Question

scoring: your score will be based on the number of correct matches minus the number of incorrect matches. there is no penalty for missing matches.
use the references to access important values if needed for this question.
compare the solubility of silver sulfite in each of the following aqueous solutions:
0.10 m agno₃
0.10 m na₂so₃
0.10 m kch₃coo
0.10 m nh₄no₃
more soluble than in pure water.
similar solubility as in pure water.
less soluble than in pure water.
clear all

Explanation:

Step1: Analyze 0.10 M AgNO₃

Silver sulfite (\(Ag_2SO_3\)) dissociates as \(Ag_2SO_3(s)
ightleftharpoons 2Ag^+(aq) + SO_3^{2-}(aq)\). In 0.10 M \(AgNO_3\), \(Ag^+\) is a common ion. Common ion effect suppresses dissociation, so solubility of \(Ag_2SO_3\) is less than in pure water.

Step2: Analyze 0.10 M Na₂SO₃

\(Na_2SO_3\) dissociates to give \(SO_3^{2-}\), a common ion with \(Ag_2SO_3\)'s dissociation. Common ion effect reduces solubility, so \(Ag_2SO_3\) is less soluble than in pure water.

Step3: Analyze 0.10 M KCH₃COO

\(KCH_3COO\) dissociates to \(K^+\) and \(CH_3COO^-\). No common ion with \(Ag_2SO_3\) (ions \(Ag^+\) and \(SO_3^{2-}\)). So solubility is similar to pure water (since no common ion to affect equilibrium).

Step4: Analyze 0.10 M NH₄NO₃

\(NH_4NO_3\) dissociates to \(NH_4^+\) and \(NO_3^-\). No common ion with \(Ag_2SO_3\). Also, \(NH_4^+\) hydrolysis might slightly affect pH, but \(Ag_2SO_3\) solubility is mainly affected by common ions. Since no common ion, solubility is similar to pure water? Wait, no—wait, actually, \(NH_4^+\) is acidic, \(SO_3^{2-}\) is basic. \(NH_4^+\) (acidic) and \(SO_3^{2-}\) (basic) might react: \(NH_4^+ + SO_3^{2-}
ightleftharpoons NH_3 + HSO_3^-\). This would remove \(SO_3^{2-}\) from solution, shifting \(Ag_2SO_3\) dissociation to the right, increasing solubility. Wait, maybe I made a mistake earlier. Let's re-examine:

For \(Ag_2SO_3\) solubility:

• \(AgNO_3\): common \(Ag^+\) → less soluble.
• \(Na_2SO_3\): common \(SO_3^{2-}\) → less soluble.
• \(KCH_3COO\): \(CH_3COO^-\) is basic, but \(Ag_2SO_3\) has \(SO_3^{2-}\) (basic) and \(Ag^+\). No common ion, and \(CH_3COO^-\) doesn't react with \(Ag^+\) or \(SO_3^{2-}\) significantly. So solubility similar to pure water.
• \(NH_4NO_3\): \(NH_4^+\) is acidic, reacts with \(SO_3^{2-}\) (basic) to form \(HSO_3^-\) or \(NH_3\), reducing \(SO_3^{2-}\) concentration. So equilibrium \(Ag_2SO_3

ightleftharpoons 2Ag^+ + SO_3^{2-}\) shifts right, increasing solubility. So \(Ag_2SO_3\) is more soluble than in pure water here.

Wait, maybe my initial step3 was wrong. Let's correct:

• 0.10 M AgNO₃: Less soluble (common \(Ag^+\))
• 0.10 M Na₂SO₃: Less soluble (common \(SO_3^{2-}\))
• 0.10 M KCH₃COO: Similar (no common ion, no significant reaction)
• 0.10 M NH₄NO₃: More soluble (since \(NH_4^+\) reacts with \(SO_3^{2-}\), removing it, increasing \(Ag_2SO_3\) dissociation)

So matches:

• 0.10 M AgNO₃ → Less soluble than pure water
• 0.10 M Na₂SO₃ → Less soluble than pure water
• 0.10 M KCH₃COO → Similar solubility as pure water
• 0.10 M NH₄NO₃ → More soluble than pure water

Answer:

• 0.10 M AgNO₃: Less soluble than pure water
• 0.10 M Na₂SO₃: Less soluble than pure water
• 0.10 M KCH₃COO: Similar solubility as pure water
• 0.10 M NH₄NO₃: More soluble than pure water