Chemistry, 16.10.2019 21:00 johnsonwhitney2

Sludge and water mixture is homogeneous or heterogeneous mixture?

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Answer from: corcoranrobert1959

It is a heterogeneous mixture

Explanation:

A mixture is a substance that is formed by several components (two or more), which do not lose their properties and characteristics due to the mixing because there is no chemical reaction between them.

Homogeneous mixtures: Those mixtures whose components cannot be distinguished with the naked eye. The homogeneous mixtures of liquids are known as solutions and consist of a solute and a solvent, the first being the one in smaller proportion and also usually the liquid. For example, water mixed with mineral salts or sugar, water would be the solvent and sugar the solute.

Heterogeneous Mixtures: A heterogeneous mixture is one that has a non-uniform composition in which its components can be distinguished with the naked eye and is formed by two or more substances, physically different, unevenly distributed. The parts of a heterogeneous mixture can be separated mechanically. For example, water and sand, water and sludge, water and oil

Answer from: Quest

I’m pretty sure it’s false i’m not sure

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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