Answer the following and show solution:

1. What is the molarity of 36.00% w/w commercial hydrochloric acid with the density of 1.180 g/ml

2. Compute for the molality of a 0.7 48 m kf solution with the density of 1.0 35 g/mL. the solvent is unspecified

3. Calculate the w/w% of 85.0g hexane added to 0.317 mol of decane.

4. What is the molar concentration of chloride ion in a solution that is 2.50 × 10^2 ppm Cl-

5. Determine the morality of an aqueous solution of hydrogen peroxide that is 30.0% w/w% and has a density of 1.11 g/mL

6. What is the normality of a solution prepared by dissolving 6.18 g barium hydroxide in enough distilled water to make 65 ml of solution

Which has a higher concentration in terms of parts per million – a 0.005 calcium chloride solution or a 0.005 m potassium iodide solution?

Let's tackle these questions step by step, ensuring we understand the concepts behind each calculation. We'll break down the problems and provide clear solutions for each one.

Molarity of Hydrochloric Acid

To find the molarity of a 36.00% w/w hydrochloric acid solution with a density of 1.180 g/mL, we can follow these steps:

• Step 1: Calculate the mass of the solution. Assume we have 100 g of the solution (for simplicity).
• Step 2: Determine the mass of HCl in the solution: 36.00 g of HCl (since it's 36.00% w/w).
• Step 3: Calculate the number of moles of HCl:

  Number of moles = mass (g) / molar mass (g/mol) = 36.00 g / 36.46 g/mol ≈ 0.987 moles.

• Step 4: Find the volume of the solution using density:

  Volume = mass / density = 100 g / 1.180 g/mL ≈ 84.75 mL = 0.08475 L.

• Step 5: Finally, calculate molarity:

  Molarity (M) = moles of solute / volume of solution (L) = 0.987 moles / 0.08475 L ≈ 11.64 M.

Molality of KF Solution

Next, let's compute the molality of a 0.748 m KF solution with a density of 1.035 g/mL:

• Step 1: Understand that molality (m) is defined as moles of solute per kilogram of solvent.
• Step 2: For a 0.748 m solution, this means there are 0.748 moles of KF in 1 kg of solvent.
• Step 3: To find the mass of the solution, we need to calculate the total mass of the solution using its density.

  Mass of solution = volume × density. If we assume 1 L of solution, mass = 1 L × 1.035 g/mL = 1035 g = 1.035 kg.

• Step 4: The mass of the solvent is then:

  Mass of solvent = mass of solution - mass of solute. The molar mass of KF is approximately 58.44 g/mol, so 0.748 moles = 43.73 g.

• Step 5: Therefore, mass of solvent = 1035 g - 43.73 g = 991.27 g = 0.991 kg.
• Step 6: Finally, molality = moles of solute / kg of solvent = 0.748 moles / 0.991 kg ≈ 0.754 m.

Weight/Weight Percentage of Hexane and Decane

To calculate the w/w% of 85.0 g of hexane added to 0.317 mol of decane:

• Step 1: Calculate the mass of decane. The molar mass of decane (C10H22) is approximately 142.28 g/mol.

  Mass of decane = 0.317 mol × 142.28 g/mol ≈ 45.05 g.

• Step 2: Total mass of the solution = mass of hexane + mass of decane = 85.0 g + 45.05 g = 130.05 g.
• Step 3: Calculate w/w% of hexane:

  w/w% = (mass of hexane / total mass) × 100 = (85.0 g / 130.05 g) × 100 ≈ 65.4%.

Molar Concentration of Chloride Ion

For a solution that is 2.50 × 10^2 ppm Cl^-, we can convert this to molarity:

• Step 1: Understand that 1 ppm means 1 mg of solute per liter of solution. Therefore, 2.50 × 10² ppm = 250 mg/L.
• Step 2: Convert mg to grams: 250 mg = 0.250 g.
• Step 3: Calculate the number of moles of Cl^-:

  Number of moles = mass (g) / molar mass (g/mol) = 0.250 g / 35.45 g/mol ≈ 0.00706 moles.

• Step 4: Since this is in 1 L of solution, molarity = 0.00706 moles/L = 0.00706 M.

Molality of Hydrogen Peroxide Solution

To determine the molality of a 30.0% w/w hydrogen peroxide solution with a density of 1.11 g/mL:

• Step 1: Assume we have 100 g of the solution. This means we have 30.0 g of H₂O₂.
• Step 2: Calculate the number of moles of H₂O₂:

  Number of moles = 30.0 g / 34.01 g/mol ≈ 0.882 moles.

• Step 3: Find the mass of the solvent (water):

  Mass of solvent = total mass - mass of solute = 100 g - 30.0 g = 70.0 g = 0.070 kg.

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