|
|
- Eustacia Adams
- 5 years ago
- Views:
Transcription
1 SOLUTIONS CHAPTER 9 TEXT BOOK EXERCISE Q1. Choose the correct answer for the given ones. (i) Morality of pure water is (a) 1. (b) 18. (c) 55.5 (d) 6. Hint: Morality of pure water Consider 1 dm 3 (-1000cm 3 ) of water. Convert this volume into mass by using density. Mass =volume x density Mass of H 2 O = 1000 cm 3 x 1 g cm 3 =1000g Molar mass of H 2 O =18 g mol -1 No. of moles of H 2 O = =55.6 mol Morality of H 2 O = = =55.6 mol dm -3 =55.6 M (ii) 18 g glucose is dissolved in 90 g of water. The relative lowering of vapour pressure is equal to (a) 1 (b) 18 (c) 55.5 (d) 6 (iii) A solution of glucose is 10%. The volume in which 1 g-mole of it is dissolved will be (a) 1 dm 3 (b) 1.8dm 3 (c) 200 cm 3 (d) 900cm 3 (iv) An aqueous solution of ethanol in water may have vapour pressure (a) equal to that of water (b) equal to that of ethanol (c) more than that of water (d) less than that of water 1
2 (v) An azeotropic mixture of two liquids boils at a lower temperature than either of them when (a) it is saturated (b) it shows positive deviation from Raoult s law (c) it shows negative deviation from Raoult s law (d) it is met stable (vi) In azeotropic mixture showing positive deviation from Raoult s law, the volume of the mixture is (a) slightly more than the total volume of the components (b) slightly less than the total volume of the components (c) equal to the total volume of the components (d) none of these (vii) Which of the following solution has the higher boiling point? (a) 5.85% solution of sodium chloride (b) 18.0% solution of glucose (c) 6.0% solution of urea (d) All have the same boiling point. (e) Two solution of NaC1and KC1 are prepared separately by dissolving same amount of solute in water. Which of the following statements is true for these solutions? (f) KC1 solution will have higher boiling point than NaC1 solution (g) Both the solution have different boiling points. (h) KC1 and NaC1 solutions possess same vapour pressure (i) KC1 solution possesses is the ratio of the elevation in boiling point to (j) The molal boiling point constant is the ratio of the elevation in boiling point to (a) molaritly (b) molality (c) mole fraction of solvent (d) mole fraction of solute (x) Colligative properties are the properties of (a) Dilute solutions which behave as nearly ideal non-ideal solutions 2
3 (b) Concentrated solutions which behave as nearly non-ideal solutions (c) Both (a) and (b) (d) Neither (a) and (b) Ans. (i) c (ii) c (iii) b (iv) c (v) b (vi) a (vii) a (viii) c (ix) b (x) a Q2. Fill in the blanks with suitable words or numbers. (i) Number of molecules of sugar in 1dm 3 of 1 M sugar solution is. (ii) 100 g of a 10% aqueous solution of NaOH contains 10 g NaOH in g of water. (iii) When an azeotropic mixture is distilled, its remains constant. (iv) The molal freezing point of an azeotropic solution of two liquids is lower than ether of them because the solution shows from Raoluls s law. (v) Among equimolal aqueous solution of NaC1, BaC1 2, and FeC1 3, the maximum depression in freezing point is shown by solution. (vi) A solution of ethanol in water shows deviations and gives azeotropic solutions with b.p. than other components. (vii) Colligative properties are used to calculate of a compound. (viii) The boiling point of an azeotropic solution of two liquids is lower than either of them because the solutions show from Raoult s law. (ix) The hydration energy of Br - ion is than that of F - ion. (x) The aqueous solution of NH 4 C1 is while that of Na 2 SO 4 is. 3
4 Ans. (i)6.02x (ii)90 (iii)composition (iv)cryoscopic (v)positive deviation (vi)fec1 3 (vii)positive ; lower (viii) molar mass (ix) lesser (x) acidic ;neutral Q3. Indicate True or False from the given statements. (i) At a definite temperature the amount of a solute in a given saturated solution is fixed. (ii) Polar solvents readily dissolve non-polar covalent compounds. (iii) The solubility of a substance decreases with increase in temperature if the heat of a solution is negative. (iv) The rate of evaporation of a liquid is inversely proportional to the intermolecular forces of attraction. (v) The molecular mass of an electrolyte determined by lowering of vapour pressure is less than the theoretical molecular mass. (vi) Boiling point elevation is directly proportional to the molality of the solution and inversely proportional to boiling point of solvent. (vii) All solutions containing 1 g of non-volatile non-electrolyte solutes in some solvent will have the same freezing point. (viii) The freezing point of a 0.05 molal solution of a non-volatile non-electrolyte solute in water is 0.93 o C. (ix) Hydration and hydrolysis are different process for Na 2 SO 4. (x) The hydration energy of an ion only depends upon its charge. Ans. (i) True (ii)false (iii)true (iv)true (v)true (vi) True (vii) False (viii) False (ix)true (x) False Q4. Define and explain the following with examples: (a) A homogeneous phase (b) A concentrated solution (c) A solution of solid in a solid (d) A consulate temperature (e) A non-ideal solution (f) Zeotropic solutions (g) Heat of hydration (h) Water of crystallization 4
5 (i) Azeotropic solution (j) Conjugate solution Q5. (a) What are the concentration units of solutions? Compare molar and molal solution. Ans. Compare molar and molal solution. Molar Solution Molar Solution 1. A solution which contains 1. A solution which contains one mole of solute per dm 3 of one mole of solute per kilogram solution is called a molar of solvent is called a molal solution. solution. 2. Its morality decreases with 2. Its molality is independent of the rise in temperature. temperature variation of 3. Its unit is mole dm 3 of solution. solution. 3. Its unit is mol kg -1 of solvent. (b) One has one molal solution of NaC1 and one molal solution of glucose. (i) Which solution has greater number of particles of solute? (ii) Which solution has greater amount of the solvent.? (iii) How do we convert these concentrations into weight by weight percentage? (b) (i) One molal solution of NaC1 has greater number of particles of solute. (ii) The amount of solvent in both solution is equal (1 kg) (iii) Mass of NaC1 = 58.5 g Mass of solvent =1000g Total mass of NaC1 solution = = g Percentage of NaC1 = x100 = x100=5.53 % Answer Mass of glucose =180g Mass of solvent =1000g 5
