Chemistry Atoms First2e2nd EditionOpenStax Publisher: OpenStax CollegeISBN: 9781947172647
Chemistry Atoms First2e
Solutions for Chemistry Atoms First2e
Problem 1E:
Complete the changes in concentrations for each of the following reactions: (a) AgI(s)Ag+(aq)+I(aq)x...Problem 3E:
How do the concentrations of Ag+ and CrO42- in a saturated solution above 1.0 g of solid Ag2CrO4...Problem 4E:
How do the concentrations of Pb2+ and S2- change when K2S is added to a saturated solution of PbS?Problem 5E:
What additional information do we need to answer the following question: How is the equilibrium of...Problem 6E:
Which of the following slightly soluble compounds has a solubility greater than that calculated from...Problem 7E:
Which of the following slightly soluble compounds has a solubility greater than that calculated from...Problem 8E:
Write the ionic equation for dissolution and the solubility product (Ksp) expression for each of the...Problem 9E:
Write the ionic equation for the dissolution and the Ksp expression for each of the following...Problem 10E:
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...Problem 11E:
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities...Problem 12E:
Use solubility products and predict which of the following salts is the most soluble, in terms of...Problem 13E:
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of...Problem 14E:
Assuming that no equilibria other than dissolution are involved, calculate the molar solubility of...Problem 15E:
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all...Problem 16E:
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all...Problem 17E:
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all...Problem 18E:
Explain why the changes in concentrations of the common ions in Exercise 15.17 can be neglected.Problem 19E:
Explain why the Changes in concentrations of the common ions in Exercise 15.18 cannot be neglected.Problem 20E:
Calculate the solubility of aluminum hydroxide, Al(OH)3, in a solution buffered at pH 11.00.Problem 21E:
Refer to Appendix J for solubility products for calcium salts. Determine which of the calcium salts...Problem 22E:
Most barium compounds are very poisonous; however, barium sulfate is often administered internally...Problem 23E:
Public Health Service standards for drinking water set a maximum of 250 mg/L (2.620103M) of SO42-...Problem 24E:
Perform the following calculations: (a) Calculate [Ag+] in a saturated aqueous solution of AgBr. (b)...Problem 25E:
The solubility product of CaSO42H2O is 2.4105. What mass of this salt will dissolve in 1.0 L of...Problem 26E:
Assuming that no equilibria other than dissolution are involved, calculate the concentrations of...Problem 27E:
Assuming that no equilibria other than dissolution are involved, calculate the concentrations of...Problem 28E:
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble...Problem 29E:
The following concentrations are found in mixtures of ions in equilibrium with slightly soluble...Problem 30E:
Which of the following compounds precipitates from a solution that has the concentrations indicated?...Problem 31E:
Which of the following compounds precipitates from a solution that has the concentrations indicated?...Problem 32E:
Calculate the concentration of Tl+ when TICl just begins to precipitate from a solution that is...Problem 33E:
Calculate the concentration of sulfate ion when BaSO4 just begins to precipitate from a solution...Problem 34E:
Calculate the concentration of Sr2+ when SrF2 starts to precipitate from a solution that is 0.0025 M...Problem 35E:
Calculate the concentration of PO43- when Ag3PO4 starts to precipitate from a solution that is...Problem 36E:
Calculate the concentration of F- required to begin precipitation of CaF2 in a solution that is...Problem 37E:
