \( \text{HCl} \) (acid) and \( \text{NaC}_2\text{H}_3\text{O}_2 \) (salt, not base) → No.
2. \( \text{NaOH} \) (base) and \( \text{NH}_4\text{Cl} \) ( \( \text{NH}_4^+ \) is acid) → Acid - base reaction (neutralization) → Yes.
3. \( \text{H}_2\text{SO}_4 \) (acid) and \( \text{Sr(OH)}_2 \) (base) → Acid - base reaction (neutralization) → Yes.
4. \( \text{HCl} \) (acid) and \( \text{NH}_4\text{OH} \) (base) → Acid - base reaction (neutralization) → Yes.

Answer:

\( \text{H}_2\text{SO}_4 \) and \( \text{Sr(OH)}_2 \), \( \text{NaOH} \) and \( \text{NH}_4\text{Cl} \), \( \text{HCl} \) and \( \text{NH}_4\text{OH} \) (the check - boxes for these three options should be selected)