6 Total mass of solution = =1180 g % of glucose = x100 = x100=15.25 % Answer Q.6 Explain the following with reasons (i) The concentrations in terms of molality is independent of the temperature but morality depends upon temperature. Ans. Molality is based on the mass of solvent. The mass of solvent does not vary not vary with temperature, so molality is independent of temperature. Morality is based on the volume of solution. Since the volume of solution varies with temperature, so morality depends upon temperature. The morality of the solution decreases with the increase in temperature of the solution. (ii) The sum of the mole fractions of all the components is always equal to unity for any solution. Ans. Suppose there be two components A and B making a solution. The numbers of moles are n A and n B respectively, then. If the mole fractions of A and B are denoted by X A and X B respectively, then X A = and X B = The sum of mole fractions of the components of a solution will be X A + X B = + X A + X B = X A + X B =1 Hence, the sum of the mole fractions of all the components of any solution is always equal to unity. (iii) 100 g of 98% H 2 SO 4 has a volume of cm 3 of H 2 SO 4 since its density is 1.84 g cm -3. Ans. Mass of 98% H 2 SO 4 =100g : density of 98% =1.84 g cm -3 Vol. of 98% H 2 SO 4 =? 6
7 Formula Used: volume = = =54.34 cm -3 Hence, 100 g of 98 % H 2 SO 4 has a volume of cm -3 of H 2 SO 4 because its density is 1.84 g cm -3. (iv) Relative lowering of vapour pressure is independent of the temperature. Ans. Since, the relative lowering of vapour pressure is equal to the mole fraction of solute, so it is independent of temperature. Hint: =X 2 or = (v) Colligative properties are obeyed when the solute is nonelectrolyte and also when the solutions are dilute. Ans. Colligative properties are obeyed when the solute is nonelectrolyte Colligative properties depend only upon the number of solute particles and not on their chemical nature. An electrolyte solute differs from a non-electrolyte principally in the number of particles produced upon dissolution. In case the solute is non-electrolyte, one mole of solute produces one mole of dissolved particles (molecules). In case the solute is electrolyte, it may split into a number of ions each of which acts as a particle and thus will affect the colligative properties of solution than non-electrolytes. For example, one mole of glucose produces one mole of dissolved particles (molecules) while one mole of NaC1 produces two moles of dissolved particles (one mole each of Na + and C1 - ions). Thus, mole for mole, the NaC1 exerts twice the colligative effect than glucose if the solution is ideal. Colligative properties are obeyed when the solutions are dilute. Colligative properties are obeyed when the solutions are dilute. A dilute solution behaves almost as an ideal solution, i.e., the solute-solute interactions are negligible. Concentrated solution is mostly non-ideal. (vi) The total volume of the solution by mixing 100 cm 3 of water with 100 cm 3 of alcohol may not be equal to 200 cm 3. Justify it. 7
8 Ans. Because the intermolecular forces of attraction between alcohol and water molecules are not the same as the intermolecular attractive forces between alcohol molecules or between water molecules. Hence, the total volume of the solution by mixing 100 cm 3 of alcohol with 100 cm 3 of water will not be equal to 200 cm 3. The total volume of solution will be greater than 200 cm 3 because the forces of attraction between alcohol and water molecules are weaker than those between alcohol molecules or between water molecules. (vii) One molal solution of urea in water is dilute as compared to one molar solution of urea, but the number of particles of the solute is the same. Justify it. Ans. One molal solution of urea in water is dilute as compared to one molar solution of urea. This is because a molal solution contains one mole of urea in 1000 g of water whereas one molar solution contains one mole of urea in 1000 cm 3 of water. At room temperature, density of water is slightly less than one. Therefore, the volume corresponding to 1000 g of water be greater than 1000cm 3. So, the volume of solvent water containing one mole of solute is more in case of molal solution than molar solution. hence, one molal solution of urea in water is dilute as compared to one molar solution of urea in water. Since both the solutions contain 1 mole of urea as solute, therefore, the number of particles of solute is the same in both the solution. (viii) Non-ideal solution do not obey the Raoult s law. Ans. They show deviations from Raoult s law due to differences in their molecular structures, i.e., size, shape and intermolecular forces. Formation of such solutions is accompanied by changes in volume and enthalpy. The vapour pressure deviation may be positive or negative in such solutions. Q7. What are non-ideal solutions? Discuss their types and give three example of each. Q8. (a) Explain fractional distillation. Justify the two curves when composition is plotted against boiling point of solutions. 8
9 (b) The solution showing positive and negative deviations cannot be fractionally distilled at their specific compositions. Explain it. Q9. (a) What are azeotropic mixtures? Explain them with the help of graphs. (b) Explain the effect of temperature on phenol-water system. Q10. (a) What are collligative properties? Why are they called so? Ans. Because the colligative properties of solution depend only upon the number of solute and solvent particles present in the solution and not upon the chemical nature of the solute molecules. For this reason these properties are called colligative properties. (b) What is the physical significance of K B and k f values of solvent? Ans. Because the change in boiling point and the freezing point of a solvent is a colligative property that depends only on the ratio of the number of particles of solute an dissolvent in the solution, so these constants are used to determine the molecular mass of an unknown solute. Q11. How to explain that the lowering of vapour pressure is a colligative property? How do we measure the molar mass of a non-volatile, nonelectrolyte solute in a volatile solvent? Q12. How do you justify that? (a) Boiling points of the solvents increase due to the presence of solutes. Ans. The temperature of a pure liquid at which its vapour pressure becomes equal to an external atmospheric pressure on its surface is called boiling point of the liquid. The addition of a non-volatile solute to a solvent always reduces its vapour pressure below that of the pure solvent. This is because solute particles occupy some of the surface area of the solution decreases the rate of evaporation and thus reduces its pressure. So, a higher temperature is needed to increase the vapour pressure to the point where the solution 9
