What happens if a solute is added to a saturated solution?   A) Nothing will happen, solute will not mix with a saturated solution. B) The added solute provides a template for the solid to begin to crystallize from solution, and a precipitate will form. C) The added solute makes the solution less saturated. D) The added solute provides a template for the gas to begin to boil from solution, and a gas will form.

HELP PLEASE! 1. because of the size of the pores of the filter paper and the small size of the precipitate, some of the product will pass through the filter paper. will the reported percent of the limiting reactant in the original salt mixture be reported as too high or too low? explain 2. the precipitate is not necessarily dry when its "dried" mass is determined. as a result, will the reported mass of the limiting reactant in the original salt mixture be too high or too low?

The mass of iron(II) carbonate that is dissolved in 125 mL of a saturated solution is __________ grams.

A. Silver Nitrate solutions are unstable and will change concentrations from week to week. Why is the silver nitrate solution unstable?

After a 5.000-g sample of concrete was dissolved, the resulting solution was found to contain 0.229g of manganese. What is the concentration of manganese in the concrete in parts per million?

You can test For the presence of chloride ions in a sample of water by adding silver nitrate AgNO3, what mass of silver chloride will precipitate from a 1.50g solution of CaCl2 of excess amount of silver nitrate is present

In your first task, you are required to prepare a 100 mL solution of sodium bicarbonate at a concentration of 0.50 M. Complete the following table and calculate the mass of sodium bicarbonate needed to prepare this solution. Molecular weight of sodium bicarbonate Required final concentration Required final volume Amount of sodium bicarbonate needed to make 1 L at 0.5 M Amount of sodium bicarbonate needed to make 100 mL at 0.5 M Mass (g) = Amount (mol) × Molecular Weight (g/mol) Value 84.01 Now that you know the amount of sodium bicarbonate in mol needed to make your solution, you can convert this value into the mass by using the molecular weight of the compound. The following equation may be helpful: Mass of sodium bicarbonate needed to make 100 mL at 0.5 M Units g/mol M (mol/L) L mol mol g In the 100 mL 0.5 M solution, how many molecules of sodium bicarbonate have been added. Hint - In 1 mole there are 6.022 × 10²³ molecules.

A silver chloride precipitate is a type of gelatinous precipitates * True False

The correct definition of the Ksp is ..... a. The product of the number of particles of the solution raised to the coefficient Cb. The product of the mole of ions in solution raised to the coefficient c. Product of the concentration of the ions in the unsaturated solution d. The product of the number of ions in the solution raised to the coefficient Ce. The product of the concentration of the saturated solution ions is raised to the co

Refer to the solubility curve below to answer this question. How many grams of NH4Cl will dissolve in 1500 g of water at 90 °C? Grams of solute per 100 g H₂O 150 140 130 120 110 100 90 80 70 60 50 40 30 20 10 K Blank 1: NH37 8 NaNO3 KCIO3. KNO3 NHẠC KCI Naci -Ce₂(SO4)3 0 0 10 20 30 40 50 60 70 80 90 100 Temperature (°C)