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CHE 110 Lecture Notes - Lecture 11: Ice Cream, Osmotic Pressure, Semipermeable Membrane

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School
ISU
Department
Chemistry
Course
CHE 110
Professor
Sarah Boesdorfer

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Document Summary

How do you dilute a salt water solution: add water. Did the number of moles of salt in the solution change: no. Moles in solution can be calculated by taking m x v, so the moles before adding water. = moles after adding water though the concentrations and volumes are different: m1*v1 = m2*v2, 1 = initials, 2 = nals. 0. 0094 l or 9. 4 ml: how much water must be added to 500. 0 ml of 0. 200 m hcl to make 0. 150 m. 167 ml: how many grams of agcl precipitate when excess nacl is added to 1. 50 l of 0. 100. Properties affected by creating solutions: boiling point (elevates, melting point (decreases, both dependent on number of particles in solution not identity (colligative property) Nacl- 2 times particles (ionic so split particles na+ and cl-) Cacl2- will freeze at lower temp, has more particles. Why boiling point raised: vapor pressure.

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Related Questions

1.This question has multiple parts. Work all the parts to get the most points.

a

In each of the following sets of ionic compounds, identify the members of the set that are soluble in water.

(Select all that apply.)

NH4I

NH4HCO3

NH4NO2

NH4NO3

b

(Select all that apply.)

NaCH3COO

AgCH3COO

Cu(CH3COO)2

Cr(CH3COO)3

c

(Select all that apply.)

CaBr2

Ca(OH)2

CaSO4

CaCl2

d

(Select all that apply.)

Ca(NO3)2

CaSO4

CaCO3

Ca3(PO4)2

2.Calculate the mass percent of solute in the following solutions.

(a) 8.94 g of NaCl dissolved in 55.5 g of H2O

%

(b) 3.52 g of LiBr dissolved in 38.6 g of H2O

%

(c) 14.4 g of KNO3 dissolved in 260 g of H2O

%

(d) 2.6×10-3 g of NaOH dissolved in 3.8 g of H2O

%

3.How many grams of water must be added to 49.5 g of NaOH in order to prepare a 6.73%(m/m) solution?

grams of water

4.Calculate the volume percent of 495 mL of acetone in enough water to give 1.07×103 mL of solution.

%(v/v)

5.How many grams of Na2CO3 are needed to prepare 49.5 mL of a 4.27%(m/v) Na2CO3 solution?

grams of Na2CO3

6.For each of the following solutions, calculate the molarity of the solution.

9.87 g MgNH4PO4 in 750. mL solution

mol/L

19.1 g NaCH3COO in 600. mL solution

mol/L

6.64 g CaC2O4 in 300. mL solution

mol/L

5.58 g (NH4)2SO4 in 500. mL solution

mol/L

7.Calculate the number of grams of solute in each of the following solutions.

(a) 4.95 L of a 2.44 M HCl solution

grams of HCl

(b) 38.0 mL of a 12.5 M HNO3 solution

grams of HNO3

(c) 50.7 mL of a 10.4 M AgNO3 solution

grams of AgNO3

(d) 1.77 L of a 6.3×10-3 M Na2SO4 solution

grams of Na2SO4

8.Calculate the mass-volume percent concentration for a 8.9 M NaOH solution.

%

9.What is the molarity of the solution prepared by diluting 35.0 mL of 1.25 M AgNO3 to each of the following final volumes?

69.6 mL

M

84.9 mL

M

810 mL

M

2.57 L

Balance the following Chemical Equations:

____Fe(s) + ____H2O(g) ® ____Fe3O4(s) + ____H2(g)

____C2H6(g) + ____O2(g) ® ____CO2(g) + ____H2O(g)

(C) ___ KClO3 (s) ® ___ KCl (s) + ___ O2 (g)

___ C6H14 (l) + ___ O2 (g) ® ___ CO2 (g) + ___ H2O (g)

___ C3H8O3 (l) + ___ O2 (g) ® ___ CO2 (g) + ___ H2O (l)

___ NaN3 (s) ® ___ Na (s) + ___ N2 (g)

__ C3H5N3O9 ® __ CO2 + ___ N2 + ___ H2O + ___ O2

Write and Balance the equations:

Aqueous calcium hydroxide reacts with aqueous sodium carbonate to produce solid calcium carbonate and aqueous sodium hydroxide.

Solid iron reacts with Oxygen gas to form solid Iron (II) oxide

Copper(II) sulfide is oxidized by molecular oxygen to produce gaseous sulfur trioxide and solid copper(II) oxide. The gaseous product then reacts with liquid water to produce liquid hydrogen sulfate as the only product. Write the two equations which represent these reactions.

Indicate what type, or types, of reaction each of the following represents: (precipitation, acid-base, and oxidation-reduction.)

