6. A salt mixture of NaCl and KCI has a mass of 0.887 g. The mixture was dissolved in water and titrated with excess AgNO3 to produce 1.913 g of AgCl. Assume that the mol of Cl- ion from each salt is equal. Calculate the mass of each compound in the salt mixture. (Relative molecular mass, g mol-¹: NaCl = 58.5, KCI = 74.6, AgCl =143.4 g/mol) Ag+ (aq) + Ct (aq) →→→ AgCl (aq) -
6. A salt mixture of NaCl and KCI has a mass of 0.887 g. The mixture was dissolved in water and titrated with excess AgNO3 to produce 1.913 g of AgCl. Assume that the mol of Cl- ion from each salt is equal. Calculate the mass of each compound in the salt mixture. (Relative molecular mass, g mol-¹: NaCl = 58.5, KCI = 74.6, AgCl =143.4 g/mol) Ag+ (aq) + Ct (aq) →→→ AgCl (aq) -
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![1. a) Boron, ¹B has relative atomic mass of 10.81 amu and its mass number is
11 amu. Explain why the relative atomic mass and its mass number is
different.
c) Sulfurous acid reacts with ammonium hydroxide to form salt and water.
Write a balanced chemical equation for the reaction and name the salt
produced.
2. Magnesium has relative atomic mass of 24.31 amu. There are three naturally
occurring isotopes of magnesium which are Mg-24, Mg-25 and Mg-26. The
relative abundance of isotope Mg-24 (23.985 amu) is 79.00%. If the relative
isotopic mass of Mg-26 is 25.983 amu and the ratio of fractional abundance of
Mg-25 to Mg-26 is 0.908, find the relative isotopic mass of Mg-25.
[Ans: 25.01 amu]
3. Aniline, a starting compound for urethane plastic foams, consists of C, H, and
N. Combustion of such compounds yields CO2, H₂O, and N2 as products. If
the combustion of 9.71 g of aniline yields 6.63 g H₂O and 1.46 g N2, find the
empirical formula of aniline. (Relative molecular mass, g mol-¹: H₂O = 18.0,
N₂ = 28.0, C = 12.0)
[Ans: C6H¬M]
4. Calcium hydroxide, Ca(OH)2 is produced by reacting 2.5 moles of calcium
chloride, CaCl₂ and 3.2 moles of sodium hydroxide, NaOH following the
equation below.
CaCl2 (s) + 2NaOH (aq) → Ca(OH)2 (s) + 2NaCl (aq)
a) Identify the limiting reactant and calculate the theoretical yield (mol) for the
reaction.
b) Calculate the moles of excess reactant that remain.
[Ans: 0.90 moŋ]
5. An aqueous solution of ethylene glycol, C₂H6O2 has 40.0% by mass.
Determine the molality (m) of C₂H6O₂ in this solution. (Relative molecular
mass of C₂H6O2 is 62.0 g/mol)
[Ans: 10.8 m]
6. A salt mixture of NaCl and KCI has a mass of 0.887 g. The mixture was
dissolved in water and titrated with excess AgNO3 to produce 1.913 g of AgCl.
Assume that the mol of Cl- ion from each salt is equal. Calculate the mass of
each compound in the salt mixture. (Relative molecular mass, g mol-¹: NaCl =
58.5, KCI = 74.6, AgCl =143.4 g/mol)
Ag+ (aq) + Ct (aq) → AgCl (aq)
[Ans: NaCl = 0.390 g, KCI= 0.497 g]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F99035a01-21cc-457e-aa7b-608d8c373f3f%2F7b2f1752-d24d-4334-93d7-02ea42ffdad7%2Fjj5spqc_processed.jpeg&w=3840&q=75)
Transcribed Image Text:1. a) Boron, ¹B has relative atomic mass of 10.81 amu and its mass number is
11 amu. Explain why the relative atomic mass and its mass number is
different.
c) Sulfurous acid reacts with ammonium hydroxide to form salt and water.
Write a balanced chemical equation for the reaction and name the salt
produced.
2. Magnesium has relative atomic mass of 24.31 amu. There are three naturally
occurring isotopes of magnesium which are Mg-24, Mg-25 and Mg-26. The
relative abundance of isotope Mg-24 (23.985 amu) is 79.00%. If the relative
isotopic mass of Mg-26 is 25.983 amu and the ratio of fractional abundance of
Mg-25 to Mg-26 is 0.908, find the relative isotopic mass of Mg-25.
[Ans: 25.01 amu]
3. Aniline, a starting compound for urethane plastic foams, consists of C, H, and
N. Combustion of such compounds yields CO2, H₂O, and N2 as products. If
the combustion of 9.71 g of aniline yields 6.63 g H₂O and 1.46 g N2, find the
empirical formula of aniline. (Relative molecular mass, g mol-¹: H₂O = 18.0,
N₂ = 28.0, C = 12.0)
[Ans: C6H¬M]
4. Calcium hydroxide, Ca(OH)2 is produced by reacting 2.5 moles of calcium
chloride, CaCl₂ and 3.2 moles of sodium hydroxide, NaOH following the
equation below.
CaCl2 (s) + 2NaOH (aq) → Ca(OH)2 (s) + 2NaCl (aq)
a) Identify the limiting reactant and calculate the theoretical yield (mol) for the
reaction.
b) Calculate the moles of excess reactant that remain.
[Ans: 0.90 moŋ]
5. An aqueous solution of ethylene glycol, C₂H6O2 has 40.0% by mass.
Determine the molality (m) of C₂H6O₂ in this solution. (Relative molecular
mass of C₂H6O2 is 62.0 g/mol)
[Ans: 10.8 m]
6. A salt mixture of NaCl and KCI has a mass of 0.887 g. The mixture was
dissolved in water and titrated with excess AgNO3 to produce 1.913 g of AgCl.
Assume that the mol of Cl- ion from each salt is equal. Calculate the mass of
each compound in the salt mixture. (Relative molecular mass, g mol-¹: NaCl =
58.5, KCI = 74.6, AgCl =143.4 g/mol)
Ag+ (aq) + Ct (aq) → AgCl (aq)
[Ans: NaCl = 0.390 g, KCI= 0.497 g]
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