Chemistry Atoms First2e
2nd Edition
ISBN: 9781947172647
Author: OpenStax
Publisher: OpenStax College
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Textbook Question
Chapter 15, Problem 89E
Calculate the equilibrium concentration of Zn2+ in a solution initially with 0.150 M Zn2+ and 2.50 M CN-.
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If 316.0 mg of AgBr is completely dissolved in 144.0 mL of 0.12 M NH3, what is the equilibrium concentration of Ag+(aq) in the final solution? Kf[Ag(NH3)2+] = 1.7E7Include at least 3 significant figures in your answer
If 316.0 mg of AgBr is completely dissolved in 144.0 mL of 0.12 M NH3, what is the equilibrium concentration of Ag+(aq) in the final solution? Kf[Ag(NH3)2+] = 1.7E7
Include 3 significant figures
4. If 283.0 mg of AgBr is completely dissolved in 143.0 mL of 0.2 M NH3, what is the equilibrium concentration of Ag* (aq) in the final solution?
K[Ag(NH3)2] = 1.7E7
Include at least 3 significant figures in your answer.
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5. The acid ionization constant of Fe(H₂O)2+ (aq) is 3E-6. Compute the pH of a 0.11 M aqueous solution of Fe(NO3)2-
Include at least 3 significant figures in your answer. D
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6. Compute the solubility of Mg(OH)2 in a buffer solution at pH=10.71. The solubility product of magnesium hydroxide is 1.2E-11
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Chapter 15 Solutions
Chemistry Atoms First2e
Ch. 15 - Complete the changes in concentrations for each of...Ch. 15 - Complete the changes in concentrations for each of...Ch. 15 - How do the concentrations of Ag+ and CrO42- in a...Ch. 15 - How do the concentrations of Pb2+ and S2- change...Ch. 15 - What additional information do we need to answer...Ch. 15 - Which of the following slightly soluble compounds...Ch. 15 - Which of the following slightly soluble compounds...Ch. 15 - Write the ionic equation for dissolution and the...Ch. 15 - Write the ionic equation for the dissolution and...Ch. 15 - The Handbook of Chemistry and Physics...
Ch. 15 - The Handbook of Chemistry and Physics...Ch. 15 - Use solubility products and predict which of the...Ch. 15 - Assuming that no equilibria other than dissolution...Ch. 15 - Assuming that no equilibria other than dissolution...Ch. 15 - Assuming that no equilibria other than dissolution...Ch. 15 - Assuming that no equilibria other than dissolution...Ch. 15 - Assuming that no equilibria other than dissolution...Ch. 15 - Explain why the changes in concentrations of the...Ch. 15 - Explain why the Changes in concentrations of the...Ch. 15 - Calculate the solubility of aluminum hydroxide,...Ch. 15 - Refer to Appendix J for solubility products for...Ch. 15 - Most barium compounds are very poisonous; however,...Ch. 15 - Public Health Service standards for drinking water...Ch. 15 - Perform the following calculations: (a) Calculate...Ch. 15 - The solubility product of CaSO42H2O is 2.4105....Ch. 15 - Assuming that no equilibria other than dissolution...Ch. 15 - Assuming that no equilibria other than dissolution...Ch. 15 - The following concentrations are found in mixtures...Ch. 15 - The following concentrations are found in mixtures...Ch. 15 - Which of the following compounds precipitates from...Ch. 15 - Which of the following compounds precipitates from...Ch. 15 - Calculate the concentration of Tl+ when TICl just...Ch. 15 - Calculate the concentration of sulfate ion when...Ch. 15 - Calculate the concentration of Sr2+ when SrF2...Ch. 15 - Calculate the concentration of PO43- when Ag3PO4...Ch. 15 - Calculate the concentration of F- required to...Ch. 15 - Calculate the concentration] of Ag+ required to...Ch. 15 - What [Ag+] is required to reduce [CO32-] to...Ch. 15 - What [F-] is required to reduce [Ca2+] to 1.0104M...Ch. 15 - A volume of 0.800 L of a 2104 -M Ba(NO3)2 solution...Ch. 15 - Perform these calculations for nickel(II)...Ch. 15 - Iron concentrations greater than 5.4106 M in water...Ch. 15 - A solution is 0.010 M in