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Chapter 4: Problem 130

The zinc in a 1.343 -g sample of a foot powder was precipitated as \(\mathrm{ZnNH}_{4} \mathrm{PO}_{4} .\) Strong heating of the precipitate yielded 0.4089 \(\mathrm{g} \mathrm{Zn}_{2} \mathrm{P}_{2} \mathrm{O}_{7}\) . Calculate the mass percent of zinc in the sample of foot powder.

Short Answer

Expert verified
The mass percent of zinc in the 1.343 g sample of foot powder is 13.01%.

Step by step solution

01

Finding the molar mass of zinc and Zn2P2O7

First, we need to find the molar mass of zinc (Zn) and zinc pyrophosphate (Zn2P2O7). The molar mass of an element or a compound is the sum of the atomic masses of the constituent atoms multiplied by their respective moles. The molar mass of Zn is 65.38 g/mol, P is 30.97 g/mol, and O is 16.00 g/mol. To find the molar mass of Zn2P2O7, we can use the equation: Molar mass Zn2P2O7 = 2(Molar mass Zn) + 2(Molar mass P) + 7(Molar mass O)
02

Calculate the molar mass of Zn2P2O7

Now let's calculate the molar mass of Zn2P2O7: Molar mass Zn2P2O7 = 2(65.38) + 2(30.97) + 7(16.00) = 130.76 + 61.94 + 112.00 = 304.70 g/mol
03

Calculate the mass of zinc in zinc pyrophosphate

We have the mass of zinc pyrophosphate, and now we have to find out the mass of zinc only: Mass of Zn in Zn2P2O7 = (mass of Zn2P2O7) * (molar mass of Zn) / (molar mass of Zn2P2O7) Mass of Zn = 0.4089 * (130.76) / 304.70
04

Calculate the mass of zinc

Now let's calculate the mass of zinc: Mass of Zn = 0.4089 * (130.76) / 304.70 = 0.1747 g.
05

Calculate the mass percent of zinc in the sample of foot powder

Finally, we can compute the mass percent of zinc in the sample of foot powder. We'll use the equation: Mass percent of Zn = (mass of Zn in the sample) / (mass of the sample) * 100 Mass percent of Zn = (0.1747) / (1.343) * 100
06

Calculate the mass percent of zinc

In the final step, we can calculate the mass percent of zinc: Mass percent of Zn = (0.1747) / (1.343) * 100 = 13.01 % So, the mass percent of zinc in the sample of foot powder is 13.01%.

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Most popular questions from this chapter

The blood alcohol \(\left(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\right)\) level can be determined by tirrating a sample of blood plasma with an acidic potassium dichromate solution, resulting in the production of \(\mathrm{Cr}^{3+}(a q)\) and carbon dioxide. The reaction can be monitored because the dichromate ion \(\left(\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}\right)\) is orange in solution, and the \(\mathrm{Cr}^{3+}\) ion is green. The unbalanced redox equation is $$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}(a q) \rightarrow \mathrm{Cr}^{3+}(a q)+\mathrm{CO}_{2}(g)$$ If 31.05 \(\mathrm{mL}\) of 0.0600\(M\) potassium dichromate solution is required to titrate 30.0 \(\mathrm{g}\) of blood plasma, determine the mass percent of alcohol in the blood.

Assign the oxidation state for nitrogen in each of the following. a \(\mathrm{L}_{3} \mathrm{N} \quad\) d. NO \(\quad\) g. \(\mathrm{NO}_{2}^{-}\) b. \(\mathrm{NH}_{3} \quad\) e. \(\mathrm{N}_{2} \mathrm{O} \quad\) h. \(\mathrm{NO}_{3}^{-}\) c\(\mathrm{N}_{2} \mathrm{H}_{4} \quad\) f. \(\mathrm{NO}_{2} \quad\) i. \(\mathrm{N}_{2}\)

Write net ionic equations for the reaction, if any, that occurs when aqueous solutions of the following are mixed. a. chromium(III) chloride and sodium hydroxide b. silver nitrate and ammonium carbonate c. copper(II) sulfate and mercury(I) nitrate d. strontium nitrate and potassium iodide

One of the classic methods for determining the manganese content in steel involves converting all the manganese to the deeply colored permanganate ion and then measuring the absorption of light. The steel is first dissolved in nitric acid, producing the manganese(II) ion and nitrogen dioxide gas. This solution is then reacted with an acidic solution containing the periodate ion; the products are the permanganate and iodate ions. Write balanced chemical equations for both of these steps.

Write the balanced formula equation for the acid–base reactions that occur when the following are mixed. a. potassium hydroxide (aqueous) and nitric acid b. barium hydroxide (aqueous) and hydrochloric acid c. perchloric acid \(\left[\mathrm{HClO}_{4}(a q)\right]\) and solid iron(III) hydroxide d. solid silver hydroxide and hydrobromic acid e. aqueous strontium hydroxide and hydroiodic acid
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