Chemistry, 28.07.2019 22:30 wcraig1998

What is the molarity of a solution made by dissolving 29.5 g of sodium hydroxide (naoh) in enough water to make 2.45 l of solution? molar mass na: 22.99 g/molmolar mass o: 16.00 g/molmolar mass h: 1.008 g/mol

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molarity is defined as the number of moles of solute in 1 L of solution.
the number of moles of NaOH = mass present / molar mass of NaOH

molar mass of NaOH = 22.99 + 16.00 + 1.008 = 40.00 g/mol

therefore NaOH moles = 29.5 g / 40.00 g/mol = 0.738 mol

the number of NaOH moles in 2.45 L solution - 0.738 mol
therefore number of NaOH moles in 1 L = 0.738 mol / 2.45 L = 0.301 mol/L molarity of NaOH = 0.301 M

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.

Answer from: Quest

Answerstrong acids and bases completely dissociate in water.this is how strong acids and bases are defined. they will ionize 100% in solution, making a non-reversible reaction

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What is the molarity of a solution made by dissolving 29.5 g of sodium hydroxide (naoh) in enough wa...

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