10 boils. Hence, the boiling points of the solvents increase due to the presence of solutes. (b) Freezing points are depressed due to the presence of solutes. Ans. The temperature f a pure liquid at which its solid and liquid are froms coexist in equilibrium is called freezing point of the liquid. When a non-volatile solute is added to a solvent, it reduces its vapour pressure. If a solution is cooled sufficiently, the temperature at which crystals of pure solvent appear is the freezing point of the solution. At this temperature the solid solvent and solution are in equilibrium, so they must have the same vapour pressure. But, at a definite temperature, a solution containing a non-volatile solute has a lower vapour pressure than the pure solvent. Therefore, solid solvent must be in equilibrium with a solution at a lower temperature than the temperature that it would be in equilibrium with pure solvent. Hence, freezing points are depressed due to the presence of solutes. (c) The boiling point of one molal urea solution is o C but the boiling of two molal urea solution is less than o C. Ans. The boiling point of 1 molal urea solution is o C at 1 atm pressure rather than 100 o C. Thus the elevation of boiling point is ( ) =0.52 o C. The boiling point of 2 molal urea solution is o C, so the elevation of boiling points is ( )= 1.04 o C. Since the boiling point elevation depends upon the number of particles of solute, therefore, e molal urea solution which contains 2 x 6.02 x molecules has double the boiling point elevation than 1 molal urea solution which contains 6.02 x10 23 molecules. (d) Beckmann s thermometer is use to note the depression in freezing point. Ans. Beckmann s thermometer is used to read temperatures up to, 0.01 o C over a range of about 5 o C. Since, freezing point depressions are 10
11 small, no more than a degree or two. Therefore, to measure a small difference in temperature Beckmann s thermometer is used. It is more sensitive than ordinary thermometer because one degree is further divided into hundred divisions. (e) In summar the antifreeze solutions protect the radiator from boiling over. Ans. Water is used as a coolant in automobile radiation to decrease the temperature of the working engine. Pure water boils at 100 o C. It is observed that solutions boil at higher temperatures than do pure liquid. So, an aqueous solution of antifreeze such as ethylene glycol is used in place of pure water in radiators because it raises the boiling point of pure water. Hence, in summer the antifreeze solution protects the liquid of the radiator to boil over. (f) NaC1 and KNO 3 are used to lower the melting point of ice. Ans. It is a common observation that the freezing point of solution is always lower than the freezing point of the pure solvent. The lowering in freezing point depends upon the number of solute particles (molecules/ ions). A mixture of NaC1 and KNO 3 salts is used as a freezing mixture to lower melting points of ice. These salts dissociate in ice water. They split up into a number of ions each of which as a particle due to which the freezing point of water, i.e., the melting point of ice is lowered. Q13. What is Raoult s law? Give is three statements. How this law can help us to understand the ideality of a solution? Q14. Give graphical explanation for elevation of boiling point of a solution. Describe one method to determine the boiling pointy elevation of a solution. Q15. Freezing points of solutions are depressed when non-volatile solutes are present in volatile solvents. Justify it. Plot a graph to elaborate 11
12 your answer. Also give one method to record the depression of freezing point of a solution. Q16. Discuss the energetics of solution. Justify the heats of solutions as exothermic and endothermic properties. Q17. (a) Calculate the molarity of glucose solution when 9 g of it are dissolved in 250 cm 3 of solution. (a) Mass of glucose C 6 H 12 O 6 =9g Molar mass of C 6 H 12 O 6 =180g mol -1 Vol. of solution =250 cm 3 =0.25dm 3 Molarity =? Formula Used: Molarity= x Molarity = x Molarity =0.2 mol dm -3 Answer (b) Calculate the mass of urea in 100 g of H 2 O in 0.3 molal solutions. Molality=0.3 Mass of H 2 O =100 g =0.1 kg Mass of urea (solute) =? Molar mass of urea, NH 2 CONH 2 =60 g mol -1 Formula Used: Molarity= x 0.3 mol kg -1 = x Mass of urea = 0.3 mol kg -1 x 60 g mol -1 x 0.1 kg Mass of urea = 1.8 g Answer (c) Calculate the concentration of a solution in moles kg -1, which is obtained by mixing 250 g of 20% solution of NaC1 with 200 g of 40% solution of NaC1. First solution: 12
13 100 g of NaC1 solution contains pure NaC1 =20g 250 g of NaC1 solution contains pure NaC1 = x250 g =80g Second solution: 100 g of solution contains pure NaC1 =40g 200 g of NaC1 solution contains pure = x200 g =80g Total mass of solute NaC1 =( )g =130 g Total mass of NaC1 solution =( ) g =450 g Mass of solvent =( )g =320 g =0.32 kg Formula used: Molarity = x Molality = x Molality=6.94 mol kg -1 Answer Q18. (a) An aqueous solution of sucrose has been labeled as 1 molal. Find the mole fraction of the solute and the solvent. Molality =1 Mass of solute, C 12 H 22 O 11 =? Molar mass of C 12 H 22 O 11 =342 g mol -1 No. of kg of solvent =1 kg Formula used: Molarity = x Mass of solute, =molality x molar mass of solute x No. of Kg of solvent = 1 x 342 x 1 =342 g Now, No. of moles of sucrose= =1mol No. of moles of water = =55.56 mol Total no. of moles = = moles 13
