"Short Note Phy. Che. PDF - Revision Notes"

## Revision ### Short Notes - Fast reaction { slow ren - Tonic reaction Molecular concentration of reactant or product - H+ + OH- H2O - Na Cl + Ag Nos - **Rate of Reaction:** The change in concentration of reactant or product per unit time is called R.O.R. - ROR = change in conc. of Rect. or...

## Revision ### Short Notes - Fast reaction { slow ren - Tonic reaction Molecular concentration of reactant or product - H+ + OH- H2O - Na Cl + Ag Nos - **Rate of Reaction:** The change in concentration of reactant or product per unit time is called R.O.R. - ROR = change in conc. of Rect. or prod/time. - unit = mol L⁻¹ s⁻¹ (aq.) - unit = atm s⁻¹ (gaseous) - **Elementary Reaction:** Takes place in single step. - **Complex reaction:** More than one step. - 3A + 4B -> 5C + 6D - 3 d[A]/dt = 4 d[B]/dt = 5 d[C]/dt = 6 d[D]/dt - d[C]/dt = 5/3 d[A]/dt - A + 2B -> 3C. Find d[C]/dt - -3 d[A]/dt = 2 d[B]/dt = d[C]/dt - d[C]/dt = -3 d[A]/dt = -2 d[B]/dt - -1/2 d[A]/dt = -1/2 d[B]/dt = d[C]/dt - ROR = -d[A]/dt = -1/2d[B]/dt = 1/2 d[C]/dt = 3/2 d[C]/dt - d[D]/dt = d[A]/dt = d[C]/dt - -3 d[A]/dt = d[C]/dt - d[C]/dt = -3 d[A]/dt = 4 d[B]/dt = 3/2 d[C]/dt - **Types of Rates of Reaction:** - **Average rate of reaction:** Measured over a period of time. It is denoted by Δ and expressed as Δ[A]/Δt - **Instantaneous R.O.R:** Measured over a very short time (t->0). Denoted by 'd' and expressed as d[ ]/dt. - **Notes:** 1. Time for ROR + ve sign. 2. Reactant के ROR के आगे –ve sign, और product के ROR के आगे + ve sign. - **Expression of ROR**: - A + B -> C + D - ROR = - d[A]/dt = - d[B]/dt = d[C]/dt = d[D]/dt ### Data - **Bank 2023 A:** - The rate of Rean 2A + B + C is represented by: - -1/2 d[A]/dt = - d[B]/dt = - d[C]/dt - ROR = + d[A]/dt = - d[B]/dt = - d[C]/dt - **Law of mass action:** Rate of Reaction is directly proportional to active mass of reactant raised by its stoichiometric coefficient. - RORα[A]³ - **Note from Question Bank:** - Rate depends on active mass of substance (2020;23A). - Rate Constant of Recfont(K) - Rate of Reaction when conch. of rectant is 1 Molar is called Rate Constant. - **Characteristics of "K":** - Depends on Temp. and Catalyst. - Does not depends upon Initial Conc. - Unit depends on Order of rean. - **Note from Question Bank:** - Rate Constant doesn't depend on temperature (2023). - ROR = K[A][B] - (A== I molar [B] 1 Molar) - ROR=K - **ROR:** - Rate Constant (K) - unit: moles L⁻¹ s⁻¹ (united) - unit: mol L⁻¹ s⁻¹ (on order of Reaction) - Depends on - Does not depend of conc. of recn. - Depends on conc. of rectop. - Change in conc. of rectop. - It is speed and proportional to conc. for reaction. - **Rate law (ROR = K[A]³)** - **The experimental relationship between Rate of Reaction and conc. of Reactont is called Rate law.** - **ROR = K[A]¹** - This is **Rate law** - **RDS = slow step.** - **Rate determining step = slow step.** ### Collision Theory of Chemical Reactions - **Given by Max Traute and lewis.** - **For chemical reactions, collisions are required.** - **The collision which forms product is called effective collision.** - **For effective collision two conditions are required:** - **Threshold Energy:** Minimum energy that must have by reactant to form product is called Threshold energy. - **Activation energy:** Minimum energy supplied to reactant to from product is called activation energy. - TE = Molecular K.E + Co - **Proper Orientation of reactant:** If ensures direct contact between reactant. - **Obj:** - ΔH = (f₀) f - (e₀) b... - ΔH = -ve (exd) - ΔH = +ve (endo) - **Note from compartment Q.B.