(A) H2O(g) + C(s) ⟶ CO(g) +H2(g)

(B) 2KClO3(s) ⟶ 2KCl(s) +3O2(g)

(C) Al(OH)3(aq) +3HCl(aq) ⟶ AlCl3(aq) + 3H2O(l)

(D) Pb(NO3)2(aq) + H2SO4(aq) ⟶ PbSO4(s) + 2HNO3(aq)

4. Silver can be separated from gold because silver dissolves in nitric acid while gold does not. Is the dissolution of silver in nitric acid an acid-base reaction or an oxidation-reduction reaction? Explain your answer.

5. Determine the oxidation states of the elements in the compounds listed. None of the oxygen-containing compounds are peroxides or superoxides.

(A) H3PO4

(B) Al(OH)3

(C) SeO2

6. Complete and balance the following acid-base equations:

(A) A solution of HClO4 is added to a solution of LiOH.

(B) Aqueous H2SO4 reacts with NaOH.

7. Write the molecular, total ionic, and net ionic equations for the following reactions:

(A) Ca(OH)2(aq) + HC2H3O2(aq) ⟶

(B) H3PO4(aq) + CaCl2(aq) ⟶

8. Write the balanced equation, then calculate the number of moles and the mass of Mg required to react with 5.00 g of HCl and produce MgCl2 and H2. Ans: 1.67 g Mg

9. H2 is produced by the reaction of 118.5 mL of a 0.8775-M solution of H3PO4 according to the following equation: 2Cr + 2H3PO4 ⟶ 3H2 + 2CrPO4. How many grams of H2 are produced? Ans: .315 g H2

10. Automotive air bags inflate when a sample of sodium azide, NaN3, is very rapidly decomposed.

2NaN3(s) ⟶ 2Na(s) + 3N2(g)

What mass of sodium azide is required to produce 2.6 ft3 (73.6 L) of nitrogen gas with a density of 1.25 g/L?

Ans: 142 g NaN3

11. Urea, CO(NH2)2, is manufactured on a large scale for use in producing urea-formaldehyde plastics and as a fertilizer. What is the maximum mass of urea that can be manufactured from the CO2 produced by combustion of 1.00 x 104 grams of CO2?

CO2(g) + 2NH3(g) ⟶ CO(NH2)2(s) + H2O(l)

Ans: 1360 g urea

12. What volume o f 0.750 M hydrochloric acid solution can be prepared from the HCl produced by the reaction of 25.0 g of NaCl with excess sulfuric acid? NaCl(s) + H2SO4(l) ⟶ HCl(g) + NaHSO4(s)

Ans: .570 L

13. A sample of 0.53 g of carbon dioxide was obtained by heating 1.31 g of calcium carbonate. What is the percent yield for this reaction? CaCO3(s)⟶CaO(s) + CO2(s)

Ans: 92.0 %

14. Citric acid, C6H8O7, a component of jams, jellies, and fruity soft drinks, is prepared industrially via fermentation of sucrose by the mold Aspergillus niger. The equation representing this reaction is

C12H22O11 + H2O +3O2 ⟶2C6H8O 7+ 4H2O

What mass of citric acid is produced from the reaction of 150. grams of sucrose if the yield is 92.30%?

Ans: 155 g

15. The phosphorus pentoxide used to produce phosphoric acid for cola soft drinks is prepared by burning phosphorus in oxygen.

(A) What is the limiting reactant when 0.200 mol of P4 and 0.200 mol of O2 react according to P4+5O2 ⟶ P4O10?

(B) Calculate the percent yield if 10.0 g of P4O10 is isolated from the reaction.

Ans: 88.0 %

16. What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? Li + N2 ⟶ Li3N

Ans: Li

17. What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO3 requires 20.22 mL of the AgNO3 solution to reach the end point?

AgNO3(aq) + NaCl(aq) ⟶ AgCl(s) +NaNO (aq)

Ans: .3374 M

18. In a common medical laboratory determination of the concentration of free chloride ion in blood serum, a serum sample is titrated with a Hg(NO3)2 solution.

2Cl−(aq) + Hg(NO3)2(aq) ⟶ 2NO3−(aq) + HgCl2(s)

What is the Cl− concentration in a 0.25-mL sample of normal serum that requires 1.46 mL of .000825 M Hg(NO3)2(aq) to reach the end point?

Ans: 0.009636 M

HERE IS HOW THIS IS GOING TO WORK! IF YOU ANSWER THE QUESTIONS IWILL GIVE YOU THE 3K POINTS + MORE AFTER I REPOST IT.





2. The amount of heat involved in the synthesis of 1 mole of acompound from its elements, with all substances in their standardstates at 25*C, is called _________.


3. What is a valid unit for specific heat?


4. Use Hess's Law to find the heat of reaction in the examplebelow.

N2O4 (g) ----> 2NO2 (g)


Given that:

N2O4 (g) ----> N2 (g) + 2O2 (g) (Delta H =-9.7kJ)

2NO2 (g) ----> 2O2(g) + N2(g) ( Delta H= -67.7kJ)


5. Use Hess's Law to find the heat of reaction in the examplebelow. (Example doesn't exist btw.)


6. (Delta H) for the formation of rust (Fe2O3) is -826 kJ/mol. Howmuch energy is involved in the formation of 5 grams ofrust?


