Chemistry, 29.10.2019 14:31 hoopstarw4438

Which statement best describes the process of making a solution by diluting a stock solution?
add more solute to decrease the concentration.
add more solute to increase the concentration.
add more solvent to decrease the concentration.
add more solvent to increase the concentration.

Answers: 2

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Answer from: alaynaakrie9151

Add more solvent to decrease the concentration.

Explanation:

Binary Solution is a homogeneous mixture of two components called as solute and solvent. Solute is the component which is present in smaller proportion and is solid for solid in liquid solution and solvent is the component which is present in larger proportion and is liquid for solid in liquid solution.

Concentrated solution is one in which there is more amount of solute.

Dilute solution is one in which there is more amount of solvent.

According to the neutralization law,

M_1V_1=M_2V_2

where,

M_1 = molarity of stock solution

V_1 = volume of stock solution

M_2 = molarity of diluted solution

V_2 = volume of diluted solution

Therefore, as the moles will remain same, if the volume increases, the concentration decreases.

Answer from: Quest

; lc

Answer from: Quest

Answerthis solution will not form a precipitateexplanationsolubility equilbrium: pbf₂(s) ⇄ pb²⁺(aq) + 2 f⁻(aq)the solubility product expression is $k_{sp} = [\text{pb}^{2+}][\text{f}^- ]^2 = 4 \times 10^{-8}$ (we exclude solids from the equilibrium expression).now suppose we have the trial ion product q, which we can define as $q = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}}$ then, we can interpret q as the product of the concentration of the ions that we have and ksp as the product of the ion concentrations that are needed to form a saturated solution.if q > ksp, then that implies that there will be a surplus of ions that exceed the amount that is required to form a saturated solution. a precipitate will then form (the precipitate continually forms until the surplus ions are removed and q is decreased to ksp's value).if q = ksp, the saturated solution that forms is barely saturated and the precipitate will be minimal.if q < ksp, then the ion concentration will not be enough to form a saturated solution (so no precipitate).using our information, we calculate the trial ion product: $\begin{aligned} q & = [\text{pb}^{2+}]_{\text{initial}} \cdot [\text{f}^- ]^2_{\text{initial}} \\ & = (1.9 \times 10^{-3} ) (3.8\times 10^{3})^2 \\ & = 2.7 \times 10^{-8} \end{aligned}$ since q = 2.7 × 10⁻⁸ < ksp = 4 × 10⁻⁸, a precipitate will not form.

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Which statement best describes the process of making a solution by diluting a stock solution?
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