14 Mole fraction of sucrose = =0.076 Answer Mole fraction of water = = Answer (b) Your are provide with 80% H 2 SO 4 having density 1.84 g cm-3. How much volume of this H 2 SO 4 sample is required to obtain one dm 3 of 20% H 2 SO 4 which has a density of 1.25 g cm -3. First solution: % of H 2 SO 4 =80 Density of H 2 SO 4 = 1.8 g cm -3 It means that: 1 cm 3 of H 2 SO 4 has mass =1.8 g 1000 cm 3 H 2 SO 4 has mass =1.8 x1000=1800g Now, 100g of H 2 SO 4 solution contains pure H 2 SO 4 =80 g 1800 g of H 2 SO 4 solution contains pure H 2 SO 4 = x 1800 =1440 g No. of moles of H 2 SO 4 = = =14.7 mol So, 14.7 moles of H 2 SO 4 are present in 100 cm 3 of concentrated H 2 SO 4 solution, therefore, the molarity of solution is Molarity of conc. H 2 SO 4 = 14.7 M Second solution: Percentage of dilute H 2 SO 4 solution =20% (w/w) Density of dilute H 2 SO 4 solution =1.25 g cm -3 It means that: 1 cm 3 of H 2 SO 4 has mass=1.25 g 1000 cm 3 of H 2 SO 4 has mass =1.25 x 1000 =1250 g Now, 100 g dilute H 2 SO 4 solution contains pure H 2 SO 4 =20g 1250 g of dilute H 2 SO 4 solution contains pure H 2 SO 4 = x1250 =250 g No. of moles of H 2 SO 4 = =2.55 mol So, 2.55 moles of H 2 SO 4 are present in 1000 cm 3 of dilute H 2 SO 4 solution, therefore the molarity of dilute H 2 SO 4 solution is 2.55 M. Now, volume of conc. H 2 SO 4 solution required to prepare dilute H 2 SO 4 solution can be calculated by using the dilution formula: 14
15 Conc. H 2 SO 4 dilute H 2 SO 4 M 1 V 1 = M 2 V xv 1 = 2.55 x 1000cm 3 V 1 V 1 = cm 3 =173.5 cm 3 Hence, volume of concentration H 2 SO 4 solution required to prepare dilute H 2 SO 4 Solution =175.5 cm 3 Answer Q cm 3 of 0.2 molar K 2 SO 4 solution is mixed with 250 cm 3 of 0.2 molar KC1 solution. Calculate the molar concentration of K + ions in the solution. K 2 SO 4 2K + + SO 0.2 M 2 x Molarity of K + ions=0.4m KC1 K + + C1 0.2 M 0.2M Molarity of K + ions =0.2M Total molarity of K + ions=( ) M=0.6M Total volume of solution =250 cm cm 3 =500cm 3 Since after mixing the two solutions, the total volume becomes 500 cm 3, so the concentration of K + ions becomes half. So, Molarity of K + ions = =0.3 M Answer Q20. 5 g of NaC1 are dissolved in 1000 g of water. The density of resulting solution is g cm -3. calculate molality, molarity and molefraction of this solution. Assume that the volume of the solution is equal to that of solvent. (i) Calculations for Molality Mass of solute, NaC1 =5g Molar mass of solute =58.5 g mol -1 15
16 Mass of solvent, H 2 O =1000g =1kg Molality=? Formula used: Molarity = x (ii) Molality = = mol kg -1 = m Answer Calculations for molarity: Mass of solute, NaC1 =5g Molar mass of solute =58.5 g mol -1 Mass of solvent, H 2 O =1000 g = 1kg Density of solution=0.997 g cm 3 Now, d or V= Vol. of solution = =1003 cm 3 Vol. of solution in dm 3 = =1.003 cm 3 Molarity = x = = mol dm -3 = M Answer (ii) Calculations for mole fraction: No. of moles of solute, NaC1 = = mol No. of moles of solvent H 2 O = = mol Total number of moles = =55.64 mol Mole fraction of NaC1, X NaC1 = = Answer Mole fraction of water, X H2O = =09984 Answer Q g of compound with empirical formula C 3 H 3 O were dissolved in g of pure benzene. The freezing point of solution was 16
17 found 1.02 o C less than that of pure benzene. The molal freezing point constant of benzene is 5.1 o C. calculate (i) the relative molar mass and (ii) the molecular formula of the compound. (i) Mass of solute=4.675 g Mass of solvent =212.5 g =5.1 o C K f T f Molar mass of solute =? Formula used: =1.02 o C Molar mass of solute = = x 1000 Molar mass of solute = = Molar mass of solute =110 g mol -1 Answer (ii) Empirical formula =C 3 H 3 O Empirical formula mass = =55 n = n = =2 Molecular formula =(Empirical formula) n =( C 3 H 3 O) 2 = C 3 H 3 O 2 Answer Q22. The boiling point of a solution containing 0.2 g of a substance A in 20.0 g of ether (molar mass =74) is 0.17 K higher than that of pure ether. Calculate the molar mass of A. Molal boiling point constant of ether is 2.16 K. Mass of A=0.2 g Mass of solvent =20 g T b =0.17 k K b =2.16K Molar mass of solute, A=? 17
18 Formula used: Molar mass of A x x1000. Molar mass of A = x x1000 Molar mass of A=127 g mol -1 Answer Q23. 3 g of a non-volatile, non-electrolyte solute X are dissolved in 50 g of ether (molar mass =74) at 293 K. The vapour pressure of ether falls from 442 torr to 426 torr under these conditions. Calculate. Calculate the molar mass of solute X. Mass of solute, X =3g Mass of solvent (ether) =50 g Molar mass of solvent (ether) =74 Vapour pressure of pure solvent, P o =442 torr Vapour pressure of solution, p =426 torr P=P o p = =16 torr Molar mass of solute, X =? Formula used: Molar mass of solute, X = x x Molar mass of solvent = = g mol -1 Answer 18
CHAPTER 9 SOLUTIONS SHORT QUESTIONS WITH ANSWER Q.1 Binary solution can be homogenous or heterogeneous explain? The solutions which contain two components only are called as binary solution. If binary
More informationIndian School Muscat
Indian School Muscat Chemistry Department Senior Section IIT JEE Solutions 1 What term is associated with the part of a solution that is present in the smallest amount? (A) ionic compound (B) solute (C)
More informationChapter 10: CHM 2045 (Dr. Capps)
Phase Diagram Phase diagrams for CO 2 and H 2 O Chapter 13. Solutions and Their Physical Properties Shows pressures and temperatures at which gaseous, liquid, and solid phases can exist. Allows us to predict
More informationSoluble: A solute that dissolves in a specific solvent. Insoluble: A solute that will not dissolve in a specific solvent. "Like Dissolves Like"
Solutions Homogeneous Mixtures Solutions: Mixtures that contain two or more substances called the solute and the solvent where the solute dissolves in the solvent so the solute and solvent are not distinguishable
More informationSubject : Chemistry Class : XII Chapter-2.Solutions Work Sheet ( WS 2. 1) Topic- 2.1 Henry s & Raoult s Laws
Work Sheet ( WS 2. 1) Topic- 2.1 Henry s & Raoult s Laws Name -. Class/ sec.. Roll No.. A. Fill in the blanks: 1. Solutions are mixtures of two or more than two components. 2. Generally, the component
More informationUnit - 2 SOLUTIONS VSA QUESTIONS (1 - MARK QUESTIONS) 1. Give an example of liquid in solid type solution.
Unit - 2 SOLUTIONS VSA QUESTIONS (1 - MARK QUESTIONS) 1. Give an example of liquid in solid type solution. 2. Which type of solid solution will result by mixing two solid components with large difference
More information11/4/2017. General Chemistry CHEM 101 (3+1+0) Dr. Mohamed El-Newehy. Chapter 4 Physical Properties of Solutions
General Chemistry CHEM 11 (3+1+) Dr. Mohamed El-Newehy http://fac.ksu.edu.sa/melnewehy Chapter 4 Physical Properties of Solutions 1 Types of Solutions A solution is a homogenous mixture of 2 or more substances.
