Question

A mixture of NaCl and NaBr has a mass of 2.07 g and is found to...

A mixture of NaCl and NaBr has a mass of 2.07 g and is found to contain 0.73 g of Na. What is the mass of NaBr in the mixture?

Homework Answers

Answer #1

no of mol of Na IN SAMPLE = 0.73/23 = 0.03174 mol

Mass of sample = mass of NaBr + mass of NaCl

         2.07   = n*Mwt of NaBr + n*Mwt of NaCl

         2.07   = (x*103+(0.03174-x)*58.5)

   x = no of mol of NaBr in sample = 0.00479 mol

mass of NaBr in the mixture = 0.00479*103

                            = 0.4934 g

Know the answer?
Your Answer:

Post as a guest

Your Name:

What's your source?

Earn Coins

Coins can be redeemed for fabulous gifts.

Not the answer you're looking for?
Ask your own homework help question
Similar Questions
Can someone show me step my step solution to this question... A mixture of NaCl and...
Can someone show me step my step solution to this question... A mixture of NaCl and NaBr has a mass of 2.00 g and contains 0.75 g of Na. What is the mass of NaBr in the mixture?
A mixture consisting of only rubidium chloride (RbCl, 120.92 g/mol) and sodium chloride (NaCl, 58.44 g/mol)...
A mixture consisting of only rubidium chloride (RbCl, 120.92 g/mol) and sodium chloride (NaCl, 58.44 g/mol) weighs 1.0333 g. When the mixture is dissolved in water and an excess of silver nitrate is added, all the chloride ions associated with the original mixture are precipitated as insoluble silver chloride (AgCl, 143.32 g/mol). The mass of the silver chloride is found to be 1.6048 g. Calculate the mass percentage of rubidium chloride in the original mixture.
A mixture contains only NaCl and Al2(SO4)3. A 1.75-g sample of the mixture is dissolved in...
A mixture contains only NaCl and Al2(SO4)3. A 1.75-g sample of the mixture is dissolved in water, and an excess of NaOH is added, producing a precipitate of Al(OH)3. The precipitate is filtered, dried, and weighed. The mass of the precipitate is 0.134 g. What is the mass percent of Al2(SO4)3 in the sample?
A mixture of NaBr, Nal and NaNO3 weights 0.6500 g. By treating it with AgNO3 a...
A mixture of NaBr, Nal and NaNO3 weights 0.6500 g. By treating it with AgNO3 a halide precipitated is formed weighing 0.9390 g. By heating this precipitate in Cl2 current it becomes AgCl that weights 0.6566 g. What is the percentage of NaNO3 in the original sample?
A 0.3146 g sample of a mixture of NaCl(s) and KBr(s) was dissolved in water. The...
A 0.3146 g sample of a mixture of NaCl(s) and KBr(s) was dissolved in water. The resulting solution required 54.50 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. Mass Percentage:__________________
A reaction of 47.7g of Na and 34.7 g of Br2 yields 37.0g of NaBr. What...
A reaction of 47.7g of Na and 34.7 g of Br2 yields 37.0g of NaBr. What is the percent yield? 2 Na (s) + Br2 (g) ---------------> 2 NaBr (s)
A mixture of Na2CO3 and NaHCO3 has a mass of 82.6 g . It is dissolved...
A mixture of Na2CO3 and NaHCO3 has a mass of 82.6 g . It is dissolved in 1.00 L of water and the pH is found to be 9.92. Find the mass of NaHCO3 in the mixture. Express your answer with the appropriate units. m=
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 47.50 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 0.3146-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 47.20 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 0.3146-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 43.30 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.