7. How many kilocalories of heat are required to raise thetemperature of 50g of aluminum from -5*C to 35*C? (Specific heat ofAluminum = 0.21 cal/g*C)


8.Calculate the (Delta H) for this reaction:


Zn(s) + Cu (2+ ion)(aq) ---> Zn(2+) + Cu(s)

(Delta H) for Cu(2+) = +64.4 kJ/Mol; (Delta H) for Zn(2+) = -152.4kJ/mol


9. The following equation shows the reaction that occurs whennitroglycerine explodes.

4C3H5O9N3 ----> 12CO2 + 6N2 + O2 +10H2O + 1725 Kcal


Is this reaction exothermic , endothermic, a combustion reaction ,or a combination reaction?


10. What does it mean for ammonia, (NH3) to have a (Delta H f) =-46 kJ/mol?

(for example: Define heat of formation. What does a negative heatof formation mean? what do the units of kJ/mol mean?)


11. What is the maximum amount of KCl that can dissolve in 500g ofwater?

(solubility of KCl is 34 g/ 100g of water at 20*C)


12.List the ways(operations) that can help make a substancedissolve faster in a solvent?


13. If a crystal added to an aqueous solution causes many particlesto come out of solution, the original solution was (saturate,unsaturated, supersaturated).


14. What is the number of moles of solute in 165 mL of a 0.82 Msolution?


15. What mass of NaCl is needed to make 350 mL of a 1.00 Msolution?


16. Colligative properties depend upon...


17. If one mole of each of these solutes in added to the sameamount of water, which solution has the highest boiling point?(glucose, aluminum sulfate, magnesium acetate, copper (I)chloride)


18. When an acid reacts with a base, what compounds areformed?


19. If the [H+] in a solution is 1x10^(-13) mol/L, what is the[OH-]?


20. If the [OH-] = 1x10^-6 mol/L, what is the pH of thesolution?


21. For a solution to be considered acidic what must be thehydrogen-ion concentration?


22. Which of the following represents a Bronsted-Lowry conjugateacid-base pair?

a) SO3(2-) and SO2 b) CO3(2-) and CO c) H3O and H2 d) NH4(+) and NH3


23. With solutions of "strong" acids and "strong" bases, the word"strong" refers to ...


24. What are the products of Al(OH)3 + H2CO3?


25.What is the concentration of hydrochloric acid if 5.0 mL of acidis neutralized by 30.0 mL of 2.00M sodium hydroxide.


26. At equilibrium, what is the rate of production of reactantscompared with the rate of production of products?


27. What is the equilibrium constant for the following reaction2SO3 ---> 2SO2 + O2


28. How does an increase in pressure affect the following reaction?2SO3 (g) --> 2SO2(g) +O2(g)


29.What stresses would shift the reaction to the right?

2SO3(g) ==> 2SO2(g) + O2(g)







30. The Keq of a reaction 4.9 x 10^(-7). Are products or reactantsfavored at equilibrium?


31. In which of these systems is the entropy decreasing?

a) air escaping from a tire b) snow melting c) a gas condensing d) salt dissolving inwater



32. If an atom is reduced in a redox reaction, what must occur toanother atom in the system?


33. Identify the oxidizing agent in the following reaction: 2Na + S---> Na2S


34. What are transferred in an oxidation -reductionreaction?


35. Give the oxidation number for each atom in KMnO4.


36. Which atom has a change in oxidation number of +4 in thefollowing reaction?

K2Cr2O7 + H2O + S ----> KOH + Cr2O3 +SO2


37. What is the oxidation number of sulfur in each of the following:

a. SO3 c.SO2(2-)

b. Na2SO4 d. S2O4 (2-)


38.Fe(3+) ----> Fe represents oxidation, reduction, orhydrolysis?


39. When the half reactions Br2+ 2e- -----> 2Br- and Na---->e- + Na(+) are combined the balanced redox equation is_____________________ ( WRITE the BALANCED REDOX eq)


40. To balance the oxygen and hydrogen for a redox reaction thattakes place in basic solution, it is necessary to use whichsubstance?


41. What particle completes this nuclear equation? 55/25 Mn + 2/1 H====> _____ +2 1/0 n


42. The half-life of tungsten-182 (182/74 W) is 1.1x10^(17) years.How long would it take for a 376.2 kg sample to decay until only123.0 grams remain?


43. After 3 days, the quantity of certain radioisotope is reducedfrom 13.6 grams to 1.9 grams. Calculate the half-life of theisotope.


44. What is the name of the compound having the formulaC8H18.


45. What is the name of the following compound:

O

//

CH3---CH2----CH---CH2--C

I \

CH3 OH


46. What is an isomer? Give an isomer of hexane (C6H14) and drawit's structure.


47. What is the name of the hydrocarbons with double covalentbonds?


48. Draw the stucture for 3-methylbutanoic acid.


49. Draw the structure for methylbenzene?


50. What is the name of the following compound:


Br

|

CH3----C-----CH3

|

CH3