Question

choose the correct products for the double replacement reaction below. click here to access the solubility rules to determine which product, if any, forms a solid precipitate in the reaction. agno₃ + kcl →? options: k + o₂ + ncl; kno₃ + agcl; agk + clno₃; k₂no₃ + agcl₂. which product in the reaction forms a precipitate? options: kno3; agcl; agk; no precipitate formed

Explanation:

For the first part (correct products of double replacement reaction):

Step1: Recall double replacement reaction pattern

In a double replacement reaction, the general form is \( AB + CD
ightarrow AD + CB \), where cations and anions swap. For \( \text{AgNO}_3 + \text{KCl} \), the cation of \( \text{AgNO}_3 \) is \( \text{Ag}^+ \), anion is \( \text{NO}_3^- \); cation of \( \text{KCl} \) is \( \text{K}^+ \), anion is \( \text{Cl}^- \). Swapping gives \( \text{KNO}_3 \) (from \( \text{K}^+ \) and \( \text{NO}_3^- \)) and \( \text{AgCl} \) (from \( \text{Ag}^+ \) and \( \text{Cl}^- \)).

Step2: Eliminate incorrect options

• \( \text{K} + \text{O}_2 + \text{NCl} \): Not following double replacement, and incorrect species.
• \( \text{AgK} + \text{ClNO}_3 \): Incorrect ion combinations.
• \( \text{K}_2\text{NO}_3 + \text{AgCl}_2 \): Incorrect formulas (e.g., \( \text{K}_2\text{NO}_3 \) is wrong, should be \( \text{KNO}_3 \); \( \text{AgCl}_2 \) is wrong, \( \text{Ag}^+ \) and \( \text{Cl}^- \) form \( \text{AgCl} \)).

For the second part (which product is precipitate):

Step1: Recall solubility rules

Nitrates (\( \text{NO}_3^- \)) are generally soluble, so \( \text{KNO}_3 \) is soluble (aqueous). Chlorides (\( \text{Cl}^- \)) are soluble except for \( \text{Ag}^+ \), \( \text{Pb}^{2+} \), \( \text{Hg}_2^{2+} \). So \( \text{AgCl} \) is insoluble (precipitate).

Step2: Determine precipitate

From the products \( \text{KNO}_3 \) (soluble) and \( \text{AgCl} \) (insoluble), \( \text{AgCl} \) is the precipitate.

Answer:

s:

• Correct products: \( \text{KNO}_3 + \text{AgCl} \)
• Precipitate product: \( \text{AgCl} \)