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Chapter 4: 4.15 (page 208)

What is the percent of chloride ion in a sample if 1.324g of sample produces 1.0881g of AgCl when treated with excess Ag+\(A{g^ + } + C{l^ - } \to AgCl\)

Short Answer

Expert verified

23.76% of chloride ion is present.

Step by step solution

01

Determine no of moles

Moles of AgCl=1.0881/143.3= 0.00759 mol or 7.59 x 10-3 mol

From the reaction, we can see that 1mol of Cl- gives 1 mol of AgCl

So, 7.59 x 10-3 mol of AgCl= 7.59 x 10-3 of Cl-

Also, 1 mol of Cl-=35.453g

7.59 x 10-3 moles of Cl-

= 7.59 x 10-3 x 35.453 g

=0.269g of Cl-

02

Mass percent

\(\begin{array}{l} = \frac{{Mass\,of\,C{l^ - }}}{{Total\,mass}} \times 100\\ = \frac{{0.2691}}{{1.1324}} \times 100\\ = 23.76\% \end{array}\)

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Most popular questions from this chapter

Classify the following as acid-base reaction or oxidation-reduction reactions.

(a)\(N{a_2}S\left( {aq} \right) + 2HCl\left( {aq} \right) \to 2NaCl\left( {aq} \right) + {H_2}S\left( g \right)\)

(b)\(2Na\left( s \right) + 2HCl\left( {aq} \right) \to 2NaCl\left( {aq} \right) + {H_2}\left( g \right)\)

(c)\(Mg\left( s \right) + C{l_2}\left( g \right) \to MgC{l_2}\left( s \right)\)

(d)\(MgO\left( s \right) + 2HCl\left( {aq} \right) \to MgC{l_2}\left( {aq} \right) + {H_2}O\left( l \right)\)

(e)\({K_3}P\left( s \right) + 2{O_2}\left( g \right) \to {K_3}P{O_4}\left( s \right)\)

(f)\(3KOH\left( {aq} \right) + {H_3}P{O_4}\left( {aq} \right) \to {K_3}P{O_4}\left( {aq} \right) + 3{H_2}O\left( l \right)\)

Fill in the blank with a single chemical formula for a covalent compound that will balance the equation:

A novel process for obtaining magnesium from sea water involves several reactions. Write a balanced chemical equation for each step of the process.

(a)The first step is the decomposition of solid calcium carbonate from seashells to form solid calcium oxide and gaseous carbon dioxide.

(b)The second step is the formation of solid calcium hydroxide as the only product from the reaction of the solid calcium oxide with liquid water.

(c)Solid calcium hydroxide is the added to the sea water, reacting with dissolved magnesium chloride to yield solid magnesium hydroxide and aqueous calcium chloride

(d)The solid magnesium hydroxide is added to a hydrochloric acid solution, producing dissolved magnesium chloride and liquid water.

(e)Finally, the magnesium chloride is melted and electrolyzed to yield liquid magnesium metal and diatomic chlorine gas.

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?

A 0.025-g sample of a compound composed of boron and hydrogen, with a molecular mass of ~28 amu, burns spontaneously when exposed to air, producing 0.063 g of B2O3. What are the empirical and molecular formulas of the compound?
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