**: - ΔH = (e₀) f - (e₀) b... - **Factors affecting ROR:** - **Ea of ROR** - **Size of ROR** - **P of ROR (for gas)** - **Catalyst:** Catalyst may increase or decrease Rate of Reaction. - +ve catalyst ↑ ROR by these activation energy. - -ve catalyst ↓ ROR by ↑ activation energy. - **Temperature:** T↑ = Molecules ↑ = Collision ↑ = ROR ↑ - On increasing Temperature Kinetic energy of molecules increase. Collision between reactant increases so Rate of Reaction increases. - For every 10℃ rate of reaction becomes 2-3 times. - **Note from Question Bank:** - Tempilatione Coff (1) = 2 - 3 - 20020 - **Concentration:** As conc. ↑ no of particles per liter ↑ so collision b/w reactant ↑ Hence Rate of Reaction increases ### Arrhenius equation - **The mathematical relationship between rate constant, Activation energy and temperature is called Arrhenius equation.** - **Molecules having energy equal to or greater than E⁻a/RT activation energy** - RORα e⁻Ea/RT - K = Ae⁻Ea/RT - **This is Arrhenius equation** - K = Rate Constant - A = Arrhenious Constant - Eₐ = Activation energy - T = Temperature (K) - R = Universal Gas Constant - **Arrhenius equation in log form:** - log₁₀ K = log₁₀ A - Ea/2.303 RT - **Note:** - loge = log₁₀ - Ea/RT - log₁₀ K₂ / K₁ = Ea / 2.303 RT (T₂ - T₁) - **Graph:** - **Molecularity of Reaction** - **Total no of rectant part in single step is called molecularity of reaction**. - **PCL₃ + CL₂ -> PCL₅** - Molecularity=2 - **2HI -> H₂ + I₂** - **It is theoretical.** - **Can not be negative.** - **Can not be fractional.** - **Order of Reaction** - **Sum of power on Conc. term in rate law is called Order of reaction.** - **In Rate law** - ROR = K[A] ᵐ [B] ⁿ - **Order w.r.t. "A" = m** - **Order w.r.t "B" = n** - **Order of reaction = m + n** - **Ex: Experimental** - ROR: K[A]³/² [B]³ - Order = 3/2 + 3 = 3 + 2 = 9/2 = 4.5 - **Order of Reaction Molecularity of reaction** - **Sum of power on total no. of rectant (concentrataterm in falce part in single rate law is called) step or rate determiny Order of Reach** - **Step is called molecularity of reaction** - **Experimental** - **It is exprimental** - **It is theoretical** - **It can not be -ve.** - **It can be negative** - **It can be zero** - **It can be Fractional** - **It can not be fractional** - **Note From Q. Bank** - Rate = K[A]²[B] - 2015(A) - Order of Reach - 3 - ROR = K[A]¹/² [B]¹/² - 2015(A) - Order of Reck = 2 - **Conce. effect on order of Reach** - **eg: Order w.r.t A = 2** - **Order w.r.t B = 1** - **[A] & [B] is halued (1/2).** - **ROR = ?** - **ROR: K[ + A]² (÷B] = 1/4 * 1/2 = 1/8 = ROR** - **Find order of Reaction** - conc. ↑ ROR ↑ ¹ Order - 0 - conc. ↑ ROR ↑² Order - 1 - conc. ↑ ROR ↑ⁿ Order - n - conc. ↑ ROR ↑n Order - n/2 - conc. ↑ ROR ↑¹/n Order - 1/n ### Zero order Reaction - **The Reaction in which Rate of Reaction is directly proportional to zeroth power of concentration of Reactant is called Zero order reaction.** - **RORα[A]⁰** - **ROR = K[A]⁰** - **ROR = K** - **Example:** - 1) H₂ + Cl₂ -> 2HCl - 2) 2NH₃ -> N₂ + 3H₂ - **Integrated Rate equation** - A - B - t₀ = 0 a = 0 - t₁ = t a = x - t₂ = ∞ a = ∞ - **From zero order** - ROR = K[A]⁰ - ROR = K (1) - **again:** - ROR = -d[A]/dt - = d[a₀ - x - a₀]/dt - ROR = dx/dt (11) - **From eqn (I) and (II):** - dx = kdt = dx = K.dt - **Integrated both Side of dx = Kdt**: - ∫dx = ∫Kdt - [x]₀ ᵃ = K[t]₀ ᵗ - **So, [at = a₀- x]** - **[at = a₀- Kt** - **This is integrated Rate of Zero order.** - **Half life time (t₁/₂)** - **The time in which 50% of the reaction is complete is called half life.