The solubility rules listed in table below.General Rules for Solubility of Ionic Compounds (Salts) in Water at 25 °C.1. Most nitrate (NO3¯) salts are soluble.2. Most salts of Na+, K+, and NH₂+ are soluble.3. Most chloride salts are soluble. Notable exceptions are AgCl, PbCl2, and Hg₂ Cl₂.4. Most sulfate salts are soluble. Notable exceptions are BaSO4, PbSO4, and CaSO4.5. Most hydroxide compounds are only slightly soluble.* The important exceptions are NaOH andKOH. Ba(OH)2 and Ca(OH)2 are only moderately soluble.6. Most sulfide (S²-), carbonate (CO3²), and phosphate (PO4³) salts are only slightly soluble.**The terms insoluble and slightly soluble really mean the same thing: such a tiny amountdissolves that it is not possible to detect it with the naked eye. d on the basis of the general solubility rules, which choice explains why cesium sulfate would be expected to be appreciably soluble in water.Most salts of Cs are only slightly soluble.Most sulfate salts are soluble.Most salts of Cs+ are insoluble.Most sulfate salts are insoluble.e On the basis of the general solubility rules, which choice explains why iron (II) chloride would be expected to be appreciably soluble in water.Most salts of Fe²+ are insoluble.Most chloride salts are soluble.Most salts of Fe²+ are soluble.Most chloride salts are insoluble.

Check the solubility rules given in the image and select the appropriate option for the given…

dOn the basis of the general solubility rules, which choice explains why cesium sulfate would be expected to be appreciably soluble in water. Most salts of Cs are only slightly soluble. Most sulfate salts are soluble. Most salts of Cs+ are insoluble. Most sulfate salts are insoluble. e On the basis of the general solubility rules, which choice explains why iron (II) chloride would be expected to be appreciably soluble in water. Most salts of Fe²+ are insoluble. Most chloride salts are soluble. Most salts of Fe²+ are soluble. Most chloride salts are insoluble.

dOn the basis of the general solubility rules, which choice explains why cesium sulfate would be expected to be appreciably soluble in water. Most salts of Cs are only slightly soluble. Most sulfate salts are soluble. Most salts of Cs+ are insoluble. Most sulfate salts are insoluble. e On the basis of the general solubility rules, which choice explains why iron (II) chloride would be expected to be appreciably soluble in water. Most salts of Fe²+ are insoluble. Most chloride salts are soluble. Most salts of Fe²+ are soluble. Most chloride salts are insoluble.

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...

See similar textbooks

Similar questions

In the laboratory you are given the task of separating Ba²+ and Cu²+ 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. NaI K₂SO4 K₂CO3 2. 13.
b) The solubility rules provide a qualitative assessment of what combination of ions will form a precipitate when mixed in water. However, what general statement can be made regarding the solubility of all ionic compounds? Why? c) Explain why gases dissolve less in solution when the solution is heated?
1. Lead compounds used to be used as paint pigments (lead based paints), but are now prohibited in homes because the Pb (II) ion is toxic. Which of the following compounds would yield the greatest amount of Pb (II) ions when added to the same quantity of water (assuming some undissolved solid always remains)? O PbCrO4 O PbSO4 O PbS 2. The molar solubility of mercury (II) sulfide is below. What is the Ksp? molar solubility = 2.9 × 105 %3D Enter your math answer 3. The molar solubility of lead (II) bromide is 0.56 g/L. What is the Ksp? Enter your math answer
predict if one or more precipitates will form when aqueous solutions of chromium(II) chloride (CrCl2) and silver(I) nitrate (AgNO3) are mixed.Write the formula of any precipitate that could form in one of the boxes. If a box is not needed, leave it blank. If no precipitate is predicted, leave both boxes blank. predict if one or more precipitates will form when aqueous solutions of cobalt(II) acetate (Co(CH3COO)2) and zinc sulfate (ZnSO4) are mixed.Write the formula of any precipitate that could form in one of the boxes. If a box is not needed, leave it blank. If no precipitate is predicted, leave both boxes blank.
Complete the table below by deciding whether a precipitate forms when aqueous solutions A and B are mixed. If a precipitate will form, enter its empirical formula in the last column. Does a precipitate form when A and B empirical formula of solution A solution B precipitate are mixed? ammonium sulfide copper(II) nitrate O yes O no potassium chloride ammonium nitrate O yes O no iron(II) iodide zinc sulfate O yes O no
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.
Suppose a group of volunteers is planning on building a park near a local lake.the lake is known to contain low levels of arsenic .Therefore prior to starting construction the group decides to measure the current level of arsenic in the lake.a) If a14.7cm3 Sample of lake water is found to have 168.3 gems mg Aersinic .What is concentration of arsenic in the sample in parts per billion ,assuming density of lake water is 1.00g/cm3
NaOH was standardized by titration against a standard acidic solution of potassium hydrogen phthalate (abbreviated KHP). NaOH reacts with KHP in a ratio of 1:1. 0.750 g of KHP were dissolved in 100 ml of water to prepare the standard KHP solution. a. KHP has the chemical formula C8H5KO4. Calculate its molar mass from the periodic table. b. If 25.22 ml of sodium hydroxide were required to neutralize the above prepared KHP standard solution, what is the molarity of NaOH? (Hint: first calculate the molarity of KHP standard solution). Show all your calculations.
III O Chemical Reactions Solving for a reactant in solution 3/5 B One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) → Cu(s) + FeSO4(aq) Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 200. mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 63. mg. Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 2 significant digits.