More informationCH 2: SOLUTIONS
1 CH 2: SOLUTIONS 2 SOLUTION, SOLVENT, SOLUTE Solutions are homogeneous mixtures of two or more than two components. i.e. composition and properties are uniform throughout the mixture. Eg: The component
More informationChapter Solutions. MockTime.com. (a) M urea (b) 0.01 M KNO3 (c) 0.01 M Na2 SO4 (d) M glucose Ans: (c)
47 Chapter Solutions 1. Freezing point of an aqueous solution is ( 0.186) C. Elevation of boiling point of the same solution is K b = 0.512 C,Kf = 1.86 C, find the increase in boiling point. [2002] (a)
More informationRegents Chemistry Unit 3C Solutions Text Chapter 13 Reference Tables F, G & T. Chemists have Solutions!
Regents Chemistry Unit 3C Solutions Text Chapter 13 Reference Tables F, G & T Chemists have Solutions! SOLUTIONS homogeneous mixture (uniform composition throughout) Solute - substance being dissolved
More informationBushra Javed Valencia College CHM 1046 Chapter 12 - Solutions
Bushra Javed Valencia College CHM 1046 Chapter 12 - Solutions 1 Chapter 12 :Solutions Tentative Outline 1. Introduction to solutions. 2. Types of Solutions 3. Solubility and the Solution Process: Saturated,
More informationChapter 17: Phenomena
Chapter 17: Phenomena Phenomena: Different masses of solute were added to 1 kg of either H 2 O or C 6 H 6. The boiling and freezing points of the solutions were then measured. Examine the data to determine
More informationChapter 11. Properties of Solutions
Chapter 11 Properties of Solutions Section 11.1 Solution Composition Various Types of Solutions Copyright Cengage Learning. All rights reserved 2 Section 11.1 Solution Composition Solution Composition
More informationThey provide us with the knowledge of phase composition and phase stability as a function of temperature (T), pressure (P) and composition(c).
They provide us with the knowledge of phase composition and phase stability as a function of temperature (T), pressure (P) and composition(c). PHASE EQUILIBRIUM one of the most important sources of information
More informationChapter 12. Physical Properties of Solutions. Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill
Chemistry, Raymond Chang 10th edition, 2010 McGraw-Hill Chapter 12 Physical Properties of Solutions Ahmad Aqel Ifseisi Assistant Professor of Analytical Chemistry College of Science, Department of Chemistry
More informationSOLUTION CONCENTRATIONS
SOLUTION CONCENTRATIONS The amount of solute in a solution (concentration) is an important property of the solution. A dilute solution contains small quantities of solute relative to the solvent, while
More informationA) sublimation. B) liquefaction. C) evaporation. D) condensation. E) freezing. 11. Below is a phase diagram for a substance.
PX0411-1112 1. Which of the following statements concerning liquids is incorrect? A) The volume of a liquid changes very little with pressure. B) Liquids are relatively incompressible. C) Liquid molecules
More informationDownloaded from
: Bhubaneswar Region CHAPTER 2-SOLUTIONS 1 MARK QUESTIONS 1 What is molarity? 2 What do you understand by saying that molality of a solution is 0.2? 3 Why is the vapour pressure of a liquid remains constant
More informationSolutions and Their Properties
Chapter 11 Solutions and Their Properties Solutions: Definitions A solution is a homogeneous mixture. A solution is composed of a solute dissolved in a solvent. When two compounds make a solution, the
More informationPSI AP Chemistry: Solutions Practice Problems
PSI AP Chemistry: Solutions Practice Problems Name Solutions: Mixtures, Solubility and Concentration Classwork 1. A student determined that there were 0.032 grams of oxygen gas dissolved in a 200.0 ml
More informationDATE: POGIL: Colligative Properties Part 1
NAME: AP Chemistry DATE: POGIL: Colligative Properties Part 1 Why? There is a general misconception that adding sodium chloride to cooking water for pasta increases the temperature of the boiling water
More informationChapter 12: Solutions. Mrs. Brayfield
Chapter 12: Solutions Mrs. Brayfield 12.1: Solutions Solution a homogeneous mixture of two or more substances Solvent the majority component Solute the minority component What is the solute and solvent
More informationAP Chemistry--Chapter 11: Properties of Solutions
AP Chemistry--Chapter 11: Properties of Solutions I. Solution Composition (ways of expressing concentration) 1. Qualitatively, use dilute or concentrated to describe 2. Quantitatively a. Mass Percentage
More information1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic.
Problems - Chapter 13 (with solutions) 1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic. a) solution - A homogeneous
More informationSolutions. Chapter 14 Solutions. Ion-Ion Forces (Ionic Bonding) Attraction Between Ions and Permanent Dipoles. Covalent Bonding Forces
Solutions Chapter 14 1 Brief Review of Major Topics in Chapter 13, Intermolecular forces Ion-Ion Forces (Ionic Bonding) 2 Na + Cl - in salt These are the strongest forces. Lead to solids with high melting
More informationColligative Properties
Colligative Properties! Consider three beakers: " 50.0 g of ice " 50.0 g of ice + 0.15 moles NaCl " 50.0 g of ice + 0.15 moles sugar (sucrose)! What will the freezing temperature of each beaker be? " Beaker
More informationLESSON 11. Glossary: Solutions. Boiling-point elevation
LESSON 11 Glossary: Solutions Boiling-point elevation Colligative properties Freezing-point depression Molality Molarity (M) Mole (mol) Mole fraction Saturated solution a colligative property of a solution
More informationPhysical Properties of Solutions
Physical Properties of Solutions Chapter 12 Copyright The McGraw-Hill Companies, Inc. Permission required for reproduction or display. 12.1- Types of solutions A solution is a homogenous mixture of 2 or
More information2 Copyright Pearson Education, Inc., or its affiliates. All Rights Reserved.