** - **Expression:** - t = 0 at = a₀ = 0 - t = t at = a₀ - x - t = t₁/₂ at = a₀ - x = a₀/2 - **From zero odrer Reaction** - at = a₀ - kt - a₀/2 = a₀ - Kt₁/₂ - a₀ - a₀/2 = Kt₁/₂ - a₀/2 = Kt₁/₂ - t₁/₂ = a₀/2k - **Note:** - t₁/₂ α a₀ - t₁/₂ α 1/K - **Complete life time (τ)** - **The time in which 100% of the reaction is completed is called complete life.** - **Expression:** - t = 0 at = a₀ - t = t at = a₀ - x - t= ∞ at = a₀ - x = 0 - **from integrated T.O.R.** - at = a₀ - Kt - 0 = a₀ - KtLT - τ = a₀/K - **Note:** - t₁/₂ α a₀ - t₁/₂ α 1/K ### First order Reaction - **The reaction in which Rate of reaction is directly proportional tofirst power of concentration of recte reactant is called First order reaction.** - **RORα[A]** - **ROR = K [A]** - **Ex: All Radioactive decay ② Decomposition of N₂O** - **Integrated rate equation** - A -> - t = 0 at = a₀ x = 0 - t = t at = a₀ - x x = x - t = ∞ at = 0 x = a₀ - **From First Order** - ROR = K[A] - ROR: K(a₀- x)-(ⅰ) - **Again.** - ROR = -dA/dt - ROR = - d[a₀ - x - a₀]/dt - ROR = dx/dt (ii) - **From eqn (ⅰ) & (ii):** - dx/dt = K(a₀ - x) - dx/(a₀ - x) = Kdt - **Integrating both side** - ∫ dx/(a₀ - x) = ∫ Kdt - Kt = [-log(a₀ - x)]₀ ᵃ - Kt = [-loge(a₀ - x)] + [-loge(a₀)] - Kt = -loge(a₀ - x) + loge (a₀) - Kt = - loge [(a₀ - x)/a₀] - Kt = - loge (1 - x/a₀ ) - Kt = loge (a₀ / (a₀ - x)) - **Kt = loge (a₀/x)** - **Kt = 2.303 log₁₀ (a₀/x)** - **Half life for 1st Order** - t = 0 at = a₀ x = 0 - t = t₁/₂ at = a₀ - x x = a₀/2 - t = ∞ at = 0 x = a₀ - **From 1st order equation:** - Kt = 2.303 log₁₀ (a₀/x) - Kt₁/₂ = 2.303 log₁₀ (a₀ / (a₀/2) ) - Kt₁/₂ = 2.303 log₁₀ 2 - t₁/₂ = 2.303 log₁₀ 2 / K - **t₁/₂ = 0.693/K** - **Complete life or life-time** - t = 0 at = a₀ x = 0 - t = t at = a₀ - x x = x - t = τ at = 0 x = a₀ - **From ept. I. order equation** - Kt = 2.303×log₁₀ (a₀/x) - Kτ = 2.303×log₁₀ (a₀/0) - Kτ = ∞ - τ = ∞ - **So First Order reach never Completed.** - **Graph: Zero order** - **Graph for first Order** - ROR = k [conc.] ### Characteristics of 1st Order reaction - **All First Order reactions follow this equation: [Kt: 2.303log₁₀(a₀/x)].** - **Half life cloes not depend on concentration of recte: [t₁/₂ = 0.693/K]** - **First Order reaction never Completed:** - τ = ∞ ### Pseudo first Order reaction or, Pseudo unimolecular Reaction - **The reaction which is not of first order but behaves as First order under the suitable condition is called pseudo unimolecular Reaction.** - **Suitable condition is one of Reactant is in excess.** - **Ex:** - **Hydrolysis of ester:** - CH₃COOC₂H₅ + H₂O -> CH₃COOH + C₂H₅OH - Ethylethanoote H+ Ethyl acetate - ROR = K[CH₃COOC₂H₅] [H₂O] - Water is excess. it does not affect ROR - ROR: K[CH₃COOC₂H₅] - Hence, Order becomes first order, So this is pseudounimolecular Reaction. - **Inversion of come sugar**: - C₁₂H₂₂O₁₁ + H₂O -> C₆H₁₂O₆ + C₆H₁₂O₆ - ROR = k(C₁₂H₂₂O₁₁] [Hycose] - Hydrolysis of ester is pseudofirst Order Reaction why? ### Solution - **Solution: Homogenous mixture of two or more component (solute and solvent) is called solution.** - **Types of component: Solute ② Solvent** | Solution | Solute | Solvent | Example | |:------------------------|:-------|:--------|:-----------------------------------| | Solid solution | Solid | Solid | Alloy | | | Liquid | Solid | Amalgam of Na in Hg | | | Gas | Solid | Chasos presen in mineral | | Liquid solution | Solid | Liquid | Sugar in water | | | Liquid | Liquid | Alcohol in water | | | Gas | Liquid | O₂ in water | | Gas solution | Solid | Gas | Camphor in w'r | | | Liquid | Gas | Water vapour in air | | | Gas | Gas | Air, O₂ in N₂ | - **Concentration of solution:** The amount of solute present in given amount of solvent. Solution is called concentration of