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NEET CHEMISTRYEquilibriumMedium

Question

The solubility of AgCl(s) with solubility product 1.6×10−101.6 \times 10^{-10} in 0.1 M NaCl solution would be?

A

1.26×10−5 M1.26 \times 10^{-5} \text{ M}

B

1.6×10−9 M1.6 \times 10^{-9} \text{ M}

C

1.6×10−11 M1.6 \times 10^{-11} \text{ M}

D

zero

Step-by-Step Solution

Let the solubility of AgCl in 0.1 M NaCl solution be SS. The dissociation of AgCl is given by: AgCl(s)⇌Ag+(aq)+Cl−(aq)\text{AgCl}(s) \rightleftharpoons \text{Ag}^+(aq) + \text{Cl}^-(aq) In the solution, Cl−\text{Cl}^- ions are also provided by the complete dissociation of the strong electrolyte NaCl. [Cl−]=S+0.1≈0.1 M[\text{Cl}^-] = S + 0.1 \approx 0.1 \text{ M} (since SS is very small compared to 0.1 M due to the common ion effect). [Ag+]=S[\text{Ag}^+] = S The solubility product expression is: Ksp=[Ag+][Cl−]K_{sp} = [\text{Ag}^+][\text{Cl}^-] 1.6×10−10=S×0.11.6 \times 10^{-10} = S \times 0.1 S=1.6×10−100.1=1.6×10−9 MS = \frac{1.6 \times 10^{-10}}{0.1} = 1.6 \times 10^{-9} \text{ M}.

Exam Context & Concepts Covered

This question aligns with the NEET CHEMISTRY syllabus, specifically targeting concepts from Equilibrium. Mastering this topic is crucial for scoring well in the upcoming medical entrance examinations. Solving conceptually related problems will help you understand the nuances of these concepts and improve your problem-solving speed.

CHEMISTRYEquilibriumsolubilitysolubilityproductsolution

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Consider the following reaction: $\text{A}_2(g) + \text{B}_2(g) \rightleftharpoons 2\text{AB}(g)$. At equilibrium, the concentrations of $[\text{A}_2] = 3.0 \times 10^{–3} \text{ M}$; $[\text{B}_2] = 4.2 \times 10^{–3} \text{ M}$ and $[\text{AB}] = 2.8 \times 10^{–3} \text{ M}$. The value of $K_c$ for the above-given reaction in a sealed container at $527^\circ\text{C}$ is:

A.3.9
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Amongst the given options, which of the following molecules/ions acts as a Lewis acid?

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D.$\text{BF}_3$
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Boric acid is an acid because its molecule

A.contains replaceable H⁺ ion
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The following solutions were prepared by mixing different volumes of NaOH and HCl of different concentrations. pH of which one of them will be equal to 1?

A.$60 \text{ mL } \frac{M}{10} \text{ HCl } + 40 \text{ mL } \frac{M}{10} \text{ NaOH}$
B.$55 \text{ mL } \frac{M}{10} \text{ HCl } + 45 \text{ mL } \frac{M}{10} \text{ NaOH}$
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The tendency of $BF_3$, $BCl_3$ and $BBr_3$ to behave as Lewis acid decreases in the sequence:

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A.$2 \times 10^{-4} \text{ mol/L}$
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In qualitative analysis, the metals of Group I can be separated from other ions by precipitating them as chloride salts. A solution initially contains $\text{Ag}^+$ and $\text{Pb}^{2+}$ at a concentration of $0.10 \text{ M}$. Aqueous $\text{HCl}$ is added to this solution until the $\text{Cl}^-$ concentration is $0.10 \text{ M}$. What will the concentration of $\text{Ag}^+$ and $\text{Pb}^{2+}$ at equilibrium? ($K_{sp}$ for $\text{AgCl} = 1.8 \times 10^{-10}$, $K_{sp}$ for $\text{PbCl}_2 = 1.7 \times 10^{-5}$)

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