16.3 Colligative of Solutions > 16.3 Colligative of Solutions > CHEMISTRY & YOU Chapter 16 Solutions 16.1 of Solutions 16.2 Concentrations of Solutions 16.3 Colligative of Solutions 16.4 Calculations Involving
More informationChapter 13. Characteristics of a Solution. Example of A Homogenous Mixtures. Solutions
Chapter 13 Solutions Characteristics of a Solution A solution is a homogeneous mixture A solution is composed of a: Solute: the substance in lesser amount Solvent: the substance in greater amount Two liquid
More informationOverview. Types of Solutions. Intermolecular forces in solution. Concentration terms. Colligative properties. Osmotic Pressure 2 / 46
1 / 46 2 / 46 Overview Types of Solutions. Intermolecular forces in solution Concentration terms Colligative properties Osmotic Pressure 3 / 46 Solutions and Colloids A solution is a homogeneous mixture
More informationName Date Class PROPERTIES OF SOLUTIONS
16.1 PROPERTIES OF SOLUTIONS Section Review Objectives Identify the factors that determine the rate at which a solute dissolves Identify the units usually used to express the solubility of a solute Calculate
More informationPHYSICAL PROPERTIES OF SOLUTIONS
PHYSICAL PROPERTIES OF SOLUTIONS Do all the exercises in your study guide. PHYSICAL PROPERTIES OF SOLUTIONS A solution is a homogeneous mixture of a solute and a solvent. A solvent is a substance that
More informationProperties of Solutions. Chapter 13
Properties of Solutions Chapter 13 Sodium acetate crystals rapidly form when a seed crystal is added to a supersaturated solution of sodium acetate. Saturated solution: contains the maximum amount of a
More informationChemistry. TOPIC : Solution and colligative properties
TOPIC : Solution and colligative properties Date : Marks : 20 mks Time : ½ hr. If 5.85 g of NaCl (molecular weight 58.5) is dissolved in water and the solution is made up to 0.5 litre, the molarity of
More informationSolutions: Multiple Choice Review PSI AP Chemistry. 1. Which of the following would be FALSE regarding mixtures?
Solutions: Multiple Choice Review PSI AP Chemistry Name Part A: Mixtures, Solubility, and Concentration 1. Which of the following would be FALSE regarding mixtures? (A) Mixtures do not obey the law of
More informationChapter 13. Ions in aqueous Solutions And Colligative Properties
Chapter 13 Ions in aqueous Solutions And Colligative Properties Compounds in Aqueous Solution Dissociation The separation of ions that occurs when an ionic compound dissolves H2O NaCl (s) Na+ (aq) + Cl-
More informationSolutions. Solution Formation - Types of Solutions - Solubility and the Solution Process - Effects of Temperature and Pressure on Solubility
Solutions Solutions Solution Formation - Types of Solutions - Solubility and the Solution Process - Effects of Temperature and Pressure on Solubility Colligative Properties - Ways of Expressing Concentration
More informationCOLLIGATIVE PROPERTIES OF SOLUTIONS
NAME: UNIT #9: MOLARITY DILUTIONS SOLUBILITY CURVES COLLIGATIVE PROPERTIES OF SOLUTIONS 1. MOLARITY a) Molarity is a measurement of the concentration of a solution in Chemistry. b) When making solutions,
More information1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic.
Problems - Chapter 13 (with solutions) 1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic. a) solution - A homogeneous
More informationColligative Properties
Colligative Properties Vapor pressures have been defined as the pressure over a liquid in dynamic equilibrium between the liquid and gas phase in a closed system. The vapor pressure of a solution is different
More information1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic.
Problems - Chapter 13 (with solutions) 1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic. a) solution - A homogeneous
More informationLecture Presentation. Chapter 12. Solutions. Sherril Soman, Grand Valley State University Pearson Education, Inc.
Lecture Presentation Chapter 12 Solutions Sherril Soman, Grand Valley State University Thirsty Seawater Drinking seawater can cause dehydration. Seawater Is a homogeneous mixture of salts with water Contains
More informationChem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.
Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. An open-tube manometer is used to measure the pressure in a flask. The atmospheric
More information1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic.
Problems - Chapter 13 (with solutions) 1) Define the following terms: a) solution, b) miscible, c) hydration, d) percent by mass (solute), e) colligative property, f) hypotonic. a) solution - A homogeneous
More informationChapter 11. General Chemistry. Chapter 11/1
Chapter 11 Solutions and Their Properties Professor Sam Sawan General Chemistry 84.122 Chapter 11/1 Solutions Solution: A homogeneous mixture. Solvent: The major component. Solute: A minor component. Copyright
More informationColligative Properties
Slide 1 Colligative Properties Practical uses of solutions Slide 2 Units of Concentration Whatever units you use, the goal is the same: specify the quantity of 1 component (the solute s ) relative to the
More informationSolution KEY CONCEPTS
Solution KEY CONCEPTS Solution is the homogeneous mixture of two or more substances in which the components are uniformly distributed into each other. The substances which make the solution are called
More informationSolutions Definition and Characteristics
Solutions Solutions Definition and Characteristics Homogeneous mixtures of two or more substances Appear to be pure substances Transparency Separation by filtration is not possible Uniform distribution
More informationPSI AP Chemistry Solutions Practice Problems
PSI AP Chemistry Solutions Practice Problems Name Solutions: Mixtures, Solubility and Concentration Classwork 1. A student determined that there were 0.032 grams of oxygen gas dissolved in a 200.0 ml sample
More informationPhysical Pharmacy. Solutions. Khalid T Maaroof MSc. Pharmaceutical sciences School of pharmacy Pharmaceutics department
Physical Pharmacy Solutions Khalid T Maaroof MSc. Pharmaceutical sciences School of pharmacy Pharmaceutics department 10/31/2015 Online access: bit.ly/physicalpharmacy 1 Mixtures a combination of two or
More informationChapter 12.4 Colligative Properties of Solutions Objectives List and define the colligative properties of solutions. Relate the values of colligative
Chapter 12.4 Colligative Properties of Solutions Objectives List and define the colligative properties of solutions. Relate the values of colligative properties to the concentrations of solutions. Calculate
More informationChapter 11 Problems: 11, 15, 18, 20-23, 30, 32-35, 39, 41, 43, 45, 47, 49-51, 53, 55-57, 59-61, 63, 65, 67, 70, 71, 74, 75, 78, 81, 85, 86, 93
Chapter 11 Problems: 11, 15, 18, 20-23, 30, 32-35, 39, 41, 43, 45, 47, 49-51, 53, 55-57, 59-61, 63, 65, 67, 70, 71, 74, 75, 78, 81, 85, 86, 93 Chapter 11 Properties of Solutions Types of mixtures: homogenous
More informationProperties of Solutions. Overview of factors affecting solubility Ways of expressing concentration Physical properties of solutions
Properties of Solutions Overview of factors affecting solubility Ways of expressing concentration Physical properties of solutions Learning objectives Define terms solute, solvent and solution Distinguish
More informationSolutions: Physical Properties and Behavior
Solutions: Physical Properties and Behavior In the previous chapter you were exposed to a great deal of information about the forces present in and the properties of individual pure substances (for example,
More informationChapter 13. Properties of Solutions
Chapter 13 Properties of Solutions Warm - Up Why doesn t salt dissolve in nonpolar solvents such as hexane? How does the orientation of water around Na + differ from the orientation of water around Cl
More informationPHASE CHEMISTRY AND COLLIGATIVE PROPERTIES
PHASE CHEMISTRY AND COLLIGATIVE PROPERTIES Phase Diagrams Solutions Solution Concentrations Colligative Properties Brown et al., Chapter 10, 385 394, Chapter 11, 423-437 CHEM120 Lecture Series Two : 2013/01
More information- Applications: In chemistry, this effect is often used to determine the molecular weight of an unknown molecule.
