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Chapter 4: Q95E (page 225)

The reaction of WCl6 with Al at ~4000C gives black crystals of a compound containing only tungsten and chlorine. A sample of this compound, when reduced with hydrogen, gives 0.2232 g of tungsten metal and hydrogen chloride, which is absorbed in water. Titration of the hydrochloric acid thus produced requires 46.2 mL of 0.1051 M NaOH to reach the end point. What is the empirical formula of the black tungsten chloride?

Short Answer

Expert verified

The empirical formula of black tungsten chloride is WCl4

Step by step solution

01

Moles of chlorine

According to the question, it is given that

The volume of sodium hydroxide is 46.2 ml or 0.0462 L

The concentration or molarity of sodium hydroxide is 0.1051 M

\(\begin{array}{l}{\rm{Moles = Molarity }} \times {\rm{ Volume}}\\{\rm{Moles = 0}}{\rm{.1051 }} \times {\rm{ 0}}{\rm{.0462 = 0}}{\rm{.00483 moles}}\end{array}\)

As 1 mole sodium hydroxide reacts with 1 mole of hydrochloric acid and it has only one chlorine atom, therefore the moles of chlorine will be 0.00483 moles.

\({\rm{3Ca(OH}}{{\rm{)}}_2}{\rm{ + 2}}{{\rm{C}}_3}{{\rm{H}}_7}{\rm{COOH }} \to {\rm{ C}}{{\rm{a}}_3}{{\rm{(}}{{\rm{C}}_3}{{\rm{H}}_7}{\rm{COO)}}_2}{\rm{ + 6}}{{\rm{H}}_2}{\rm{O}}\)

As 3 mole of calcium hydroxide reacts with 2 moles of propionic acid then 0.284 moles of propionic acid will react with \(\frac{3}{2}{\rm{ }} \times {\rm{ 0}}{\rm{.284 = 0}}{\rm{.426 moles}}\)

02

Moles of tungsten

In the question, given mass of tungsten is 0.2232 g

The molecular mass of tungsten is 183 g/mole

Therefore, the number of moles of tungsten will be

\(\begin{array}{l}{\rm{Moles = }}\frac{{{\rm{Mass}}}}{{{\rm{Molecular mass}}}}\\{\rm{Moles = }}\frac{{0.2232}}{{183}}{\rm{ = 0}}{\rm{.001214 moles}}\end{array}\)

03

Empirical formula of tungsten chloride

The simplest ratio of the atoms or elements present in a compound is illustrated by the empirical formula. To calculate the empirical formula, the number of moles of each atom is divided with the smallest number of moles to get the simplest whole number ratio that is:

Atom

Number of moles

Simplest whole number ratio

Tungsten

0.001214

\(\frac{{0.001214}}{{0.001214}}{\rm{ = 1}}\)

Chlorine

0.004856

\(\frac{{0.004856}}{{0.001214}}{\rm{ = 4}}\)

Therefore, the empirical formula of the black tungsten chloride will be WCl4

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Most popular questions from this chapter

Uranium can be isolated from its ores by dissolving it as UO2(NO3)2, then separating it as solid UO2(C2O4). Addition of 0.4031 g of sodium oxalate, NaC2O4, to a solution containing 1.481 g of uranyl nitrate, UO2(NO3)2, yields 1.073 g of solid

\(Na{C_2}{O_4} + U{O_2}{\left( {N{O_3}} \right)_2} + 3{H_2}O \to U{O_2}\left( {{C_2}{O_4}} \right) \cdot 3{H_2}O + 2NaN{O_3}\)

Potatoes can be peeled commercially by soaking them in a 3-M to 6-M solution of sodium hydroxide, then removing the loosened skins by spraying them with water. Does a sodium hydroxide solution have a suitable concentration if titration of 12.00 mL of the solution requires 30.6 mL of 1.65 M HCI to reach the end point?

This equation describes the production of tin (II) chloride.\(Sn\left( s \right) + 2HCl\left( g \right) \to SnC{l_2}\left( s \right) + {H_2}\left( g \right)\)Is this a redox reaction? If so, provide a more specific name to the reaction if appropriate, and identify the oxidant and reductant.

Titration of a 20.0-mL sample of acid rain required 1.7 mL of 0.0811MNaOH to reach the end point. If we assume that the acidity of the rain is due to the presence of sulfuric acid, what was the concentration of sulfuric acid in this sample of rain?

Potassium acid phthalate, KHC6H4O4or KHP, is used in many laboratories, including general chemistry laboratories, to standardize solutions of base. KHP is one of only a few stable solid acids that can be dried by warming and weighed. A 0.3420-g sample of KHC6H4O4 reacts with 35.73 mL of a NaOH solution in a titration. What is the molar concentration of the NaOH?

\({\rm{KH}}{{\rm{C}}_6}{{\rm{H}}_4}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + NaO}}{{\rm{H}}_{({\rm{aq}})}}{\rm{ }} \to {\rm{ KNa}}{{\rm{C}}_6}{{\rm{H}}_4}{{\rm{O}}_{4({\rm{aq}})}}{\rm{ + }}{{\rm{H}}_2}{{\rm{O}}_{({\rm{aq}})}}\)
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