Calculate the concentration] of Ag+ required to begin precipitation of Ag2CO3 in a solution that is...Problem 40E:
A volume of 0.800 L of a 2104 -M Ba(NO3)2 solution is added to 0.200 L of 5104M Li2SO4. Does BaSO4...Problem 41E:
Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a...Problem 42E:
Iron concentrations greater than 5.4106 M in water used for laundry purposes can cause staining....Problem 43E:
A solution is 0.010 M in both Cu2+ and Cd2+. What percentage of Cd2+ remains in the solution when...Problem 44E:
A solution is 0.15 M in both Pb2+ and Ag+. If Cl- is added to this solution, what is [Ag+] when...Problem 45E:
What reagent might be used to separate the ions in each of the following mixtures, which are 0.1 M...Problem 46E:
A solution contains 1.0105 mol of KBr and 0.10 mol of KCl per liter. AgNO3 is gradually added to...Problem 47E:
A solution contains 1.0102 mol of Kl and 0.10 mol of KCl per liter. AgNO3 is gradually added to this...Problem 48E:
The calcium ions in human blood serum are necessary for coagulation (Figure 15.5). Potassium...Problem 49E:
About 50% of urinary calculi (kidney stones) consist of calcium phosphate, Ca3(PO4)2. The normal...Problem 51E:
Magnesium metal (a component of alloys used in aircraft and a reducing agent used in the production...Problem 52E:
Hydrogen sulfide is bubbled into a solution that is 0.10 M in both Pb2+ and Fe2+ and 0.30 M in HCl....Problem 53E:
Perform the following calculations involving concentrations of iodate ions: (a) The iodate ion...Problem 55E:
How many grams of Pb(OH)2 will dissolve in 500 mL of a 0.050-M PbCl2 solution (KSP=1.21015)?Problem 56E:
Use the simulation (http://openstaxcollege.org/l/16solublesalts) from the earlier Link to Learning...Problem 57E:
How many grams of Milk of Magnesia, Mg(OH)2 (s) (58.3 g/mol), would be soluble in 200 mL of water....Problem 58E:
Two hypothetical salts, LM2 and LQ, have the same molar solubility in H2O. If Ksp for LM2 is...Problem 59E:
Which of the following carbonates will form first? Which of the following will form last? Explain....Problem 60E:
How many grams of Zn(CN)2(s) (117.44 g/mol) would be soluble in 100 mL of H2O? Include the balanced...Problem 61E:
Even though Ca(OH)2 is an inexpensive base, its limited solubility restricts its use. What is the pH...Problem 62E:
Under what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water?Problem 63E:
Explain why the addition of NH3 or HNO3 to a saturated solution of Ag2CO3 in contact with solid...Problem 64E:
Calculate the cadmium ion concentration, [Cd2+], in a solution prepared by mixing 0.100 L of 0.0100...Problem 65E:
Explain why addition of NH3 or HNO3 to a saturated solution of Cu(OH)2 in contact with solid Cu(OH)2...Problem 66E:
Sometimes equilibria fur complex ions are described in terms of dissociation constants. Kd . For the...Problem 67E:
Using the value of the formation constant for the complex ion Co(NH3)62+ calculate the dissociation...Problem 68E:
Using the dissociation constant, Kd=7.81018, calculate the equilibrium concentrations of Cd2+ and...Problem 69E:
Using the dissociation constant, Kd=3.41015, calculate the equilibrium concentrations of Zn2+ and...Problem 70E:
Using the dissociation constant, Kd=2.21034, calculate the equilibrium concentrations of Co3+ and...Problem 71E:
Using the dissociation constant kd=1*10-44 calculate the equilibrium concentrations of Fe3+ and CN-...Problem 72E:
Calculate the mass of potassium cyanide ion that must be added to 100 mL of solution to dissolve...Problem 73E:
Calculate the minimum concentration of ammonia needed in 1.0 L of solution to dissolve 3.0103 mol of...Problem 74E:
A roll of 35-mm black and white photographic film contains about 0.27 g of unexposed AgBr before...Problem 75E:
We have seen an introductory definition of an acid: An acid is a compound that reacts with water and...Problem 76E:
Write the Lewis structures of the reactants and product of each of the following equations, and...Problem 77E:
Write the Lewis structures of the reactants and product of each of the following equations, and...Problem 78E:
Using Lewis structures, write balanced equations for the following reactions: (a) HCI(g)+PH3(g) (b)...Problem 79E:
Calculate [HgCl42-] in a solution prepared by adding 0.0200 mol of NaCl to 0.250 L of a 0.100-M...Problem 80E:
In a titration of cyanide ion, 28.72 mL of 0.0100 M AgNO3 is added before precipitation begins. [The...Problem 82E:
In dilute aqueous solution HF acts as a weak acid. However, pure liquid HF (boiling point = 19.5 C)...Problem 83E:
The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they...Problem 84E:
Boric acid, H3303, is not a Bronsted-Lowry acid but a Lewis acid.. (a) Write an equation for its...Problem 85E:
A saturated solution of a slightly soluble electrolyte in contact with some of the solid electrolyte...Problem 88E:
Calculate the equilibrium concentration of Cu2+ in a solution initially with 0.050 M Cu2+ and 1.00 M...Problem 89E:
Calculate the equilibrium concentration of Zn2+ in a solution initially with 0.150 M Zn2+ and 2.50 M...Problem 90E:
Calculate the Fe3+ equilibrium concentration when 0.0888 mole of K3[Fe(CN)6] is added to a solution...Problem 91E:
Calculate the CO2+ equilibrium concentration when 0.100 mole of [CO(NH3)6](NO3)2 is added to a...Problem 92E:
Calculate the molar solubility of Sn(OH)2 in a buffer solution containing equal concentrations of...Problem 93E:
Calculate the molar solubility of Al(OH)3 in a buffer solution with 0.100 M NH3 and 0.400 M NH4+.Problem 95E:
What is the molar solubility of BaSO4 in a 0.250-M solution of NaHSO4? Ka for HSO4=1.2102.Problem 98E:
A solution of 0.075 M CoBr2 is saturated with H2S([H2S]=0.10M). What is the minimum pH at which CoS...Problem 99E:
A 0.125-M solution of 0.075 Mn(NO3)2 is saturated with H2S([H2S]=0.10M). At what pH does Mns begin...Problem 100E:
Both AgCl and Agl dissolve in NH3.. (a) What mass of AgI dissolves in 1.0 L of 1.0 M NH3?. (b) VNhat...Problem 101E:
The following question is taken from a Chemistry Advanced Placement Examination and is used with the...Problem 102E:
Which of the following compounds, when dissolved in a 0.01-M solution of HClO4, has a solubility...Problem 103E:
Which of the following compounds, when dissolved in a 0.01-M solution of HClO4, has a solubility...Problem 104E:
What is the effect on the amount of solid Mg(OH)2 that dissolves and the concentrations of Mg2+ and...Browse All Chapters of This Textbook
Chapter 1 - Essential IdeasChapter 2 - Atoms, Molecules, And IonsChapter 3 - Electronic Structure And Periodic Properties Of ElementsChapter 4 - Chemical Bonding And Molecular GeometryChapter 5 - Advanced Theories Of BondingChapter 6 - Composition Of Substances And SolutionsChapter 7 - Stoichiometry Of Chemical ReactionsChapter 8 - GasesChapter 9 - ThermochemistryChapter 10 - Liquids And Solids
Chapter 11 - Solutions And ColloidsChapter 12 - ThermodynamicsChapter 13 - Fundamental Equilibrium ConceptsChapter 14 - Acid-base EquilibriaChapter 15 - Equilibria Of Other Reaction ClassesChapter 16 - ElectrochemistryChapter 17 - KineticsChapter 18 - Representative Metals, Metalloids, And NonmetalsChapter 19 - Transition Metals And Coordination ChemistryChapter 20 - Nuclear ChemistryChapter 21 - Organic Chemistry
Sample Solutions for this Textbook
We offer sample solutions for Chemistry Atoms First2e homework problems. See examples below:
More Editions of This Book
Corresponding editions of this textbook are also available below:
CHEMISTRY: ATOMS FIRST
18th Edition
ISBN: 9781947172180
Chemistry: Atoms First
1st Edition
ISBN: 9781630182151
Chemistry: Atoms First
18th Edition
ISBN: 9781938168154
Related Chemistry Textbooks with Solutions
Still sussing out bartleby
Check out a sample textbook solution.