73 FREEZING POINT DEPRESSION concentration of solute (molality) Freezing point depression constant (for SOLVENT) Freezing point depression: The amount the freezing temperature is LOWERED by the solute.
More informationChapter 13 Properties of Solutions
Chapter 13 Properties of Solutions Learning goals and key skills: Describe how enthalpy and entropy changes affect solution formation. Describe the relationship between intermolecular forces and solubility,
More informationAIIMS,CBSE,AIPMT, & PMT,
1 Which of the following solutions has the highest boiling point? (a) 5.85% solution of NaCl (b) 18.0% solution of glucose (c) 6.0% solution of urea (d) all have same boiling point 2 Two solutions of NaCl
More informationThe Water Molecule. Draw the Lewis structure. H O H. Covalent bonding. Bent shape
Water & Solutions 1 The Water Molecule Draw the Lewis structure. H O H Covalent bonding. Bent shape 2 Water What determines whether a molecule is polar? Is water a polar molecule? d- d+ d+ 1. Oxygen is
More informationx =!b ± b2! 4ac 2a moles particles solution (expt) moles solute dissolved (calculated conc ) i =
Properties of Solution Practice Exam Solutions Name (last) (First) Read all questions before you start. Show all work and explain your answers. Report all numerical answers to the proper number of sig.
More informationSolutions: Formation and Properties
New Jersey Center for Teaching and Learning Slide 1 / 48 Progressive Science Initiative This material is made freely available at www.njctl.org and is intended for the non-commercial use of students and
More information- Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)
68 HOW THINGS DISSOLVE - Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)... what happens? - Water molecules pull the sugar molecules out of
More informationBig Idea Three Topics
Big Idea Three Topics 1. Molecular, Ionic, Net Ionic Equations 2. Stoichiometry 3. Synthesis, Decomposition Reactions 6. Chemical Change Evidence 7. Endothermic & Exothermic Reactions 8. Electrochemistry
More informationChapter 11 Solutions and Colloids 645
Chapter 11 Solutions and Colloids 645 11.5 Colloids Colloids are mixtures in which one or more substances are dispersed as relatively large solid particles or liquid droplets throughout a solid, liquid,
More informationClass XII Chapter 2 Solutions Chemistry
Class XII Chapter 2 Solutions Chemistry Question 2.1: Calculate the mass percentage of benzene (C 6 H 6 ) and carbon tetrachloride (CCl 4 ) if 22 g of benzene is dissolved in 122 g of carbon tetrachloride.
More informationALE 24. Colligative Properties (Part 2)
Name Chem 162, Section: Group Number: ALE 24. Colligative Properties (Part 2) (Reference: 13.6 Silberberg 5 th edition) Why is calcium chloride spread on highways in the North during the Winter? The Model:
More informationCHM Colligative properties (r15) Charles Taylor 1/6
CHM 111 - Colligative properties (r15) - 2015 Charles Taylor 1/6 Introduction We will now discuss the unique properties of solutions. As you might imagine, a mixture of substances might share some of the
More informationChem 1100 Pre-Test 3. Multiple Choice Identify the choice that best completes the statement or answers the question.
Chem 1100 Pre-Test 3 Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Determine the oxidation number of the underlined element in K 2CO 3. a. 1 b. 2 c.
More informationPX-III Chem 1411 Chaps 11 & 12 Ebbing
PX-III Chem 1411 Chaps 11 & 12 Ebbing 1. What is the name for the following phase change? I 2 (s) I 2 (g) A) melting B) condensation C) sublimation D) freezing E) vaporization 2. Which of the following
More informationChapter 11: Properties of Solutions - Their Concentrations and Colligative Properties. Chapter Outline
Chapter 11: Properties of Solutions - Their Concentrations and Colligative Properties Chapter Outline 11.1 Energy Changes when Substances Dissolve 11.2 Vapor Pressure 11.3 Mixtures of Volatile Substances
More information- Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)
68 HOW THINGS DISSOLVE - Let's look at how things dissolve into water, since aqueous solutions are quite common. sucrose (table sugar)... what happens? - Water molecules pull the sugar molecules out of
More informationDATA THAT YOU MAY USE UNITS Conventional Volume ml or cm 3 = cm 3 or 10-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr = Pa CONSTANTS
DATA THAT YOU MAY USE UNITS Conventional S.I. Volume ml or cm 3 = cm 3 or 0-3 dm 3 Liter (L) = dm 3 Pressure atm = 760 torr =.03 0 5 Pa torr = 33.3 Pa Temperature C 0 C = 73.5 K PV L-atm =.03 0 5 dm 3
More informationLiquid in liquid: ethanol in water. Solid in liquid: any salt in water. Solid in solid: brass, bronze, and all alloys
1 of 6 I. The solution process Solutions, colloids, and suspensions Solution: homogeneous mixture, equally dispersed at the molecular level, uniform throughout in its physical and chemical properties Colloid:
More information3 BaCl + 2 Na PO Ba PO + 6 NaCl
Q. No. 1 In which mode of expression, the concentration of solution remains independent of temperature? Molarity Normality Formality Molality Explanation Molality because molality involves mass which is
More informationWater & Solutions Chapter 17 & 18 Assignment & Problem Set
Water & Solutions Chapter 17 & 18 Assignment & Problem Set Name Warm-Ups (Show your work for credit) Date 1. Date 2. Date 3. Date 4. Date 5. Date 6. Date 7. Date 8. Water & Solutions 2 Vocabulary (know
More informationSOLUTIONS. (i) Mass Percentage(w/w): Amount of solute present in grams dissolved per 100g of solution.
