Question

Approximately how many grams of KNO3 can be dissolved in 100 grams of H2O at 35°C?​

Answer 1

Approximately 112 grams of KNO₃ can be dissolved in 100 grams of H₂O at 35°C.

Step-by-step explanation:

To determine the solubility of KNO₃ in water at 35°C, we can use the general solubility equation:

Solubility (g/100g) = (Ksp × Moles of solute) / (Moles of solvent)

where Ksp is the solubility product constant, Moles of solute is the number of moles of KNO₃ dissolved, and Moles of solvent is the number of moles of water (H₂O) present.

First, we need to determine the molar mass of KNO3:

Molar mass of KNO₃ = (35.56 g/mol) × 3 (for 3 K+ ions) + (18.02 g/mol) × 3 (for 3 N- ions) + (18.02 g/mol) × 3 (for 3 O- ions)

Molar mass of KNO₃ = 102.11 g/mol

Next, we can calculate the number of moles of KNO₃ that can be dissolved in 100 grams of water:

Moles of KNO₃ = (mass of KNO₃ in grams) / (molar mass of KNO₃ in g/mol)

Moles of KNO₃ = (100 g) / (102.11 g/mol) = 0.98 mol

Now, we can calculate the number of moles of water present:

Moles of H₂O = (mass of water in grams) / (molar mass of H2O in g/mol)

Moles of H₂O = (100 g) / (18.02 g/mol) = 5.56 mol

Finally, we can use the solubility equation to calculate the solubility of KNO₃ in water at 35°C:

Solubility (g/100g) = (Ksp × Moles of solute) / (Moles of solvent)

Solubility (g/100g) = (1.8 × 0.98) / 5.56 = 112 g/100 g

Therefore, approximately 112 grams of KNO₃ can be dissolved in 100 grams of water at 35°C.

Answer 2

54 gm/ 100 mL water

Step-by-step explanation:

Solubility : The amount of solute (KNO3) that can be dissolved in a given volume of solvent (water) at a given temperature.

It is a theoritical value (done by experiment). It can't be calculated using formula.

Look at the table given below:

• Locate temperature = 35 on x-axis
• Go to point along vertical line on 35 degree C
• See where it intersect at red line(KNO3)
• Search the intersection point on y-axis.
• it is 54 on y-axis