Molarity = moles of solute(CuSO4)/volume of solution(Liters)
0.967 grams CuSO4 (1 mole CuSO4/159.62 grams) = 0.00606 moles CuSO4
Molarity = 0.00606 moles/0.020 liters
= 0.303 Molarity
First, calculate the moles of CuSO4 in the residue using its molar mass. Then, using the volume of the original solution, calculate the molarity by dividing the moles by the volume in liters (20.0 mL converted to liters). This will give you the molarity of the original CuSO4 solution.
Sodium chloride (NaCl) would be left behind after evaporating the solution to dryness. This is because when sodium hydroxide (NaOH) reacts with hydrochloric acid (HCl), it forms sodium chloride and water. Evaporating the water leaves behind solid sodium chloride.
Evaporating a filtrate to dryness is a physical change because it involves the phase transition of a liquid (filtrate) to a gas (water vapor) without changing the chemical composition of the substance.
The percentage of solute in the solution is calculated by dividing the mass of the solute recovered (14.3g) by the initial mass of the solution (125g) and then multiplying by 100. Percentage of solute = (14.3g / 125g) * 100 = 11.44%, or approximately 11.4%.
Crystals of sugar are obtained.
A hygrometer is commonly used to measure dryness in the air. It provides a quantitative measurement of the amount of water vapor present in the air, indicating the level of dryness or humidity.
Sodium chloride (NaCl) would be left behind after evaporating the solution to dryness. This is because when sodium hydroxide (NaOH) reacts with hydrochloric acid (HCl), it forms sodium chloride and water. Evaporating the water leaves behind solid sodium chloride.
formaldehyde
Heating a solution until all the solvent has evaporated is known as heating to dryness.
Evaporating a filtrate to dryness is a physical change because it involves the phase transition of a liquid (filtrate) to a gas (water vapor) without changing the chemical composition of the substance.
Which piece of laboratory apart it would most likely be used to evaporated E1 millimeters sample of a solution to drynes
Pure potassium nitrate can be obtained by dissolving a source of potassium nitrate, such as KNO3 crystals, in water and then filtering the solution to remove any soil or impurities. The filtered solution can then be evaporated to dryness, leaving behind pure potassium nitrate crystals.
The percentage of solute in the solution is calculated by dividing the mass of the solute recovered (14.3g) by the initial mass of the solution (125g) and then multiplying by 100. Percentage of solute = (14.3g / 125g) * 100 = 11.44%, or approximately 11.4%.
Crystals of sugar are obtained.
If 50 grams of water saturated with potassium chlorate at 23 degrees Celsius is slowly evaporated to dryness, approximately 6.5 grams of the dry salt (potassium chlorate) would be recovered. This is based on the solubility of potassium chlorate in water at that temperature.
Evaporating to dryness
Yes, you can obtain pure calcium nitrate crystals by evaporating the solution to dryness. As the water evaporates, calcium nitrate will start to crystallize out of the solution. To ensure purity, it is important to start with a pure calcium nitrate solution and use distilled water for evaporation.
drought