(0.7] General solubility rule for lonic compounds in water tells us that potassium sulfate is soluble inwater while strontium sulfate is insoluble. Describe further what actually happens whenpotassium sulfate is mixed with water and becomes completely dissolved to make the aqueoussolution while the same does not happen to strontium sultate (nothing dissolved in water).

The solubility is the maximum amount of solute that can dissolve in a known quantity of solvent at a…

Answered: General solubility nule for ionic…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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How could you have used the color change property of iron(III) chloride to monitor when the reaction had reached completion? You could have added drops of iron(III) chloride directly to the reaction mixture until a change in color occurred. You could have placed a drop of iron(III) chloride directly to the reaction mixture and waited until the color disappeared. You could have placed a drop of reaction mixture every minute in one test tube containing iron(III) chloride until there was no color change. You could have placed a drop of reaction mixture into different test tubes containing iron(III) chloride every minute until there was no color change. Incorrect
A student weighs out 4.16 g of magnesium chloride and adds enough water to make 125.0 mL of solution. The student then weighs out 8.82 g of sodium phosphate and adds enough water to make 250.0 mL of solution. 25.0 mL of the magnesium chloride solution is combined with 25.0 mL of the sodium phosphate solution. a. Write a balanced equation for the reaction that occurs (remember to include phases). b. If a precipitate forms, write the name of the precipitate and calculate the theoretical yield for the precipitate. If no precipitate forms, calculate the limiting reactant. c. If the temperature of the solution decreases, is this reaction exothermic or endothermic?
Suppose 3.32g of nickel(II) iodide is dissolved in 50mL of a 0.40 M aqueous solution of potassium carbonate. Calculate the final molarity of iodide anion in the solution. You can assume the volume of the solution doesn’t change when the nickel(II) iodide is dissolved in it.
In the laboratory you are given the task of separating Ag" and Cu* ions in aqueous solution. For each reagent listed below indicate if it can be used to separate the ions. Type "Y" for yes or "N" for no. If the reagent CAN be used to separate the ions, give the formula of the precipitate. If it cannot, type "No" Y or N Reagent Formula of Precipitate if YES 1. Nal 2. NaOH 3.O K2S
Imagine you were working as a laboratory technician and your principal investigator asked you to develop Benedict’s test into a quantitative measure of the concentration of reducing sugar in a solution. To do this, you would first need to decide what to measure and then establish the relationship between your measurements and different concentrations of reducing sugars. Explain generally what you would decide to measure and how you would go about determining the relationship of your measurements to the concentration of reducing sugar.
Suppose 0.274 g of lead(II) acetate is dissolved in 100. mL of a 23.0 mM aqueous solution of ammonium sulfate. Calculate the final molarity of acetate anion in the solution. You can assume the volume of the solution doesn't change when the lead(II) acetate is dissolved in it.
b) Water "softeners" work via the principle of ion-exchange. The tank of a water softener is filled with a soluble salt such as sodium chloride. As "hard" water passes through the tank, the undesirable ions in hard water (e.g., calcium, magnesium, and iron III) are exchanged for the more desirable "soft" (meaning more soluble) ions like sodium. Explain how swapping the "soft"-water sodium ions for "hard"-water ions would influence the behavior (the cleaning effectiveness) of soaps and detergents.
2. A 0.1864 g sample of an unknown Ni(II) salt was put into solution and properly treated to form the solid nickel(II) complex (molar mass=288.917 g mol ¹). When the precipitate was rinsed, dried, and cooled, dimethylglyoxime it was determined to have a mass of 0.1165 g. Calculate the mass of nickel in the precipitate and the percent (by mass) of nickel in the original (unknown) salt sample.
A 1.00 g sample of KCl is dissolved in 38.0 mL of water. The resulting solution is then added to 56.0 mL of a 0.350 M CaCl2 (ag) solution. Assuming that the volumes are additive, calculate the concentrations of each ion present in the final solution. Concentration of K+ ions = M Concentration of Ca²+ ions = M Concentration of Cl- ions M %3D
Solid potassium hydroxide is slowly added to 75.0 mL of a chromium(III) nitrate solution until the concentration of hydroxide ion is 0.0417 M. The maximum amount of chromium(III) ion remaining in solution is M.
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Describe the process of the solubility of ionic compounds?

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