solution. - **Methods of conc. of solution:** - **Molarity:** The number of moles of solute present in 1 liter solution is called molarity. - It is denoted by 'M' (Molar) - It depends of Temp.. - Molarity: Moles of solute / Volume of solution (L) - Unit = mol/L or mol/dm³ - Volume 1 L = Molarity 1 - **Molality:** The no. of moles of solute present in 1 kg solvent is called molality. It's denoted by molal (m). - Molality = moles of solute / mass of solvent (kg) - It is not depend on temp. - Unit: mol/kg - **Notes:** - Molality is better concentration of solution than molarity. - **Mole Fraction:** The ratio of one moles of one component and total moles of solution is called moles fraction. It is denoted by X. - Mole Fraction: Moles of one component/ Total no. of solution - It is unit less. - **Formula:** - Moles of solute/ volume of solution - given mass of solute x1000/ Molecular mass of solute x Volume of solu. (ml) - Moles of solute/ Mass of soluent - Mass of solute x1000 / Molecular mass of solute x Mass of solvent - **Mass of solvent = Mass of solution - Mass of solute. ** - **Molecular Mass.** - Castis soda (NaOH) = 40g - Sugar or Cane Sugar = 342g - Glucose = 180 g. - H2SO4 = 98 g - H2O = 18g - Nacl = 58.5g - Urea = 60g - **Normality:** - [N = M x vf.] - 0.1M H3PO4 → N = ? - N = M x Vf - = 0.1 x 3 - = 0.3 N - **Normality depend on temp** - **Question from Question Bank:** 1. 239.2 g sugar syrup contains 34.2g of sugar what is molarity of solution. - Molarity= 342x1000 / 2000 = 0.5M 2. 2g NaCl present in 200ml solution. Is molarity? (2013;15) - Molarity: 2 x 1000 / 40 x 200 = 0.25M 3. If 18g glucose is present in 100g of solvent then the solution is said to be (2023A) - Molality: 18 x 1000 / 180 x 100 = 0.1 m ### Henry's law - **Statement:** At Constant temp. Solubility of gas in liquid is directly proportional to pressure of gas. - Pa solubility of gas - Pa = K_H x - P = pressure of gas - K_H = Henry constant. - x = Mole Fraction - **Scuba divers feel pain ful effect called bend when come towards surface of sea.** - **This is due to decompression of Neé gas which dissolved more due to high pressure of under water. To avoid painful effect of bends the gas cylinder of scubacdrivers is diluted with less soluble of Helium gas.** - **Note:** - K_H unit = unit of Conc. of gas - K_H ↑ d Solubility of gas - Aquatic amimals fell car in cold water then lat- water. - **Solubility of:** - Solubility of O₂ in water high, in water low. - Easy to breathe, tough to breathe. - So aquatic animals feel comfort in cold water than hot water. ### Vapour pressure - **Pressure exerted by vapour when it is in equilibrium with liquid is called vapour pressure. It depends on:** - Vapour press & temp: - v.p α Boiling point: - **When non-volatile Solute is added to pure solvent then vop. of solvent decrease why?** - On adding non-volatile solute the surface molecule of solvent are replaced by non-volatile solute so v.p decrease. - **Case I of Raoult's law:** - Liquid-solid solution - Solvent solution (non valatile) - Volatile solute (volatile) - **Statement:** At constant temp. vop of solution is directly proportional to mole Fraction of solvent in solution. - **Let: volatile solvent = A** - **non-volatile solvent = B** - **Mole Fraction of A = X_A** - **Mole Fraction of B = X_B** - **Vapour pressure of pure A: P_A** - **v.p of A in solution: P_A'** - **V.p of solu = P_S** - **Alic to Raoults law:** - P_A' = X_A P_A - P_B = 0 - P_S = P_A' + P_B - P_S = P_AX_A + 0 - P_S = P_AX_A - **Ideal solution:** The solution on which obeys Raoult's law is called Ideal solution → PA = PAXA, PB= PRXBPAT PAXB; PB=PBXB - **Non-Ideal solution:** The solution which obey Raoult's law is called Non-Ideel soth - **Case II of Raoult's law:** - Liquid-solid solution - Solvent solution (non valatile) - Volatile solute (volatile) - **Statement:** At constant temp. vop of solution is directly proportional to mole Fraction of solvent in solution. - **If observe U.p > calculated up then solution shows positive deviation from Rault's law.** - **If obs- u.p< colou--- show negative deviation from Rault's law.** - **Let: volatile solvent = A** - ** non-volatile solvent = B** - **Mole Fraction of A = X_A** - **Mole Fraction of B = X_B** - **Vapour pressure of pure A: P_A** - **v.p of A in solution: P_A'** - **V.p of solu = P_S** - **Alic to Raoults law:** - P_A' = X_A P_A - P_B = 0 - P_S = P_A' + P_B - P_S = P_AX_A + 0 - P_S = P_AX_A - **or** - **solute solute < solute** - **solvent solvent solvent solute > solvent** - **Interaction Solvent Solvent** - **Interaction Interfum** - **Volume increases after mixing of solution** - **AH = +ve** - **Mixing = +ve** - **Volume decrease after mixing of solution** - **AH = -ve** - **Mixing = -ve** - **eg: ** - CH₃Cl₃ = +ve - C₆H₆ = +ve - CH₃Cl₃ + C₆H₆ = -ve - **Azeotropic mixture:** Mixture of two liquid having same composition in liquid and vapour pressure and boil at same temp. is called Azeotropic mixture. - **eg. HCl+ H₂O (20.2%), HNO₃+H₂O(68%)** - **Types of Azeotropic mixture** - **Minimum boiling point Azeotropic mixture** - **Maximom boiling point Azeotropic mixture** - **The properties dilute soln which depends on conc. of solute partick is called collegative properties.** ### Types of collegative properties: - **Relative lowering of vop** - **Elevation in boiling point** - **Depression in Freezing point** - **osmotic presscure** - **Q. What is Relative lowering of vop? ** - **Aw The ratio of lowering of vip and vop of pure solvent is called Relative lowering of vib** - **PA-PS Relative lowering of up** - **POA** - **Q. What is Roulls law of Relative lowering of vop? ** - **The Relative lowering of up is equal to mole fraction of non-volatile solute** - **PA-PS = X_B** - **PA** - **PA-PS = Lowering of uop** - **PA-PS = Relative Rawering of v.p** - **PA** - **X_B = Mole fraction of v.p** - **Q. Relative lowering of vip is ^.p?** - **Alc. to Roults low of Relative lowering of usp** - **PA-PS/PA = X_B = n_B/n_A + n_B** - **Here Relative lowering of vop depend on moles od solute present in solution so it is the coligative property.** - **How can you Determine mole mass of non volatile solute by Relative: lowering of vip '11 Roults law?** - **Let: volatile solute = [A] & Non volatile solute = [B]** - **Molecular,mass of solute (PA)** - **Mass of solule = (WWB)** - **Molecular mass of schent = (Ma)** - **Mass of solvent = (WA)** - **V.p:of Bolution = (ps)** - **Ale to Roolt's law of Relative lowering of vapoure pressure. ** - **PA-PS = X_Bn_B /n_A + n_B** - **PA** - **Solution is dilute so n_A + n_B ≈ n_A** - **PA = n_A*PA** - **PA = n_A*PS** - **PA-PS = MB*X_B*WA** - **PA*WA = MB*X_B*MA** - **MB = PA*WB/X_B*MA** - **By putting lenovon data we can get molecular mass of non volatile solure. ** - **Note: Elevation in boiling point** - **Relative lowering of vip is measured by astwald any wy/ker method.** ### Elevation in boiling point - **What is elevation in boiling point?** - **Ay. The difference blow boiling point of solution and boiling point of soluent is called elevation in boiling point.** - **ΔT_b = Elevation in boiling point** - **T_b = Boiling point of solution.** - **T_o = Boiling point of solvent.