SOLUTIONS Section A : LEARNING POINTS: Units of concentration of Solution : (i) Mass Percentage(w/w): Amount of solute present in grams dissolved per 100g of solution. Ex : 10% (w/w) glucose in water by
More informationSOLUTIONS. Chapter Test B. A. Matching. Column A. Column B. Name Date Class. 418 Core Teaching Resources
16 SOLUTIONS Chapter Test B A. Matching Match each term in Column B to the correct description in Column A. Write the letter of the correct term on the line. Column A Column B 1. the number of moles of
More informationChapter 11 Review Packet
Chapter 11 Review Packet Name Multiple Choice Portion: 1. Which of the following terms is not a quantitative description of a solution? a. molarity b. molality c. mole fraction d. supersaturation 2. Which
More informationCOLLIGATIVE PROPERTIES. Engr. Yvonne Ligaya F. Musico 1
COLLIGATIVE PROPERTIES Engr. Yvonne Ligaya F. Musico 1 Colligative Properties Properties that depend on the collective effect of the number of solute particles. Engr. Yvonne Ligaya F. Musico 2 COLLEGATIVE
More informationLecture outline: Chapter 13
Lecture outline: Chapter 13 Properties of solutions Why solutions form at the molecular l levell Units of solution concentration Colligative properties: effects of solutes on BP, MP, and vapor pressure
More informationColligative Properties
Colligative Properties Some physical properties of solutions differ in important ways from those of the pure solvent. For example, pure water freezes at 0 C, but aqueous solutions freeze at lower temperatures.
More informationColligative Properties
Slide 1 Colligative Properties Practical uses of solutions Slide 2 Solution homogeneous mixtures composition may vary from one sample to another appears to be one substance, though really contains multiple
More informationSolutions. Definitions. Some Definitions. Page 1. Parts of a Solution
Chapter 15 s 1 Definitions 4 Why does a raw egg swell or shrink when placed in different solutions? s can be classified as saturated or unsaturated. A saturated solution contains the maximum quantity of
More informationPhysical Properties of Solutions
Physical Properties of Solutions Physical Properties of Solutions Types of Solutions (13.1) A Molecular View of the Solution Process (13.2) Concentration Units (13.3) Effect of Temperature on Solubility
More informationChapter 11 Properties of Solutions
Chapter 11 Properties of Solutions Solutions Homogeneous mixtures of two or more substances Composition is uniform throughout the sample No chemical reaction between the components of the mixture Solvents
More informationUNIT 2 SOLUTION. Q. 1. The vapour pressure of deliquescent substance is less or more than that of water vapours in air?
UNIT 2 SOLUTION 1 MARK QUESTIONS Q. 1. The vapour pressure of deliquescent substance is less or more than that of water vapours in air? Ans. Less than that of water vapours in air. Q. 2. If is the degree
More informationChapter 11: Properties of Solutions - Their Concentrations and Colligative Properties. Chapter Outline
Chapter 11: Properties of Solutions - Their Concentrations and Colligative Properties Chapter Outline 11.1 Energy Changes when Substances Dissolve 11.2 Vapor Pressure 11.3 Mixtures of Volatile Substances
More information70 Example: If a solution is m citric acid, what is the molar concentration (M) of the solution? The density of the solution is 1.
70 Example: If a solution is 0.688 m citric acid, what is the molar concentration (M) of the solution? The density of the solution is 1.049 g/ml molality definition molarity definition To solve the problem,
More informationHEMISTRY 110 EXAM 3 April 6, 2011 FORM A When the path is blocked, back up and see more of the way. 1. A 250 L vessel is evacuated and then connected to a 50.0 L bulb with compressed nitrogen. The pressure
More informationBorn-Haber Cycle: ΔH hydration
Born-Haber Cycle: ΔH hydration ΔH solution,nacl = ΔH hydration,nacl(aq) U NaCl ΔH hydration,nacl(aq) = ΔH hydration,na + (g) + ΔH hydration,cl (g) Enthalpies of Hydration 1 Sample Exercise 11.3 Use the
More information(B) Which of the following in each pair will be more soluble in water?
CHM 112 Chapter 11 Solutions: Study Guide Purpose: This is a guide for your as you work through the chapter. The major topics are provided so that you can write notes on each topic and work the corresponding
More informationColligative Properties. Vapour pressure Boiling point Freezing point Osmotic pressure
Colligative Properties Vapour pressure Boiling point Freezing point Osmotic pressure Learning objectives Describe meaning of colligative property Use Raoult s law to determine vapor pressure of solutions
More information1. Which substance will conduct the current in the solid state? 1. Diamond 2.Graphite 3.Iodine 4.Sodium chloride.
CHAPTER :SOLIDS 1. Which substance will conduct the current in the solid state? 1. Diamond 2.Graphite 3.Iodine 4.Sodium chloride. 2. Molten sodium chloride conducts electricity due to the presence of ions:
More informationStudyHub: AP Chemistry
StudyHub+ 1 StudyHub: AP Chemistry Solution Composition and Energies, Boiling Point, Freezing Point, and Vapor Pressure StudyHub+ 2 Solution Composition: Mole Fraction: Formula: Mole Fraction of Component
More informationProperties of Solutions
Properties of Solutions The Solution Process A solution is a homogeneous mixture of solute and solvent. Solutions may be gases, liquids, or solids. Each substance present is a component of the solution.
More informationAn aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is g/ml Find: molality, mole fraction, molarity.
66 An aqueous solution is 8.50% ammonium chloride by mass. The density of the solution is 1.024 g/ml Find: molality, mole fraction, molarity. Find molality: mass percent molality Assuming 100 g solution,
More informationCHAPTER 7: Solutions & Colloids 7.2 SOLUBILITY. Degrees of Solution. Page PHYSICAL STATES of SOLUTIONS SOLUTION
CHAPTER 7: Solutions & Colloids Predict the relative solubility of materials on the basis of polarity Describe solution formation in terms of solutesolvent interactions Calculate solution concentrations
More informationChapter 11. Properties of Solutions. Copyright 2017 Cengage Learning. All Rights Reserved.
Chapter 11 Properties of Solutions Chapter 11 Table of Contents (11.1) (11.2) (11.3) (11.4) (11.5) (11.6) (11.7) (11.8) Solution composition The energies of solution formation Factors affecting solubility
More information