Interpretation:
The net ionic reaction for the reactions where both products are insoluble and precipitate from aqueous solution has to be written.
Concept introduction:
Balancing reaction:
Balanced reaction is a
Steps in balancing the information
- Step 1: Write the unbalanced equation
- Step 2: Find the coefficient to balance the equation.
- The coefficient should be reduced to the smallest whole number.
Precipitation reaction: The formation of the product is insoluble when the ions combine in the solution is called precipitation reaction.
Most of the ionic compounds are soluble in water, very few of the ionic compounds are sparingly soluble, and some of the ionic compounds are insoluble in water. When it is soluble in water ions gets separated in the solution.
Want to see the full answer?
Check out a sample textbook solutionChapter 3 Solutions
Chemistry: The Molecular Science
- n general terms, what are the spectator ions in a precipitation reaction? Why are the spectator ions not included in writing the net ionic equation for a precipitation reaction? Does this mean that the spectator ions do not have to be present in the solution?arrow_forwardWrite the net ionic equation for the reaction, if any, that occurs on mixing (a) solutions of sodium hydroxide and magnesium chloride. (b) solutions of sodium nitrate and magnesium bromide. (c) magnesium metal and a solution of hydrochloric acid to produce magnesium chloride and hydrogen. Magnesium metal reacting with HCl.arrow_forwardMany over-the-counter antacid tablets are now formulated using calcium carbonate as the active ingredient, which enables such tablets to also be used as dietary calcium supplements. As an antacid for gastric hyperacidity, calcium carbonate reacts by combining with hydrochloric acid found in the stomach, producing a solution of calcium chloride, converting the stomach acid to water, and releasing carbon dioxide gas (which the person suffering from stomach problems may feel as a “burp”). Write the unbalanced chemical equation for this process.arrow_forward
- In each of the following cases, does a precipitation reaction occur when solutions of the two water-soluble reactants are mixed? Give the formula of any precipitate that forms, and write a balanced chemical equation for the precipitation reactions that occur. (a) sodium carbonate and copper(11) chloride (b) potassium carbonate and sodium nitrate (c) nickel(11) chloride and potassium hydroxidearrow_forwardOn the basis of the general solubility rules given in Table 4.1, predict the identity of the precipitate that forms when the following aqueous solutions are mixed. If no precipitate forms, indicate which rules apply.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
- World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub CoChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningIntroductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning