Physical Chemistry CHM101 Past Questions PDF 2020/2021

SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) PHYSCICAL CHEMISTRY CHM101 SOLVE EASY ACADEMY INNOCENT JEREMIAH.T SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 2020/2021 Exam Que...

SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) PHYSCICAL CHEMISTRY CHM101 SOLVE EASY ACADEMY INNOCENT JEREMIAH.T SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 2020/2021 Exam Questions 1. If the volume of gas molecules is constant, the relationship between the pressure and the absolute Temperature will be (A) constant (B) inversely proportional (C) directly proportional (D) no relationship (E) normal 2. What are standard temperature and pressure conditions? (A) 0 K and 760 mm of Hg (B) 0°C and 760 mm of Hg (C) 0°C and 1 mm of Hg. (D) All of the above (E) None of the above 3. What is the relationship between temperature and volume if pressure is constant? (A) constant (B) inversely proportional (C) directly proportional (D) no relationship (E) Normal 4. According to kinetic theory of gasses at absolute zero temperature (A) Water freezes, (B) Liquid molecules are converted to gases, (C) Molecules motion stops, (D) Gas molecules Liquefies (E) All of the above 5. The increase in the volume of gas particles will...... (A) Increase their KE and absolute temperature, (B) Decrease their KE and their pressure, (C) Decrease their KE and increase pressure, (D) Decrease their KE and increase temperature, (E) Increase their KE and decrease temperature 6. Covert 327 °C to Kelvin temperature. (A) 600K (B) 607 K, (C) 527K (D) 327K (E) 273.15K 7. In a mixture of gasses, gas A has mole fraction of 0.341, if the total pressure of the gaseous mixture is 5.2 atmosphere, what will be the partial pressure of gas A? (A) 17.52 (B) 17.13 (C) 0.066 (D) 3.10 (E) 17.73 8. 150 𝑐𝑚 3 of a gas has pressure of 25 atmosphere. What will be its volume if the pressure is increase to 75 atmospheres assuming there is no change in temperature? (A) 40 cm³ (B) 50 cm³ (C) 55 cm³ (D) 450 cm³ (E) 460 cm³ 9. Which of the gases possesses maximum r.m.s. speed if all are kept at the same temperature?(A) Oxygen, (B) Nitrogen, (C) Hydrogen, (D) Carbon dioxide (E) carbon monoxide 10.1.5 moles of an ideal gas has a temperature of -15°C and a pressure of 2 atm. What volume in 𝑑𝑚 3will the gas occupy at that temperature? (R=0.082 𝑎𝑡𝑚 𝑑𝑚 3𝐾 −1 𝑀𝑜𝑙−1 ) (A) 15.87 dm³, (B) 0.9 dm³ (C) 15.02 dm³ (D) 1.5 dm³ (E) 32.02 dm³ SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 11.Which of the following gases will deviate positively from ideality at all conditions of temperature and pressure? (A) Nitrogen (B) helium (C) hydrogen (D) carbon dioxide (E) oxygen 12.A real gas deviates from ideal gas under conditions of...(A) high P and low T, (B) low P and high T, (C) low P and T, (D) high P and T 13. A molecule of mass m moving with a velocity v makes 5 elastic collisions with a wall of the container per second. The change in its momentum per second will be...(A) mv (B) 5 mv (C) mv/10(D) 10 mv (E) 25 mv 14.𝑃𝑉/2 = 𝑅𝑇, 𝑃 represents the pressure of (A) Any amount of gas (B) 2 moles of gas (C) 3 moles of gas (D) 4 moles of gas (E) 6 moles of gas 15. 280 cm³ of a gas X diffuses in 40 seconds what will be the rate of diffusion of gas X.(A) 7.0 𝑐𝑚 3 𝑠𝑒𝑐 −1 (B) 3.0 𝑐𝑚 3 𝑠𝑒𝑐 −1 (C) 7.9 𝑐𝑚 3 𝑠𝑒𝑐 −1 (D) 3.5 𝑐𝑚 3 𝑠𝑒𝑐 −1 (E) 7.68 𝑐𝑚 3𝑠𝑒𝑐 −1 -1 16.At standard temperature and pressure, one mole of a gas occupies a volume of 22.415 dm³ exert a pressure of one atmosphere at 0°C. Calculate the molar gas constant R (A) 0.08206 𝑎𝑡𝑚 𝑑𝑚3 𝐾 −1 𝑀𝑜𝑙−1 (B) 0.008206 𝑎𝑡𝑚 𝑑𝑚3 𝐾 −1 𝑀𝑜𝑙−1 (C) 0.8206 𝑎𝑡𝑚 𝑑𝑚3 𝐾 −1 𝑀𝑜𝑙−1 (D) 8.0206 𝑎𝑡𝑚 𝑑𝑚3 𝐾 −1 𝑀𝑜𝑙−1 (E) 0.18206 𝑎𝑡𝑚 𝑑𝑚3 𝐾 −1 𝑀𝑜𝑙−1 17. An ideal gas differs from a real gas in that the molecules of an ideal gas.. (A) Have no kinetic energy, (B) have a molecular weight of zero (C) have appreciable molecular volumes (D) have no attraction for one another (E) have an average molecular mass 18.Which among the following statements is correct about the molar gas volume? For n number of molecule (A) 𝑉 = 𝑛𝑉𝑚 (B) 𝑉 = 𝐾𝑇, (C) 𝑉𝑚 = 𝑛 𝑛𝑘𝑇 (D) 𝑉𝑚 = , (E) 𝑉𝑚 = 𝑛/𝑝𝑇 𝑘𝑇 19.At low temperature, real gases show...... deviation from ideality, (A) positive (B) negative (C) no (D) constant (E) none of. the above 20.One of the factors responsible for the difference between ideal and real gases is..... (A) Pressure, (B) Absolute Temperature (C) Van Der Waal forces (D) root mean square speed, of the gas (E) Average kinetic energy of the gas. 21.Which of these is not an example of a physical change? (A) Crystallization (B) Melting (C) Condensation (D) Neutralization (E) Vapourization SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 22.Given that C (graphite) → C (Diamond), ∆𝐻𝑜 = 1.89𝑘𝐽. the heat absorbed in the process is called the heat of (A) Atomization (B) Allotropic (C) Transition (D) Dissociation (E) Fission 23.The quantity of heat qp, absorbed when the temperature of a system is increased at constant temperature is dependent on which of the following parameters (A) Heat capacity (B) Heat of atomization (C) Heat of dilution (D) Heat of transition (E)Weight of the system 24.If the molar heat of combustion of liquid benzene at constant volume and 300K is 3272 kJ, what will be the heat of combustion at constant pressure at the same temperature? (A) 7203 kJ (B)-4562 kJ (C)-3270 kJ (D) 4823 kJ (E)-7203 Kj 25. Equation in which values of beat changes are called (A) Enthalpy equations (B) Entropy equations (C) Physicochemical equations (D) Thermo chemical equations (E) Latent heat equations 26. Consider the equation' C+ 𝑂2 → 𝐶𝑂2 ∆𝐻 = −393.513 KJ The reaction is said to be (A) Endothermic (B) Exothermic (C) Thermo-chemical (D) Molar enthalpy (E) None of the above 27.Physicochemical changes accompanied by absorption of heat are referred to as (A) Endothermic (B) Exothermic(C) Thermometry (D) Thermodynamics (E) Latent 28.Given that the standard molar heat of combustion of propane is -526.3 kcal. Mol-1, what is its calorific value? (C=12, H=1) (A) 55.82 kcal.𝑔 −1(B) 11.96 kcal.𝑔−1(C) 13.25 kcal.𝑔−1 (D) 17.52 kcal.𝑔−1(E) 20.33 kcal.𝑔 −1 29. What is the heat of reaction between F𝑒2 𝑂3 and C𝑂2 , given the following heat of formation F𝑒2 𝑂3 (-838.52KJ), CO (-110.53KJ) and CO₂ (-393.5 KJ) (A) ∆𝐻 = −18.42 𝐾𝐽 (B) ∆𝐻 =14.32 KJ (C) 18.64 KJ (D)-25.63 KJ (E)-13.67 KJ 30.The determination of the heat of reaction is carried out in an instrument called (A) Desiccator (B) furnace (C) Bomb Calorimeter (D) oven (E) water bath 31.The quantity of heat which must be applied to decompose a compound into it element is equal to the heat evolved when the compound is formed from its element is called the law of (A) Lavoisier and Laplace (B) Hess (C)Avogadro (D) Charles(E) Dalton 32.Which of these is a chemical change? (A) Crystallization (B) Condensation (C) Vapourization (D) Combustion (E) Melting SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 33.The enthalpy change when one mole of a solute is added to such a large amount of solution that the concentration of the solution remains unchanged is called (A) Heat of dilution (B) Heat of atomization (C) Heat of solution (D) Differential heat of solution (E) Heat of combustion 34.What is the C-H bond energy given the heat of formation of CH4 (-74.85 KJ), heat of dissociation of H2 (430.95 KJ) and the heat of sublimation of graphite C (s) (711.28 KJ) (A) ∆𝐻 =1648.0 KJ (B) 1567.3 KJ (C) 4245.6 KJ (D) 1432.5 KJ (E) 3267.2 KJ 35.Which of these is correct unit of rate of reaction? (a) M𝑠 −1 (b) Ms(c) 𝑀−1 𝑠 −1 (c) 𝑀−1s (d) mol 𝑠 −1 (e) 𝑚𝑜𝑙−1 s 36.Change in [CO] is 0.05 M in a given reaction after a period of 60 sec. Determine the average rate for CO in the reaction. Assume the values are given in appropriate rate unit. (a) 7.3 × 10−4(b) 8.3 × 10−4 (c) 8.9 × 10−4 (c) 8.3 × 10−5 (d) 8.3 × 10−6 (e) 3.3× 10−4 37. A catalyst may facilitate the rate of reaction by lowering the reaction's_____ (a) Kinetic energy(b) Potential energy (c) Internal Energy (d) Electrical energy (e) Activation energy 38.In the expression, Rate = k[A]𝑛 , n represent ________(a) Law (b) rate law (c) rate constant (d) order (c) all of the above 39.k in the above expression (i.e. in the question above) stands for.____(a) Law (b) rate law (c) rate constant (d) order (e) power 40.An acid-base conjugate pair are any two substances which differ in chemical composition by a _ (a) Sodium (b) Calcium (c) Proton (d) Chlorine (e) Neon 41.Given the expression; Rate = k[A][B]; the overall order of the reaction is? (a) 0 (b) 1 (c) 0.5 (d) 3(e) 2 42.One of these is an example of reference electrode. (a)Standard Sodium Electrode (b) Standard Potassium Electrode (c) Standard Hydrogen Electrode (d) Standard Calcium Electrode (e) All of the above 43. Which of these equations represent the dissolution of C𝐻3 COONa in water? (a) C𝐻3 COONa+ H₂O → N𝑎 + +CH,COOH (b) C𝐻3 COONa+ H₂O →Na + C𝐻3 COOH + OH (c) C𝐻3 COONa+ H₂O →N𝑎 ++ OH (d) C𝐻3 COONa+ H₂O→C𝐻3 COOH + OH (e) All of the above 44. The reaction of ion and water is referred to as (a) Solvolysis (b) Acidification (c) Hydropholysis (d) hydrolysis (e) All of them 45.When an element undergoes oxidation, the oxidation number______(a) Decrease (b) Constant (c) Increases(d) All of them (e) None of them SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 46.An element undergoing reduction shows, in the oxidation number (a) Decrease (b) Increases (c) Constant (d) All of them (e) None of them 47.Methods of balancing redox reactions include the following _______(a) Oxidation number method (b) Half reaction method (c) a, b, d & e (d) Algebraic method (e) Redox reactions in alkaline solutions method 48.Buffer Solutions show resistance to changes in ______ when small amount of acids and bases are added (a) [H](b) pH(c) [OH] (d) [OH] (e) None of the above 49._________are substances which in solution or molten state can conduct electricity and are decomposed in the process. (a) ions (b) cations (e) electrolytes (d) anions (e) all of the above 50.A good example of Lewis acid is(a) AIC𝑙4 (b) AIC𝑙3 (c) NaCl (d) CaC𝑙2 (e) NaF 51.Which of these expressions is correct; (a) pOH = -log [OH] (b) pOH = log[OH] (c) pOH = log [OH] (d) pOH =-log [O] (e)pOH = -log [H-] 52. The larger the dissociation constant of an acid the________ is the acid (a) Weaker (b) Neutral (c) a & b(d) Stronger (e) All of the above 53. Calculate the pH of 0.03 M sulphuric acid (a)13.78 (b) 10.78 (c)1.22 (d) 9.78 (e) 8.78 54. Hence the pOH of the sulphuric acid in the above question is ______(a) 12.68 (b) 12.57 (c) 12.47 (d) 12.78 (e) 12.11 SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 2020/2021 ANSWERS 1. If the volume of gas molecules is constant, the relationship between the pressure and the absolute temperature will be (C) directly proportional. This is based on Gay-Lussac's law, which states that the pressure of a gas is directly proportional to its absolute temperature when the volume is held constant. 2. Standard temperature and pressure conditions are (B) 0°C and 760 mm of Hg. This is defined as Standard Temperature and Pressure (STP). 3. The relationship between temperature and volume if pressure is constant is (C) directly proportional. This is described by Charles's law, which states that the volume of a gas is directly proportional to its absolute temperature when the pressure is constant. 4. According to the kinetic theory of gases at absolute zero temperature (C) molecules' motion stops. At absolute zero (0 K), the kinetic energy of molecules would theoretically be zero, and molecular motion stops. 5. The increase in the volume of gas particles will (B) decrease their KE and their pressure. According to the ideal gas law, if the volume increases while the number of particles and temperature remain constant, the pressure will decrease, 6. To convert 327 °𝐶 to Kelvin temperature, add 273.15 to the Celsius temperature: 327 + 273.15 = 600.15 𝐾. (B) Since the options are rounded to whole numbers, the closest answer is (A) 600 K 7. Given: Mole fraction of gas 𝐴 = 0.341, Total pressure = 5.2 𝑎𝑡𝑚. To find partial Pressure: Partial pressure of gas 𝑨 = Mole fraction of gas 𝑨 × Total pressure Partial pressure of gas 𝑨 = 0.341 × 5.2 = 1.7732 atm. The answer isn’t stated 8. To find the volume of Gas at increase pressure: SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) Given: 𝑃1 = 25𝑎𝑡𝑚 𝑉1 = 150 𝑐𝑚3 𝑃1 = 75𝑎𝑡𝑚 𝑉2 =? 𝑢𝑠𝑖𝑛𝑔 𝐵𝑜𝑦𝑙𝑒𝑠 𝑙𝑎𝑤 : 𝑃1 𝑉1 = 𝑃2 𝑉2 25 × 150 = 75 × 𝑉2 25×150 𝑉2 = = 50 𝑐𝑚3 75 𝑡ℎ𝑒 𝑎𝑛𝑠𝑤𝑒𝑟 𝑖𝑠 (𝐵)50 𝑐𝑚3 9. To know the gas that possesses Maximum r.m.s speed, you have to know that: At the same temperature, the gas with the smallest molar mass has the highest r.m.s. speed. Hydrogen has the smallest molar mass. The answer is (C) Hydrogen. 10.To find Volume of an ideal Gas: Given: 𝑛 = 1.5 𝑚𝑜𝑙𝑒𝑠, 𝑇 = −15°𝐶 = 258.15 𝐾 𝑃 = 2𝑎𝑡𝑚, 𝑅 = 0.082 𝑎𝑡𝑚. 𝑑𝑚 3. 𝑚𝑜𝑙 −1 using Ideak Gas Law : 𝑃𝑉 = 𝑛𝑅𝑇 𝑛𝑅𝑇 1.5×0.082×258.15 𝑉= = = 15.87𝑑𝑚 3 𝑃 2 The answer is A) 15.87𝑑𝑚 3 11.Helium is known to deviate positively from ideality at all conditions due to its very low intermolecular forces. The answer is (B) helium. 12.Real gases deviate from ideal behavior under conditions of high pressure and low temperature. The answer is (A) high P and low T. 13.To find its change in momentum per sec: Given: A molecule makes 5 elastic collisions with a wall per second, each collision changes its momentum by 2𝑚𝑣 SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) change in momentum per second= 5 × 2𝑚𝑣 = 10𝑚𝑣 The answer is (D) 10mv. 𝑃𝑉 14.Pressure of gas in Equation = 𝑅𝑇 2 Rearranging the equation to the form 𝑃𝑉 = 𝑛𝑅𝑇. We get 𝑛 = 2 The answer is (B) 2 moles of gas. 15.To find the rate of Diffusion of Gas X: Given: 280 cm³ of gas X diffuses in 40 seconds. Rate of diffusion = 𝑉𝑜𝑙𝑢𝑚𝑒/𝑇𝑖𝑚𝑒 280 = 7.0 cm³/sec 40 The answer is (A) 7.0 cm³/sec. 16..To Calculate the Molar Gas Constant 𝑅. Given: 1 mole of gas occupies 22.415 dm³ at 1 atm and 0°C (273.15 K). using Ideak Gas Law : 𝑃𝑉 = 𝑛𝑅𝑇 𝑃𝑉 1𝑎𝑡𝑚×22.415 dm³ 𝑅= = = 0.08206𝑎𝑡𝑚. 𝑑𝑚 3. 𝑚𝑜𝑙−1 𝑛𝑇 1𝑚𝑜𝑙 ×273.15 K 𝑡ℎ𝑒 𝑎𝑛𝑠𝑤𝑒𝑟 𝑖𝑠 (𝐴)0.08206𝑎𝑡𝑚. 𝑑𝑚 3. 𝑚𝑜𝑙−1 17.An ideal gas differs from a real gas in that the molecules of an ideal gas (D) have no attraction for one another 18.Correct Statement about Molar Gas Volume: For 𝑛 number of molecules, the correct relationship is (A) 𝑉 = 𝑛𝑉𝑚 19..At low temperatures, real gases show (B) negative deviation from ideality. 20. One of the Factors Responsible for Difference between Ideal and Real Gases: is (C) Van der Waals forces 21.(D) Neutralization is a chemical change, not a physical change. 22. The head Absorbed in the process C (graphite) → C (Diamond is called the heat of Transition(C ) 23.The quantity of heat 𝑞𝑝 absorbed when temperature increases at constant Pressure is dependent on Heat capacity. (A) 24. The Heat of Combustion of Benzene at Constant Pressure: Given: ∆𝑈 𝑎𝑡 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 𝑣𝑜𝑙𝑢𝑚𝑒 = −3272 𝑘𝐽 ∆𝐻 = ∆𝑈 + ∆𝑛𝑅𝑇 SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 1 𝑤ℎ𝑒𝑟𝑒 ∆𝑛 = − 2 ∆𝐻 = −3272𝑘𝐽 (since ∆𝑛𝑅𝑇 is negligible at 300k). 𝑡ℎ𝑒𝑟𝑒𝑓𝑜𝑟𝑒 ∶ 𝑎𝑛𝑠𝑤𝑒𝑟 𝑖𝑠 (𝑐) − 3272𝑘𝐽 25. The Equations with heat change values are called: Thermochemical equations. (D) 26. This type of reaction C+ 𝑂2 → 𝐶𝑂2 ∆𝐻 = −393.513 KJ is Endothermic(B) 27.Physicochemical Changes with Absorption of Heat: These changes are referred to as (A) Endothermic. 28. To determine the calorific value of Propane: Given : 𝑘𝑐𝑎𝑙 Molar heat of combustion= −526.3 𝑚𝑜𝑙 𝑔 Molar mass of propane 𝐶3 𝐻8 = 44. 𝑚𝑜𝑙 526.3𝑘𝑐𝑎𝑙 𝑐𝑎𝑙𝑜𝑟𝑖𝑓𝑖𝑐 𝑣𝑎𝑙𝑢𝑒 = = 11.96 𝑘𝑐𝑎𝑙/𝑔 44𝑔 The answer is (B) 11.96 𝑘𝑐𝑎𝑙/𝑔 29. Calculate the heat of reaction between F𝑒2 𝑂3 and C𝑂2 ∆𝐻 = [∆𝐻𝑓 (𝐹𝑒2 𝑂3 ) + ∆𝐻𝑓 (C𝑂2 )] − ∆𝐻𝑓 (𝐶𝑂) ∆𝐻 = [−838.52 + (−393.5)] − (−110.53) ∆𝐻 = −1121.55 + 110.53 ∆𝐻 = −11011.02𝑘𝐽 30.The Instrument for Determining Heat of Reaction: is a Bomb Calorimeter. (C) 31.The quantity of heat which must be applied to decompose a compound into its elements is equal to the heat evolved when the compound is formed from its elements is called the law of (A) Lavoisier and Laplace. 32. (D) Combustion is a chemical change. 33.The enthalpy change when one mole of a solute is added to such a large amount of solution that the concentration of the solution remains unchanged is called (A) Heat of dilution. 34. C-H bond energy Calculation Given: Heat of formation 𝐶𝐻4 = −74.85𝑘𝐽 Heat of dissociation of 𝐻2 = 430.95𝑘𝐽 Heat of sublimation of graphite 𝐶 = 711.28𝑘𝐽 SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) ∆𝐻 = ∆𝐻𝑓 (C𝐻4 ) + 4 × ∆𝐻𝑑𝑖𝑠𝑠𝑜𝑐𝑖𝑎𝑡𝑖𝑜𝑛 (𝐻) − ∆𝐻𝑠𝑢𝑏𝑙𝑖𝑚𝑎𝑡𝑖𝑜𝑛 (𝐶 ) 430.95 ∆𝐻 = −74.85 + 4 × − 771.28 2 ∆𝐻 = 75.77 75.77 The C-H bond energy should be calculated for 4 bonds, so =18.94 kJ 4 per bond, but this calculation doesn't match any options. It might need reevaluation. 35.The correct unit of rate of reaction is 𝑀𝑠 −1 (A) 36. To find the average rate of reaction Given: Change in [CO] =0.05M, Time= 60sec 𝑐ℎ𝑎𝑛𝑔𝑒 𝑖𝑛 [𝐶𝑂] 0.05 𝐴𝑣𝑒𝑟𝑎𝑔𝑒 𝑟𝑎𝑡𝑒 = = = 8.33 × 10−4 𝑀/𝑠 𝑡𝑖𝑚𝑒 60 Option (B) 37.A catalyst may facilitate the rate of reaction by lowering the reaction's (𝐸) Activation energy. 38. From the Expression : Rate= 𝐾[𝐴]𝑛 In the expression, 𝑛 represents order of the reaction (D) 39.From the Expression : Rate= 𝐾[𝐴]𝑛 In the expression, 𝑘 stands for rate constant (C) 40.An acid-base conjugate pair are any two substances which differ in chemical composition by a Proton(C) 41. The overall order of reaction (𝑟𝑎𝑡𝑒 = 𝑘[𝐴][𝐵]) is 2.(E) 42.An example of a reference electrode is (c) Standard Hydrogen Electrode. 43. The equation of dissolution of 𝐶𝐻₃𝐶𝑂𝑂𝑁𝑎 in water is 𝐶𝐻₃𝐶𝑂𝑂𝑁𝑎 + 𝐻₂𝑂 → 𝑁𝑎⁺ + 𝐶𝐻₃𝐶𝑂𝑂𝐻. option(A) 44.The reaction of ion and water is referred to as (d) hydrolysis. 45.When an element undergoes oxidation, the oxidation number (c) Increases. 46.An element undergoing reduction shows a (a) Decrease in the oxidation number. 47.Methods include (c) a, b, d & e. 48.Buffer solutions show resistance to changes in (b) pH when small amounts of acids and bases are added. 49.These substances are called (c) electrolytes. SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 50.A good example of a Lewis acid is (b) AlCl₃. 51.The pOH of a solution is defined as the negative logarithm of the hydroxide ion concentration: 𝑝𝑂𝐻 = −log[𝑂𝐻 − ] Thus the correct answer is A 52.The dissociation constant (Ka) of an acid measures its strength; a larger Ka indicates a stronger acid because it dissociates more completely in water: Thus, the larger the dissociation constant of an acid, the (d) Stronger is the acid. 53. Sulphuric acid (H₂SO₄) is a strong diprotic acid, meaning it dissociates completely in water to produce 2 moles of H⁺ ions for every 1 mole of H₂SO₄: For a 0.03 M solution of H₂SO₄ the concentration of 𝐻+ ions is 2 × 0.03𝑀 = 0.06𝑀 The pH is calculated using the formula: 𝑝𝐻 = −log[𝑂𝐻 + ]. Substituting in the concentration: pH= − log(0.06) = 1.22 The answer is (C ) 54.The relationship between pH and pOH in a solution is given by: 𝑝𝐻 + 𝑝𝑂𝐻 = 14 From the previous calculation, we know that the 𝑝𝐻 = 1.22 To find pOH: 𝑝𝑂𝐻 = 14 − 𝑝𝐻 = 14 − 1.22 𝑝𝑂𝐻 = 12.78 Option (D) SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 2022/2023 EXAMINATION QUESTION 1. Nitrogen gas occupied a volume at a pressure o 0.971 atm calculate the volume it will occupy if the pressure is increased to 150 atm at constant temperature. A) 342 mL, B) 424 mL, C) 324 mL, D) 442 mL, E) 242 mL. 2. Hydrogen gas was found to occupy a 4 liter container at a temperature of 320 K and it exerts pressure of 800torrs. The gas was transferred into a 2 liter container and cooled to 160 K. Calculate the new pressure it will exert. A) 800 torr B) 1600 torr C) 200 torr D) 400 torr E) 500 torr. 3. Which gas law is involved hen a balloon pops after being sat on? A) Charles Law B) Boyles Law C) Law of Pressure Gradient D) Daltons Law E) Avogadros Law. 4. A small sample of helium gas occupies 6 mL at a temperature of 250 K. At what temperature does the volume expand to 9 mL? A) 125 K B) 375 K C) 500 K D) 2250 K E) 225 K. 5. Arrange the following gasses in order of their rate of diffusion from the slowest to the fastest (i) Oxygen (ii) Ammonia (iii) Hydrogen (iv) Carbon dioxide. A) Hydrogen, Oxygen, Carbon dioxides, Ammonia B) Oxygen, Hydrogen, Carbon dioxide, Ammonia C) Hydrogen, Ammonia, Oxygen, Carbon Dioxide D)Hydrogen, oxygen, ammonia, carbon dioxide. E) Carbon dioxide, oxygen, ammonia, hydrogen 6. PV/nRT is known as___________A) compressibility factor, B) volume factor C) pressure factor, D) temperature factor, E) Ideality factor 7. Compressibility can be expressed as_________ A) real volume divided by the ideal volume, B) real universal gas constant by ideal universal gas constant, C) real temperature by ideal temperature D) real volume divided by real pressure E) none of the above. 8. Above Boyle temperature real gases show deviation from ideal gases. A) positive, B) negative, C) no, D) both positive and negative, E) all of the above. 9. What are the units of "b" in van der Waals equation? A) L B) L mol C) 1/L mol D) L/mol E) mmHg 10.The density of chlorine gas at STP in grams per liter, is approximately.A) 6.2, B) 3.2, C) 3.9, (D) 4.5, E) 1.3 11.What is the molecular weight of a pure gaseous compound having a density of 4.95 g/L at -35 °C and 1020 torr? (A) 24, B) 11, C) 72 D) 120, E) 44 SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 12.A real gas most closely approaches the behavior of an ideal gas under conditions of: A) high P and low T, B) low P and high T, C) low P and T, D) high P and T, E) STP 13. What pressure (in atm) would be exerted by a mixture of 1.4 g of nitrogen gas and 4.8 g of oxygen gas in a 200 mL container at 57°C? A) 4.7, B) 34 C) 47, D) 27, E) 0.030 14.Calculate the molar gas constant for a mole gas that occupies a volume of 22.4dm³ at 0 °C and 1.0 atmospheric pressure. A) 0.08206 𝑎𝑡𝑚𝑑𝑚 3 𝑚𝑜𝑙−1 𝐾 −1 B) 0.8206 𝑎𝑡𝑚𝑑𝑚 3 𝑚𝑜𝑙−1 𝐾 −1 C) 8.0206 𝑎𝑡𝑚𝑑𝑚 3 𝑚𝑜𝑙−1 𝐾 −1 D) 0.8206 𝑎𝑡𝑚𝑑𝑚 3 𝑚𝑜𝑙−1 𝐾 −1E) 8.314 𝑎𝑡𝑚𝑑𝑚 3 𝑚𝑜𝑙−1 𝐾 −1 15.A mixture of gases contains 0.31 moles of methane, and 0.25 moles of ethane. If the total pressure of the gaseous mixture is 1.5 atm. Calculate the partial pressure of methane. A) 0.67 atm. B) 0.45 atm. C) 0.83 atm.,D) 0.55 atm. E) none of the above 16.Convert 2.3 atmosphere to mmHg. A) 2300 mmHg, B) 230 mmHg C) 2.3 mmHg D) 0. 23mmHg E) 23 mmHg 17.A molecule of mass m moving with a velocity v makes 5 elastic collisions with a wall of the container per second. The change in its momentum per second will be- A) mv, B) 5 mv C) mv/10 D) 10 mv E) 25 mv 𝑃𝑉 18. = RTP represents the pressure of (A) Any amount of gas (B) 2 moles 3 of gas (C) 3 moles of gas (D) 4 moles of gas (E) 6 moles of gas 19.If helium effuses through a porous barrier at a rate of 4.0 moles per minute, at what rate (in moles per minute) would oxygen gas diffuse? A) 0.20, B) 0.50, C) 2.0, D) 8.0 E) 1.41 20.How does one liquid a gas A) By increasing temperature, B) By Reducing Pressure C) By reducing pressure and temperature D) by increasing pressure and reducing temperature E) by increasing the volume and reducing temperature 21.Consider the equation HCl (g) + 5H₂O (I)- → HCl in 5H₂O ∆𝐻 =63.995 kJ. The heat evolved in this process is called (A) Heat of dilution (B) Integral heat of dilution (c) Heat of solution (D) Integral heat of solution (E) Mixing 22.Which of these is not a division of defect and imperfections? (A) Point defect (B) Planar defect (C) Line defect (D) Volume defect (E) Annealing defect SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 23.An equation in which the value of heat change is given is called (A) Enthalpy equation (B) Entropy equation (C) Physicochemical equation (D) Thermo-chemical equation (E) Latent heat equation 24.The two dimensional imperfection that enables a ferromagnetic material to be magnetized and demagnetized is called (A) Bloch walls (B) Interfacial defect (C) Bulk defects (D) Dislocation walls (E) Volume defect 25. Consider the equation; ∆𝐻 = ∆𝐸 + P∆𝑉, what will be the value of ∆𝐻 if the reaction is run in a bomb calorimeter? (A) ∆𝐻 = ∆𝐸 + ∆𝑛 (RT) (B) ∆𝐻 = ∆𝐸 + P∆𝑉 (C) ∆𝐻 = ∆𝐸 (D) ∆𝐻 = 𝑃∆𝐸 (E) ∆𝐻 = ∆𝐸 – P∆𝑉 26.The migration of a cation and an anion to the surface, creating a vacancy pair defect is referred to as (A) Schottky imperfection (B) Frenkel imperfection (C) Vacancy-interstitial pair defect (D) High-energy(E) Macroscopic defect 27.In a dissolution process; when the heat absorbed 𝑞1 is greater than the heat released from the interaction with the solutes and solvent 𝑞2 , the dissolution is termed (A) Endothermic (B) exothermic (C) Negative enthalpy (D) Positive enthalpy (E) Hydrolysis 28.The plane in which a dislocation moves through the lattice is called (A) draw (B) plane symmetry (C) Slip (D) Fracture (E)fractional plane 29.The quantity of heat Op absorbed when the temperature of the system is increased at constant pressure depends on the followings except (A) The weight of the system (B) The temperature increase (C) The heat of dilution (D) The specific heat capacity of the system (E) All of the above 30.What is the name given to the motion of dislocation when the extra half plane is extended farther or partially withdrawn from it? (A) Dislocation drive (B) Dislocation plane(C) Dislocation angle (D) Dislocation climb (E) Dislocation symmetry 31.Physicochemical changes accompanied by absorption of heat are referred to as (A) Endothermic (B) Exothermic (C) Thermometry (D) Thermodynamics (E) Latent 32.Interfaces between solid and gases are known as (A) Domain boundaries (B) Grain boundaries (C) Crystalline lattice (D) Phase boundaries (E) Free boundaries 33.The relationship between the heat of reaction at constant pressure (∆H) and at constant volume (∆E) is given by (A) ∆𝐻 = ∆𝐸 + 𝑃∆𝑉(B) ∆ E=∆𝐻 + 𝑃∆𝑉(C) ∆H=∆E, (D) ∆H=∆n(RT) (E) ∆E=nRT SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 34. A homogenous, physically distinct and mechanically separable portion of the material with a given chemical composition and structure is known as (A) Crystal (B) Lattice (C) System (D) Phase (E) Boundary 35.The study of the heat changes accompanying chemical reaction and physical changes is called (A) Thermochemistry (B) Thermo gravimetric (C) Thermo chemical (D) Thermo couple (E) Thermo static 36. The pattern of particles, which describes the arrangement of particles in a crystal is known as (A) X-ray (B) Crystal dimension (C) Lattice (D) Polymorphism (E) Hexagonal 37.If the molar heat of combustion of liquid benzene at constant volume and 300K is 3272 kJ, what will be the heat of combustion at constant pressure at the same temperature? (A) 7203 kJ (B)-4562 kJ (C) - 3270 kJ(D) 4823 kJ (E)-7203 kJ 38.The followings are examples of crystal systems except (A) Orthorhombic (B) Hexagonal (C) Rhombohedral (D) Tetragonal (E) Diagonal 39.Heat absorbed during the process of vapourization without change in temperature of the system is called (A) Latent heat (B) Heat of sublimation (C) Heat of dilution (D) Enthalpy change (E) Heat of atomization 40.The interaction of the solute molecules or ions with the solvent molecules during dissolution is referred to as (A) Hydration (B) Solvation (C) Dilution (D) Liquefaction (E) Solution 41.All these are electrolytes except (a) NaCl (b) KCI (c) CuCl (d) sugar (e) CuSO4 42.Which of these is/ are strong electrolyte(s) (a) NaCl (b) sugar (c) C𝐻3 COOH (d) a &b (e) b & c 43.Ethanoic acid can show acidic property in the presence of_____(a) Benzene (b) Toluene (c) cyclohexane (d) b &c (e) water 44._________+ 2𝐻 +→C𝑢2++𝐻2 O; the missing reactant is: (a) Cu (b) CO (c) CuO (d) H2 (e) H 45.An acid-base conjugate pair are any two substances which differ in chemical composition by (a) electron (b) hydroxonium (c) proton (d) positron (e) nucleon 46.These are Bronsted - Lowry acids, except (a) KHS𝑂4 (b) N𝐻4+ (c) HCI (d) C𝐻3 COOH (e) N𝐻3 47.Any substance which has ability to accept or donate proton is called_____(a) phiprotic (b) amphitic (c) protic (d) amphiprotic (e) amphi SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 48.H𝑔2+ can behave as_____(a) base (b) acid (c) protic (d) amphiprotic (e) amphi 49.Concentration of OH ions in a certain household ammonia cleaning solution is 0.001 M. Calculate the [H].(a) 1 × 10−11 M (b) 2× 10−11M (c) 3 × 10−11M (d) 1 × 10−13M (e) 1× 10−14M 50.Calculate the pH of 0.03 M 𝐻2 S𝑂4 (a) 3.11 (b) 2.22 (c) 0.21 (d) 1.22 (e) 2.00 51.Hence determine the pOH of 𝐻2 S𝑂4 in the above question (a) 12.00 (b) 12.78 (c) 13.79 (d) 11.78 (e) 10.89 52.Calculate [H] of 0.03 M acetic acid solution (take K, 1.80 × 10−5 M) (a) 0.000735 M (b) 0.00735 M (c) 0.0735 M (d) 0.735 M (e) 7.35 M 53.Hence determine the degree of dissociation (a) of acetic acid in the above question (a) 3.45% (b) 2.45% (c) 1.45% (d) 0.45% (e) 3.55% 54.The name of this salt, HONH,CI is _______ (a) lamine chloride (b) hydroxyl chloride (c) ammonia chloride (d) hydroxylamine chloride (e) none of the above 55.What is the [OH] of 0.2 M C𝐻3 COONa solution? Ka= 1.80 × 10−5 (a) 1.05 × 10−7 (b) 5.05 × 10−5 M(c) 3.05 × 10−5M (d) 1.05 × 10−5M (e) 2.05 × 10−5 M 56.Hence determine the pOH (a) 5.98 (b) 2.98 (c) 3.98 (d) 4.98 (e)0.98 𝐾𝑤 57.Which of these is a correct relationship; (a) 𝐾ℎ = (b) 𝐾𝑤 = 𝐾ℎ × 𝐾𝑎 𝐾𝑎 𝐾ℎ (c) 𝐾𝑎 = (d) a & b (e) all of the above 𝐾𝑤 58.The reaction of ion and solvent is known as____________(a) solvolysis (b) hydrolysis (c) oxidation (d) neutralization (e) displacement 59.Lewis acid is an electron pair_____ (a) donor (b) acceptor (c) oxidation (d) reduction (e) neutralization 60.Solutions that show resistance to changes in pH when small amount of acids and bases are added are called (a) electrolytes (b) nonelectrolyte (c) buffers (d) a& b (e) none of the above. SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 2022-2023 ANSWERS 1. From the question Given: initial pressure 𝑃1 = 0.971 𝑎𝑡𝑚 Final pressure 𝑃2 = 150 𝑎𝑡𝑚 initial Volume 𝑉1 = 𝑛𝑜𝑡 𝑔𝑖𝑣𝑒𝑛 and we were asked to find final volume V2 which we cant find since we were not given V1 𝑃1 𝑉1 𝑉2 = 𝑃2 2. Given: initial pressure 𝑃1 = 800 𝑡𝑜𝑟𝑟 final volume 𝑉2 = 2𝐿 initial Volume 𝑉1 = 4𝐿 initial Temperature 𝑇1 = 320𝐾 Final Temperature 𝑇2 = 160𝐾 To find , final pressure 𝑃2 Using combined gas law 𝑃1 𝑉1 𝑃2 𝑉2 = 𝑇1 𝑇2 𝑃1 𝑉1 𝑇2 𝑃2 = 𝑇1 𝑉2 800×4×160 𝑃2 = = 800 𝑡𝑜𝑟𝑟 320×2 Option A) 3. A balloon pops when sat on because the pressure inside increases as the volume decreases. Law Used: Boyle's Law (pressure and volume are inversely proportional) So the correct answer is: B) Boyle's Law 4. Given: Initial volume 𝑉1 = 6𝑚𝐿 Initial Temperature 𝑇1 = 250𝑘, Final Volume 𝑉2 = 9𝑚𝐿 To find : Final Temperature 𝑇2 Using Charles law: 𝑉1 𝑇1 = 𝑉2 𝑇2 𝑉2 𝑇1 9×250 𝑇2 = = = 375𝐾 𝑉1 6 Option B) SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 5. The rate of diffusion of a gas is inversely proportional to the square root of its molar mass (Graham's Law). Molar masses:  Oxygen (O2) ≈ 32 g/mol  Ammonia (NH3) ≈ 17 g/mol  Hydrogen (H2) ≈ 2 g/mol  Carbon dioxide (CO2) ≈ 44 g/mol The correct order from slowest to fastest is based on the molar mass: E) Carbon dioxide, Oxygen, Ammonia, Hydrogen 6. PV/nRT is known as: A) compressibility factor 7. Compressibility can be expressed as: A) real volume divided by the ideal volume 8. Above Boyle temperature real gases show deviation from ideal gases: A) positive 9. What are the units of "b" in van der Waals equation? : D) L/mol 10.The density of chlorine gas at STP in grams per liter, is approximately: B) 3.2 11.To find the molecular weight (M), we can use the ideal gas law rearranged as follows: 𝑑𝑅𝑇 𝑀= 𝑃 Where : 𝑑 = 𝑑𝑒𝑛𝑠𝑖𝑡𝑦 = 4.95 𝑔/𝑙 𝐿 𝑎𝑡𝑚 𝐿 𝑡𝑜𝑟𝑟 𝑅 = 0.0821 = 62.36 𝐾𝑚𝑜𝑙 𝐾𝑚𝑜𝑙 𝑇 = −35𝐶 + 273 = 238𝐾 𝑃 = 1020 𝑡𝑜𝑟𝑟 4.95×62.36×238 𝑀= = 72 𝑔/𝑚𝑜𝑙 1020 Option C) 12.A real gas most closely approaches the behavior of an ideal gas under conditions of: B) low P and high T 13. Firstly, we calculate the number of moles of each gas: Molar mass of 𝑁2 = 28 𝑔/𝑚𝑜𝑙 Molar mass of 𝑂2 = 32 𝑔/𝑚𝑜𝑙 SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 1.4𝑔 Moles of 𝑁2 = = 0.05 𝑚𝑜𝑙 28 𝑔/𝑚𝑜𝑙 4.8𝑔 Moles of 𝑂2 = = 0.15 𝑚𝑜𝑙 28 𝑔/𝑚𝑜𝑙 Total moles of the gas = 0.05 + 0.15 = 𝟎. 𝟐𝟎 𝒎𝒐𝒍 Convert the temperature to Kelvin: 𝑇 = 57 + 273 = 330𝐾 Use the ideal gas law to find the total pressure: 𝑃𝑉 = 𝑛𝑅𝑇 𝑛𝑅𝑇 𝑃= 𝑉 0.20×0.0821×330 𝑃= = 27𝑎𝑡𝑚 0.2000 Option D) 14. Using the ideal gas law: 𝑃𝑉 = 𝑛𝑅𝑇 𝑃𝑉 𝑅= 𝑛𝑇 𝑤ℎ𝑒𝑟𝑒: 𝑃 = 1𝑎𝑡𝑚 𝑉 = 22..4 𝑑𝑚 3 𝑛 = 1𝑚𝑜𝑙 𝑇 = 0℃ = 273𝐾 1×22.4 𝑅= = 0.0821 𝑎𝑡𝑚𝑑𝑚3 𝑚𝑜𝑙−1 𝐾 −1 1×273 𝑜𝑝𝑡𝑖𝑜𝑛 𝐴 15. Using Dalton’s law of Partial Pressure: 𝑛𝐶𝐻4 𝑃𝐶𝐻4 = × 𝑃𝑡𝑜𝑡𝑎𝑙. 𝑛𝑡𝑜𝑡𝑎𝑙 𝑤ℎ𝑒𝑟𝑒: 𝑛𝑡𝑜𝑡𝑎𝑙 = 0.31 + 0.25 = 0.56 𝑚𝑜𝑙𝑒𝑠 0.31 𝑃𝐶𝐻4 = × 1.5 = 0.83 𝑎𝑡𝑚 0.56 𝑜𝑝𝑡𝑖𝑜𝑛 𝐶) 16.To convert 2.3 atmosphere to mmHg 1𝑎𝑡𝑚 = 760𝑚𝑚𝐻𝑔 2.3𝑎𝑡𝑚 = 2.3 × 760 = 1748𝑚𝑚𝐻𝑔 SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 17.In each collision, the momentum change is 2𝑚𝑣 (since it reverses direction). For 5 collisions per second: Change in momentum per second= 5 × 2𝑚𝑣 = 10𝑚𝑣 D) 10 mv 18.Rearranging the equation 𝑃𝑉 = 3𝑅𝑇 implies 3 moles of gas because the gas constant 𝑅 is typically for 1 mole. C) 3 moles of gas 19.Using Grahams law of Effusion: 𝑅𝑎𝑡𝑒 𝑜𝑓 𝐻𝑒 𝑀𝑂2 =√ 𝑅𝑎𝑡𝑒 𝑜𝑓 𝑂2 𝑀𝐻𝑒 4.0 𝑚𝑜𝑙𝑒𝑠/𝑚𝑖𝑛 4.0 𝑅𝑎𝑡𝑒 𝑜𝑓 𝑂2 = = = 1.41 √ 33 √8 4 Option E) 20.How does one liquefy a gas: D) by increasing pressure and reducing temperature 21. The process is called: Heat of Dilution (A) 22. E) Annealing defect 23.D) Thermo-chemical equation 24.A) Bloch walls 25.In a bomb calorimeter, the volume is constant, so 𝛥𝑉 = 0, hence: 𝛥𝐻 = 𝛥𝐸 C) ∆H = ∆E 26. A) Schottky imperfection 27.A) Endothermic 28.C) Slip 29.C) The heat of dilution 30.D) Dislocation climb 31.Physicochemical changes accompanied by absorption of heat are referred to as: A) Endothermic 32.Interfaces between solid and gases are known as: D) Phase boundaries 33.The relationship between the heat of reaction at constant pressure (∆H) and at constant volume (∆E) is given by: A) ∆H = ∆E + P∆V SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 34.A homogeneous, physically distinct and mechanically separable portion of the material with a given chemical composition and structure is known as: D) Phase 35.The study of the heat changes accompanying chemical reactions and physical changes is called: A) Thermochemistry 36.The pattern of particles, which describes the arrangement of particles in a crystal is known as: C) Lattice 37. At constant volume ∆𝐸 = −3272 𝑘𝐽 Using : ∆𝐻 = ∆𝐸 + 𝑃∆𝑉 𝑤𝑒 𝑎𝑝𝑝𝑟𝑜𝑥𝑖𝑚𝑎𝑡𝑒 ∆𝐻 ≈ ∆𝐸 (𝑠𝑖𝑛𝑐𝑒 𝑐ℎ𝑎𝑛𝑔𝑒𝑠 𝑎𝑟𝑒 𝑡𝑦𝑝𝑖𝑐𝑎𝑙𝑙𝑦 𝑠𝑚𝑎𝑙𝑙) C) -3270 kJ (since it's closest to -3272 kJ) 38.The following are examples of crystal systems except: E) Diagonal 39.Heat absorbed during the process of vaporization without change in temperature of the system is called: A) Latent heat 40.The interaction of the solute molecules or ions with the solvent molecules during dissolution is referred to as: B) Solvation 41.All these are electrolytes except: (d) sugar 42.Which of these is/are strong electrolyte(s): (a) NaCl 43.Ethanoic acid can show acidic property in the presence of: (e) water 44.The missing reactant is: (c) CuO 45.An acid-base conjugate pair are any two substances which differ in chemical composition by: (c) proton 46.These are Bronsted-Lowry acids, except: (e) NH₃ 47.Any substance which has the ability to accept or donate a proton is called: (d) amphiprotic 48.Hg²⁺ can behave as: (d) amphiprotic 49.To calculate [𝐻+ ] Given that: [𝑂𝐻− ] = 0.001 𝑀 Using: [𝐻 + ][𝑂𝐻− ] = 10−14 SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 10−14 [𝐻+ ] = = 10−11 𝑀 0.001 Option A) 50.Calculate the pH of 0.03 M H₂SO₄: H₂SO₄ dissociates completely to give 2𝐻+ : [𝐻+ ] = 2 × 0.03 𝑀 = 0.06𝑀 𝑝𝐻 = −log(0.06) ≈ 1.22 Option d) 51. To determine the 𝑝𝑂𝐻 of the above question: 𝑝𝑂𝐻 = 14 − 𝑝𝐻 = 14 − 1.22 = 12.78 Option B) 52. Using the formula of weak acid: [𝐻+ ] = √𝐾𝑎 × [𝑎𝑐𝑖𝑑] = √1.80 × 10−5 × 0.03 ≈ 0.000735 𝑀 Option A) 53. To determine the degree of dissociation α\alphaα of acetic acid in the above question: [𝐻 +] 0.000735 ∝= = × 100% ≈ 2.45% [𝑎𝑐𝑖𝑑] 0.03 𝑜𝑝𝑡𝑖𝑜𝑛 𝐵 54.The name of this salt, HONH₂Cl is: (d) hydroxylamine chloride 55. The acetate ion (𝐶𝐻3 𝐶𝑂𝑂−) is a weak base , so we need to use the base dissociation constant 𝐾𝑏 𝐾𝑤 𝐾𝑏 = 𝐾𝑎 𝑔𝑖𝑣𝑒𝑛: 𝐾𝑤 = 1.0 × 10−14 1.0×10−14 𝐾𝑏 = = 5.56 × 10−10 1.80×10−5 Next, we use the formula for the concentration of 𝑂𝐻 − in a weak base solution: [𝑂𝐻− ] = √𝐾𝑏 × [𝑏𝑎𝑠𝑒] = √5.56 × 10−10 × 0.2 ≈ 3.33 × 10−5 None of the provided options directly match this calculation. However, the closest value is: (c) 3.05 × 10{−5} 56.. to determine pOH from the above question: 𝑝𝑂𝐻 = −𝑙𝑜𝑔[𝑂𝐻− ] = −log(3.33 × 10−5)≈ 4.48 None of the options provided directly match this calculation either. However, the closest value is; (d) 4.98 SOLVE EASY ACADEMY CHM 101 ©InnocentJeremiah (07037026683) 57.. (d) a & b 58.The reaction of ion and solvent is known as: (b) hydrolysis 59.Lewis acid is an electron pair: (b) acceptor 60.Solutions that show resistance to changes in pH when small amounts of acids and bases are added are called: (c) buffers