Videos
(a)
Interpretation:Whether the zinc chloride soluble in water or not is to be predicted.
Concept introduction:The solubility of any substance depends upon the solubility product and ionic product of that substance in water. If the value of the solubility product is greater than the tonic product then that substance would get soluble in water but if the value of the ionic product is greater than the solubility product then that substance would get precipitate.
(b)
Interpretation:Whether the lead(II) nitrate soluble in water or not is to be predicted.
Concept introduction:The solubility of any substance depends upon the solubility product and ionic product of that substance in water. If the value of the solubility product is greater than the tonic product then that substance would get soluble in water but if the value of the ionic product is greater than the solubility product then that substance would get precipitate.
(c)
Interpretation:Whether the lead (II) sulfate soluble in water or not is to be predicted.
Concept introduction:The solubility of any substance depends upon the solubility product and ionic product of that substance in water. If the value of the solubility product is greater than the tonic product then that substance would get soluble in water but if the value of the ionic product is greater than the solubility product then that substance would get precipitate.
(d)
Interpretation:Whether the sodium iodide soluble in water or not is to be predicted.
Concept introduction:The solubility of any substance depends upon the solubility product and ionic product of that substance in water. If the value of the solubility product is greater than the tonic product then that substance would get soluble in water but if the value of the ionic product is greater than the solubility product then that substance would get precipitate.
(e)
Interpretation:Whether the cobalt (III)sulfide soluble in water or not is to be predicted.
Concept introduction:The solubility of any substance depends upon the solubility product and ionic product of that substance in water. If the value of the solubility product is greater than the tonic product then that substance would get soluble in water but if the value of the ionic product is greater than the solubility product then that substance would get precipitate.
(f)
Interpretation:Whether the chromium (III) hydroxide soluble in water or not is to be predicted.
Concept introduction:The solubility of any substance depends upon the solubility product and ionic product of that substance in water. If the value of the solubility product is greater than the tonic product then that substance would get soluble in water but if the value of the ionic product is greater than the solubility product then that substance would get precipitate.
(g)
Interpretation:Whether the magnesiumcarbonate soluble in water or not is to be predicted.
Concept introduction:The solubility of any substance depends upon the solubility product and ionic product of that substance in water. If the value of the solubility product is greater than the tonic product then that substance would get soluble in water but if the value of the ionic product is greater than the solubility product then that substance would get precipitate.
(h)
Interpretation:Whether the ammonium carbonate soluble in water or not is to be predicted.
Concept introduction:The solubility of any substance depends upon the solubility product and ionic product of that substance in water. If the value of the solubility product is greater than the tonic product then that substance would get soluble in water but if the value of the ionic product is greater than the solubility product then that substance would get precipitate.
Want to see the full answer?
Check out a sample textbook solution
Chapter 4 Solutions
EBK CHEMICAL PRINCIPLES
- uppose you are trying to help your friend understand the general solubility rules for ionic substances in water. Explain in general terms to your friend what the solubility rules mean, and give an example of how the rules could be applied in determining the identity of the precipitate in a reaction between solutions of two ionic compounds.arrow_forwardOn the basis of the general solubility rules given in Table 7.1, predict the identity of the precipitate that forms when aqueous solutions of the following Substances are mixed. If no precipitate is likely, indicate which rules apply. mg src=Images/HTML_99425-7-16ALQ_image001.jpg alt="" align="top"/>arrow_forwardUsing the general solubility rules discussed in Chapter 7, give the formulas of live substances that would be expected to be readily soluble in water and five substances that would be expected to not be very soluble in water. For each of the substances you choose, indicate the specific solubility rule you applied to make your prediction.arrow_forward
- On the basis of the general solubility rules given in Table 7.1, predict which of the following substances are not likely to be soluble in water. Indicate which specific rule(s) led to your conclusion. :math>PbSe. BaCO3 :math>Mg(OH)2f. AlPO4 :math>Na2SO4g. PbCl2 :math>(NH4)2Sh. CaSO4arrow_forwardThe procedures and principles of qualitative analysis are coy cred in many introductory chemistry laboratory courses. In qualitative analysis, students learn to analyze mixtures of the common positive and negative ions, separating and confirming the presence of the particular ions in the mixture. One of the first steps in such an analysis is to treat the mixture with hydrochloric acid, which precipitates and removes silver ion, lead(II) ion, and mercury(I) ion from the aqueous mixture as the insoluble chloride salts. Write balanced net ionic equations for the precipitation reactions of these three cations with chloride ion.arrow_forwardWhat mass of silver chloride can be prepared by the reaction of 100.0 mL of 0.20 M silver nitrate with 100.0 mL of 0.15 M calcium chloride? Calculate the concentrations of each ion remaining in solution after precipitation is complete.arrow_forward
- Lead(II) nitrate is added to four separate beakers that contain the following: aker 1 (sodium chloride) eaker 2 (sodium hydroxide) eaker 3 (sodium phosphate) eaker 4 (sodium sulfate) ter the addition of the lead(II) nitrate solution to each beaker, in which beaker(s) will a precipitate form? Use the general solubility rules given in Table 7.1 to guide you.arrow_forwardHow many grams of precipitate are formed if 175 mL of a 0.750 M aluminum sulfate solution and 375 mL of a 1.15 M sodium hydroxide solution are mixed together?arrow_forwardummarize the simple solubility rules for ionic compounds. How do we use these rules in determining the identity of the solid formed in a precipitation reaction? Give examples including balanced complete and net ionic equations.arrow_forward
- 42. a. Fill in the following table as if it is a well plate and you are mixing two aqueous compounds at a time to see if a precipitate forms. If a precipitate is expected to form, indicate that by writing the correct formula for the precipitate in the corresponding box in the table. If no precipitate is expected to form, write “NO” in the box. CaCI2 Pb(NO3)2 (NH4)3PO4 Na2CO3 AgNO3 K2SO4 b. How do you prepare 300.0 mL of a 0.250 M CaCl2 solution using an available 2(X) M solution? Support your answer with calculations, but also make sure you describe how to prepare the solution.arrow_forwardApply Students conducted a lab to investigate limiting and excess reactants. The students added different volumes of sodium phosphate solution (Na3PO4) to a beaker. They then added a constant volume of cobalt(ll) nitrate solution (CO(NO3)2) stirred the contents, and allowed the beakers to sit overnight. The next day, each beaker had a purple precipitate at the bottom. The students decanted the supernatant from each beaker, divided it into two samples, and added one drop Of sodium phosphate solution to one sample and one drop of cobalt(ll) nitrate solution to the second sample. Their results are shown in Table 11.5. a. Write a balanced chemical equation for the reaction. b. Based on the results, identify the limiting reactant and the excess reactant for each trial.arrow_forwardBased on the general solubility rules given in Table 7.1, propose five combinations of aqueous ionic reagents that likely would form a precipitate when they are mixed. Write the balanced full molecular equation and the balanced net ionic equation for each of your choices.arrow_forward
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781285199030Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning