Question

In: Chemistry

A 0.2368 sample contained only NaCl and KBr. It was dissolved in water and required 44.80...

A 0.2368 sample contained only NaCl and KBr. It was dissolved in water and required 44.80 mL of 0.04873 M AgNO3 for complete titration of both halides. Calculate the weight percent of Br in the solid sample. (answer is 60.85 but please show work)

Expert Solution

Molar mass of NaCl = 58.44g/mol

Molar mass of KBr = 119.00 g/mol

Let's say mass of NaCl = x

Mass of KBr =0.2368-x

Moles of NaCl = x/58.44

Moles of KBr = (0.2368-x)/119.00

KBr + AgNO3 = AgBr + KNO3

NaCl + AgNO3 = NaNO3 + AgCl

AgNO3 is completely consumed by these two reactions combined

Moles of AgNO3 used = molarity*volume in litres

= 0.04873M*0.0448L

= 0.002183 moles

Which is equal to moles of KBr+NaCl as seen from reaction equation that each of them need equavalent amount of AgNO3

0.002183 moles =x/58.44 + (0.2368-x)/119.00

15.18 = 119x +13.84 -58.44x

1.34 = 60.56x

x = 0.02213 g

Mass of KBr =0.2368-0.02213

=0.21467g

119.00 g KBr has 79.90g Br

0.21467g KBr has 0.14414 g Br

%Br = mass of Br/total mass *100

= 0.14414/0.2368 *100 = 60.86%

queen_honey_blossom answered 2 years ago

A 0.444 g sample contained only NaCl and KBr. It was dissolved in water and required...

A 0.444 g sample contained only NaCl and KBr. It was dissolved in water and required 81.13 mL of 0.05664 M AgNO3 for complete titration of both halides (giving AgCl (s) and AgBr (s)). Calculate the mass of KBr in the solid sample.

A 0.3146-g sample of a mixture of NaCl(s) and KBr(s) was dissolved in water. The resulting...

A 0.3146-g sample of a mixture of NaCl(s) and KBr(s) was dissolved in water. The resulting solution required 36.00 mL of 0.08765 M AgNO3(aq) to precipitate the Cl–(aq) and Br–(aq) as AgCl(s) and AgBr(s). Calculate the mass percentage of NaCl(s) in the mixture.

A 0.9140 g sample of a mixture of NaCl and KCl is dissolved in water, and...

A 0.9140 g sample of a mixture of NaCl and KCl is dissolved in water, and the solution is then treated with an excess of AgNO3 to yield 1.943 g of AgCl. Calculate the percent by mass of each compound in the mixture.

A 0.9000 g sample of a mixture of NaCl and KCl is dissolved in water, and...

A 0.9000 g sample of a mixture of NaCl and KCl is dissolved in water, and the solution is then treated with an excess of AgNO3 to yield 1.923 g of AgCl. Calculate the percent by mass of each compound in the mixture. ____% mass of NaCl ____% mass of KCl

A mixture contains only and . A 4.51-g sample of the mixture is dissolved in water...

A mixture contains only and . A 4.51-g sample of the mixture is dissolved in water and an excess of is added, producing a precipitate of . The precipitate is filtered, dried, and weighed. The mass of the precipitate is 1.06 g. What is the mass percent of in the sample? %

If 17.5 g of NaCl is dissolved in 100. g of water, what is the mass...

If 17.5 g of NaCl is dissolved in 100. g of water, what is the mass % concentration of NaCl in this solution? Note: 1. Use 3 sig figs for your final answer. 2. Do not answer as fractions. For example, if you think 30% is the correct answer, either "30" or "30%" will be accepted, but "0.30" will not. "30%" will actually be converted to 30 automatically

A kilogram of solution contains following particles dissolved in water 3g of NaCl and 5g of...

A kilogram of solution contains following particles dissolved in water 3g of NaCl and 5g of CaCl calculate the osmolarity of the solution ( molecular weight NaCl 58.44g/mol and 110.98g/mol forCaCl).

a 0.5153g solid sample containing only a mixture of LaCl3 & Ce(NO3)3 was dissolved in water....

a 0.5153g solid sample containing only a mixture of LaCl3 & Ce(NO3)3 was dissolved in water. Potassium iodate was then added to the obtained solution producing the precipitates La(IO3)3 molar mass 663.61 g/mol & Ce(IO3)3 molar mass 664.82 g/mol. the total mass of the precipitates was found to be equal to 1.1650g. Calc the % of LaCl3 and Ce(NO3)3 in the sample. i have to where there are two equations and two unknowns. I just don't know how to solve...

KBr crystallizes in a NaCl (B1) structure with a lattice constant of a=0.65966nm. Determine the bulk...

KBr crystallizes in a NaCl (B1) structure with a lattice constant of a=0.65966nm. Determine the bulk density of KBr and the distance between a K ion and a touching Br ion in the structure. Rationalize your result with the sum of ionic radii for K and Br

1) identify the substance that conducts electricity a)sugar dissolved in water b)water c)solid sugar d)solid NaCl...

1) identify the substance that conducts electricity a)sugar dissolved in water b)water c)solid sugar d)solid NaCl e)Nacl dissolved in water 2) using periodic trends, place the follwing bonds in order of increasing ionic character S-F Se-F O-F 3)Choose the bond below that is the strongest a)N=O b)N=N c)N-I d)N-O e)N-S