** - **When non-volatile solute is added to solvent boiling point of solution Increases why? (BSEB)** - **On adding non-volatile solute, v.p of soln decreases. Now to make v.p of solution equal to 1 atm more and more heat is required so boiling point of solution Increase. ** - **What is Rault's law of ElBPY?** - **For dilute solution elevation in boiling point is directly propor to molality of solution.** - **ΔT_b = K_b m** - **ΔT_b = Kb*M** - **Here, ΔT_b= elevation in Boiling point, K_b= Molal elevation Constant (Kb), M = molality of Solution.** - **Molat elevation Constant (kh)** - **# Elevation in boiling point for I mobl Solution is called molal elevation Constant It is denoted by kb** - **Unit of kb:- k/m, k/mol, k/kg** - **ΔT_b = Kb x moles of solute /mass of solvent (leg)** - **ΔT_b = Kb x Gimimass of solute X1000 / Molecular muss of solute xmass of Sohent** - **ΔT_b = Kb x W_B x 1000 / M_B x W_A** - **M_B = Kb x W_B x 1000 / ΔT_B x W_A** - **By putting brown data we get M_B - At Sol. ** - **Note: Elevation in boiling point is measured by landsberger method.** - **Elevation to bolling point is colpative bouberty why?** - **Ale to Raoullis law for elevation in boiling point ** - **ΔT_h α moles of solute / Mass of soluent ** - **Here, elevation in boiling point depends on moles of solute present in 1g of solvent so iti's collegative property.** - **Q. How can you determine molecular mass of non-volatile solute by elevation in bp?** - **How can you relate molecular mass of volattle Soufe and alevation in b.p?** - **Let: volatile solvent = A & Non volatile solvent = B** - **Molecular mass of solute = M_B** - **Mass of solute = W_B** - **Mass of solvent = W_A** - **Alc to Raoult's law for elevation in boiling bomt: ** - **ΔT_b = K_bM, ΔT_b = K_b x moles of solute/Mass of solvent (leg), ΔT_b = Kb x Gimimass of solute X1000 / Molecular muss of solute xmass of Sohent, ΔT_b = Kb x W_B x 1000 / M_B x W_A, M_B = Kb x W_B x 1000 / ΔT_B x W_A** ### Depression in Freezing point - **What is Freeting point?** - **Ave. The demp. of which uop of Solid becomes equal to uop of ligourd is called Freering point.** - **What is Depression in Freering point?** - **The difference blew Freezing point of pure soluent and freezing point of coln is called Depression in Freering point.** - **ΔT_f = P_f-T_f** - **Here, ΔT_f= Depression in F.p.** - **P_f = Freezing point of pure Sohee** - **T_f = Freezing point of soln.** - **Q3. On addition of non-volatile solute Freezing point of solution decreates why?** - **On adding of non-volatile solute in solvent vapour pressure of Solution decreases. Now vip of liquid solvent becomes equal to vop of solid solvent at low temp. so the freezing point of solution decreases.** - **[ΔT_f = T_s-T_f]** - **Here, ΔT_f = Depression in freezing point** - **T_s = freezing point of bure Solunt** - **T_f = freezing point of solution.** - **Depression in Freezing point is collegtive property winy?** - **Ale to Raoult's law for Depression in freezing point** - **ΔT_f = k_fxM, ΔT_f = k_f * moks of solute/mass of soluent (og).** - **Here, Depression in freezing point depends on molality i'e moes of Solute of solute present I lay Soluendo it's called collegatiue property** - **Q. How can you Determine molecular mass of non-volatile solute by Depression in freeing paintor, for?** - **How can you relate molecular mass of non-volatile solute and depression in freezing polud?** - **Ay-let, Volatile solute = A, Non volatile solute = B. Molecular mass of solute = MB, Mass of solute = INB, Mass of soluent = WA. Alc to Raoult's law for Depression in Freezing point: ΔT_f = K_fXm. ΔT_f = Kf x mole of solute. Mafs of Solvent