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Chapter 13: Problem 136

What is the weight percent of \(23.4 \mathrm{g}\) of \(\mathrm{CaF}_{2}\) if dissolved in 10.5 mol of water? (a) \(0.028\); (b)\( 1.59\);(c) \(11.0\); (d) \(12.4 ;\) (e) none of these.

Short Answer

Expert verified
The weight percent of \(23.4 g\) of \(CaF_{2}\) if dissolved in 10.5 mol of water is approximately 11.01%. So, the closest answer choice is (c) 11.0. If none of the options were close enough, then (e) 'none of these' would be chosen.

Step by step solution

01

Identify Given Information

Extract the given values from the problem - the mass of the solute (Calcium Fluoride - \(CaF_{2}\)) which is \(23.4 g\), and volume of the solvent (Water - \(H_{2}O\)) expressed in moles, which is 10.5mol.
02

Convert Moles of Solvent to Mass

Convert the moles of water to grams using water’s molar mass (18.02 g/mol). So, the mass of the water = 10.5 mol * 18.02 g/mol = 189.21 g.
03

Calculate the total mass of the solution

Add the mass of the solute (\(CaF_{2}\)) to the mass of the solvent (water) to find the total mass of the solution. The total mass = 23.4g (\(CaF_{2}\)) + 189.21g (water) = 212.61 g.
04

Calculate Weight Percentage

Use the weight percentage formula: (Mass of solute / Total mass of solution) * 100. So, weight percent = (23.4 g / 212.61 g) * 100 = 11.01%.

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Most popular questions from this chapter

Thiophene \(\left(\mathrm{fp}=-38.3 ; \mathrm{bp}=84.4^{\circ} \mathrm{C}\right)\) is a sulfur containing hydrocarbon sometimes used as a solvent in place of benzene. Combustion of a \(2.348 \mathrm{g}\) sample of thiophene produces \(4.913 \mathrm{g} \mathrm{CO}_{2}, 1.005 \mathrm{g} \mathrm{H}_{2} \mathrm{O},\) and \(1.788 \mathrm{g} \mathrm{SO}_{2} .\) When a \(0.867 \mathrm{g}\) sample of thiophene is dissolved in \(44.56 \mathrm{g}\) of benzene \(\left(\mathrm{C}_{6} \mathrm{H}_{6}\right),\) the freezing point is lowered by \(1.183^{\circ} \mathrm{C} .\) What is the molecular formula of thiophene?

Explain the important distinctions between each pair of terms: (a) molality and molarity; (b) ideal and nonideal solution; (c) unsaturated and supersaturated solution; (d) fractional crystallization and fractional distillation; (e) osmosis and reverse osmosis.

At \(25^{\circ} \mathrm{C}\) a \(0.50 \mathrm{g}\) sample of polyisobutylene (a polymer used in synthetic rubber) in \(100.0 \mathrm{mL}\) of benzene solution has an osmotic pressure that supports a \(5.1 \mathrm{mm}\) column of solution \((d=0.88 \mathrm{g} / \mathrm{mL}) .\) What is the molar mass of the polyisobutylene? (For \(\mathrm{Hg}\), \(d=13.6 \mathrm{g} / \mathrm{mL} .)\)

Two of the substances listed here are highly soluble in water, two are only slightly soluble in water, and two are insoluble in water. Indicate the situation you expect for each one. (a) iodoform, \(\mathrm{CHI}_{3}\) (b) benzoic acid, (c) formic acid, (d) 1-butanol, (e) chlorobenzene, (f) propylene glycol, \(\mathrm{CH}_{3} \mathrm{CH}(\mathrm{OH}) \mathrm{CH}_{2} \mathrm{OH}\)

An important test for the purity of an organic compound is to measure its melting point. Usually, if the compound is not pure, it begins to melt at a lower temperature than the pure compound.(a) Why is this the case, rather than the melting point being higher in some cases and lower in others?(b) Are there any conditions under which the melting point of the impure compound is higher than that of the pure compound? Explain.
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