Types Of Solutions

Step 1: Δ Tf = Kf m m=(0.3)/(1.86)=0.161
Step 2: Moles required: n = 0.161 × 5 = 0.805
Step 3: Mass: m = 0.805 × 62 ≈ 50 g

Step 1: Molality calculation. m = (1/250)/(0.0512) = 0.078
Step 2: Freezing point depression. Δ Tf = Kf m = 5.12 × 0.078 ≈ 0.4

Step 1: Calculate the equivalent weight of the acid.
The number of equivalents of acid is given by:
Step 2: Use the formula for neutralization.
The amount of base required for neutralization is: The basicity (number of replaceable hydrogen ions per molecule) is 2. Thus, the correct answer is (2).

Step 1: van’t Hoff factor.
The van’t Hoff factor is greater than 1 for electrolytes that dissociate, as it represents the number of ions produced. If association occurs, the factor is less than 1 as fewer ions are formed.
Thus, the correct answer is (4).

Step 1: Formula for elevation in boiling point.
The formula for the elevation in boiling point is: where is the ebullioscopic constant, is the molality, is the mass of the solvent, and is the molar mass of the solute.
Thus, the correct answer is (1).

Step 1: Use the neutralization equation.
The neutralization of sulfuric acid and sodium carbonate can be represented by .
Step 2: Conclusion.
The required volume is 176.66 ml based on the equivalent amounts of acid and base. Final Answer:

Step 1: Use the neutralization equation.
The neutralization reaction between sodium carbonate and sulphuric acid is given by: The molar equivalents of sodium carbonate are equal to those of sulphuric acid. Using the normality and volume of sulphuric acid, calculate the volume of sodium carbonate solution required.
Step 2: Calculate the volume.
The required volume of sodium carbonate solution is calculated as 176.66 ml using the equivalence factor. Final Answer:

Step 1: Use the dilution equation.
The dilution equation is , where and are the concentration and volume of the concentrated acid, and and are the concentration and volume of the diluted solution.
Step 2: Calculate the amount of concentrated acid.
The volume of the concentrated acid required is calculated as follows:

Step 1: Understand the concept of molarity.
Molarity is given by . If equal weights of NaCl and KCl are dissolved in the same volume, the molarity will be higher for NaCl due to its lower molar mass.
Step 2: Conclusion.
The molarity of NaCl will be more than that of KCl. Final Answer:

Step 1: Equivalents of acid: N₁V₁=N₂V₂ ⟹ 0.1×20= N×25 ⟹ N=0.08
Step 2: Total equivalents in 250 mL: 0.08×10=0.8
Step 3: Equivalent weight of Na₂CO₃ =53.
Step 4: Mass of Na₂CO₃ =0.8×53=0.848g
Step 5: Percentage: (0.848)/(1.25)×100=84.8%

Step 1: 26% w/v means 26g in 100mL.
Step 2: Molar mass of NH₃ =17.
Step 3: Molarity: (26/17)/(0.1)≈15.3
Step 4: For monobasic base: N=M=15.3

Step 1: Henry’s law: p = KH x
Step 2: Raoult’s law: p = p^∘ x
Step 3: When KH = p^∘, Henry’s law reduces to Raoult’s law.

Step 1: pH = 2 ⇒ [H⁺]=10⁻2.
Step 2: Degree of ionisation: α=frac10⁻20.1=0.1
Step 3: van’t Hoff factor: i=1+α=1.1
Step 4: π=iCRT=0.11RT

Step 1: 26% (w/v) means 26g of NH₃ per 100mL.
Step 2: Mass per litre: 260g/L
Step 3: Molar mass of NH₃=17. Molarity=(260)/(17)≈15.3M
Step 4: Ammonia is a monobasic base: Normality=Molarity=15.3

Step 1: Normality relation: N₁V₁=N₂V₂ Nbase×25 = 0.1×20 ⟹ Nbase=0.08
Step 2: Total equivalents in 250mL: 0.08×(250)/(1000)=0.02
Step 3: Only Na₂CO₃ reacts. Equivalent weight of Na₂CO₃=53. Mass of Na₂CO₃=0.02×53=1.06g
Step 4: Percentage: (1.06)/(1.25)×100=84.8%

Step 1: Henry’s law: p = KH x Step 2: Raoult’s law: p = p^∘ x Step 3: When Henry’s constant equals vapour pressure of pure component: KH = p^∘ Then Henry’s law reduces to Raoult’s law.

Step 1: Understanding the Concept:
Parts per million (ppm) is a unit of concentration used for very dilute solutions. It expresses the mass of a solute present in one million ( ) parts by mass of the solution. For aqueous solutions, where the density is approximately , of solution weighs .

Step 2: Key Formula or Approach:
The formula for ppm can be expressed as: Alternatively, for dilute aqueous solutions:

Step 3: Detailed Calculation:
1. Convert mass of solute from grams to milligrams: Given mass of CaCO = Since : 2. Calculate ppm using the volume of the solution: Given Volume = Alternatively, using the mass-to-mass formula: Mass of solute = Mass of solution

Step 4: Final Answer
The concentration of the CaCO solution is 9 ppm.