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Chapter 27: Q1TY (page 752)

How many grams ofBr-were in a sample that produced 1.000 g of

AgBr precipitate (FM 5 187.77)?

Short Answer

Expert verified

The number of bromide ions generated in a sample that can cause silver bromide precipitation is 0.4255g

Step by step solution

01

Define molarity

The ratio of moles of solute to the volume of the solution is known as molarity (in litres).

Molartiv(M) = Moles of solute(inmol)

02

Find the mass of  AgBr

The amount of bromide ions generated in a sample that can result in silver bromide precipitation.

The number of moles of silver bromide is computed using 1.00 g of AgBr

The number of moles of silver bromide to the number of moles of bromide ion is 1 : 1

Molarmass=MassMole=79.904g/mol脳0.00533=0.4255g

Therefore, the amount of bromide ions formed in a sample that can produce silver bromide precipitate is 0.4255 g.

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Most popular questions from this chapter

Marie Curie dissolved 0.091 92 g of RaCl2 and treated it with excess AgNO3to precipitate 0.088 90 g of AgCl. In her time (1900), the atomic mass of Ag was known to be 107.8 and that of Cl

was 35.4. From these values, find the atomic mass of Ra that Marie Curie would have calculated.

We now examine some examples that illustrate how to relate the mass of a gravimetric precipitate to the quantity of the original analyte. The general approach is to relate the moles of product to the moles of reactant.

LaCoO3+x, has a perovskite structure (Box 19-1) with variable oxygen content. The figure shows the thermogravimetric curve observed when 41.8724m gwere heated in role="math" localid="1665035505591" 5vol%H2inAr.La(II)does not react, but cobalt is reduced to Co(s)

(a) What is the oxidation state of cobalt in the ideal formula LaCoO3

(b) Write the reaction of role="math" localid="1665035588740" LaCoO3withH2 to produce La2O3with(s),Co(s),andH2O(s)

(c) If 41.8724mgofLaCoO3 react completely, what will be the mass of product(La2O3+(Co)?

(d) Write the balanced reaction of role="math" localid="1665035782894" LaCoO3+xwithH2O to produce La2O3,Co,andH2O.If41.8724mgofLaCoO3+1react completely; what will be the mass of solid product? Your answer will be an expression with x in it.

(e) From the observed product mass (37.767mg)at700掳c, find x inLaCoO3+x Write the formula of the starting solid.

(f) In part (c), the mass lost from the ideal formula LaCoO3+x, is 4.0877 mg. What is the product nearrole="math" localid="1665035980286" 500掳Cwhere the mass is -40.51 mg?

What is the purpose of theWO3 and Cu in Figure 27-8?

Explain how the quartz crystal microbalance at the opening of Chapter 2 measures small masses
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