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Chapter 22: Problem 76

(a) Determine the number of sodium ions in the chemical formula of albite, \(\mathrm{Na}_{x} \mathrm{AlSi}_{3} \mathrm{O}_{8}\) . (b) Determine the number of hydroxide ions in the chemical formula of tremolite, \(\mathrm{Ca}_{2} \mathrm{Mg}_{5}\left(\mathrm{Si}_{4} \mathrm{O}_{11}\right)_{2}(\mathrm{OH})_{x}\)

Short Answer

Expert verified
(a) The number of sodium ions in the chemical formula of albite, \(\mathrm{Na}_{x} \mathrm{AlSi}_{3} \mathrm{O}_{8}\), is 1. (b) The number of hydroxide ions in the chemical formula of tremolite, \(\mathrm{Ca}_{2}\mathrm{Mg}_{5}\left(\mathrm{Si}_{4}\mathrm{O}_{11}\right)_{2}(\mathrm{OH})_{x}\), is 1.

Step by step solution

01

Identify the subscript of sodium ions in the chemical formula of albite

The given chemical formula for albite is \(\mathrm{Na}_{x} \mathrm{AlSi}_{3} \mathrm{O}_{8}\). Sodium ions are represented by \(\mathrm{Na}\). According to the formula, the subscript for sodium ions is `x`.
02

Determine the number of sodium ions in the chemical formula of albite

The subscript for sodium ions in the chemical formula of albite is `x`. Since there is no numerical value given, it means there is only 1 sodium ion present in the formula. So we have found that the number of sodium ions in albite is 1.
03

Identify the subscript of hydroxide ions in the chemical formula of tremolite

The given chemical formula for tremolite is \(\mathrm{Ca}_{2}\mathrm{Mg}_{5}\left(\mathrm{Si}_{4}\mathrm{O}_{11}\right)_{2}(\mathrm{OH})_{x}\). Hydroxide ions are represented by \(\mathrm{OH}\). The subscript for hydroxide ions in the formula is `x`.
04

Determine the number of hydroxide ions in the chemical formula of tremolite

The subscript for hydroxide ions in the chemical formula of tremolite is `x`. Since there is no numerical value given, it means there is only one hydroxide ion present in the formula. So we have found that the number of hydroxide ions in tremolite is 1.

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Most popular questions from this chapter

Complete and balance the following equations:$$\begin{array}{l}{\text { (a) } \mathrm{Mg}_{3} \mathrm{N}_{2}(s)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow} \\ {\text { (b) } \mathrm{NO}(g)+\mathrm{O}_{2}(g) \longrightarrow} \\ {\text { (c) } \mathrm{N}_{2} \mathrm{O}_{5}(g)+\mathrm{H}_{2} \mathrm{O}(I) \longrightarrow}\end{array}$$ $$ \begin{array}{l}{\text {{d} ) ~ } \mathrm{NH}_{3}(a q)+\mathrm{H}^{+}(a q) \longrightarrow} \\ {\text { (e) } \mathrm{N}_{2} \mathrm{H}_{4}(l)+\mathrm{O}_{2}(g) \longrightarrow}\end{array} $$ Which ones of these are redox reactions?

Write the chemical formula for each of the following, and indicate the oxidation state of the halogen or noble-gas atom in each: (a) calcium hypobromite, (b) bromic acid, (c) xenon trioxide, (d) perchlorate ion, (e) iodous acid,(f) iodine pentafluoride.

Borazine, \((\mathrm{BH})_{3}(\mathrm{NH})_{3},\) is an analog of \(\mathrm{C}_{6} \mathrm{H}_{6},\) benzene. It can be prepared from the reaction of diborane with ammonia, with hydrogen as another product; or from lithium borohydride and ammonium chloride, with lithium chloride and hydrogen as the other products. (a) Write balanced chemical equations for the production of borazine using both synthetic methods. (b) Draw the Lewis dot structure of borazine. (c) How many grams of borazine can be prepared from 2.00 L of ammonia at STP, assuming diborane is in excess?

Manganese silicide has the empirical formula MnSi and melts at \(1280^{\circ} \mathrm{C}\) . It is insoluble in water but does dissolve in aqueous HF. (a) What type of compound do you expect MnSi to be: metallic, molecular, covalent- network, or ionic? (b) Write a likely balanced chemical equation for the reaction of MnSi with concentrated aqueous HF.

Write a balanced equation for each of the following reactions. (You may have to guess at one or more of the reaction products, but you should be able to make a reasonable guess, based on your study of this chapter.) (a) Hydrogen selenide can be prepared by reaction of an aqueous acid solution on aluminum selenide. (b) Sodium thiosulfate is used to remove excess \(\mathrm{Cl}_{2}\) from chlorine-bleached fabrics. The thiosulfate ion forms \(\mathrm{SO}_{4}^{2-}\) and elemental sulfur, while \(\mathrm{Cl}_{2}\) is reduced to \(\mathrm{Cl}^{-}\) .
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