both Cu2+ and Cd2+. What...Ch. 15 - A solution is 0.15 M in both Pb2+ and Ag+. If Cl-...Ch. 15 - What reagent might be used to separate the ions in...Ch. 15 - A solution contains 1.0105 mol of KBr and 0.10 mol...Ch. 15 - A solution contains 1.0102 mol of Kl and 0.10 mol...Ch. 15 - The calcium ions in human blood serum are...Ch. 15 - About 50% of urinary calculi (kidney stones)...Ch. 15 - The pH of normal urine is 6.30, and the total...Ch. 15 - Magnesium metal (a component of alloys used in...Ch. 15 - Hydrogen sulfide is bubbled into a solution that...Ch. 15 - Perform the following calculations involving...Ch. 15 - Calculate the molar solubility of AgBr in 0.035 M...Ch. 15 - How many grams of Pb(OH)2 will dissolve in 500 mL...Ch. 15 - Use the simulation...Ch. 15 - How many grams of Milk of Magnesia, Mg(OH)2 (s)...Ch. 15 - Two hypothetical salts, LM2 and LQ, have the same...Ch. 15 - Which of the following carbonates will form first?...Ch. 15 - How many grams of Zn(CN)2(s) (117.44 g/mol) would...Ch. 15 - Even though Ca(OH)2 is an inexpensive base, its...Ch. 15 - Under what circumstances, if any, does a sample of...Ch. 15 - Explain why the addition of NH3 or HNO3 to a...Ch. 15 - Calculate the cadmium ion concentration, [Cd2+],...Ch. 15 - Explain why addition of NH3 or HNO3 to a saturated...Ch. 15 - Sometimes equilibria fur complex ions are...Ch. 15 - Using the value of the formation constant for the...Ch. 15 - Using the dissociation constant, Kd=7.81018,...Ch. 15 - Using the dissociation constant, Kd=3.41015,...Ch. 15 - Using the dissociation constant, Kd=2.21034,...Ch. 15 - Using the dissociation constant kd=1*10-44...Ch. 15 - Calculate the mass of potassium cyanide ion that...Ch. 15 - Calculate the minimum concentration of ammonia...Ch. 15 - A roll of 35-mm black and white photographic film...Ch. 15 - We have seen an introductory definition of an...Ch. 15 - Write the Lewis structures of the reactants and...Ch. 15 - Write the Lewis structures of the reactants and...Ch. 15 - Using Lewis structures, write balanced equations...Ch. 15 - Calculate [HgCl42-] in a solution prepared by...Ch. 15 - In a titration of cyanide ion, 28.72 mL of 0.0100...Ch. 15 - What are the concentrations of Ag+, CN-, and...Ch. 15 - In dilute aqueous solution HF acts as a weak acid....Ch. 15 - The simplest amino acid is glycine, H2NCH2CO2H....Ch. 15 - Boric acid, H3303, is not a Bronsted-Lowry acid...Ch. 15 - A saturated solution of a slightly soluble...Ch. 15 - Calculate the equilibrium concentration of Ni2+ in...Ch. 15 - Calculate the equilibrium concentration of Zn2+ in...Ch. 15 - Calculate the equilibrium concentration of Cu2+ in...Ch. 15 - Calculate the equilibrium concentration of Zn2+ in...Ch. 15 - Calculate the Fe3+ equilibrium concentration when...Ch. 15 - Calculate the CO2+ equilibrium concentration when...Ch. 15 - Calculate the molar solubility of Sn(OH)2 in a...Ch. 15 - Calculate the molar solubility of Al(OH)3 in a...Ch. 15 - What is the molar solubility of CaF2 in a 0.100-M...Ch. 15 - What is the molar solubility of BaSO4 in a 0.250-M...Ch. 15 - What is the molar solubility of Tl(OH)3 in a...Ch. 15 - What is the molar solubility of Pb(OH)2 in a...Ch. 15 - A solution of 0.075 M CoBr2 is saturated with...Ch. 15 - A 0.125-M solution of 0.075 Mn(NO3)2 is saturated...Ch. 15 - Both AgCl and Agl dissolve in NH3.. (a) What mass...Ch. 15 - The following question is taken from a Chemistry...Ch. 15 - Which of the following compounds, when dissolved...Ch. 15 - Which of the following compounds, when dissolved...Ch. 15 - What is the effect on the amount of solid Mg(OH)2...Ch. 15 - What is the effect on the amount of CaHPO4 that...Ch. 15 - Identify all chemical species present in an...
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- A volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?arrow_forwardCalculate K for the reactions in Question 2.arrow_forwardA few drops of each of the indicators shown in the accompanying table were placed in separate portions of a 1.0-M solution of a weak acid, HX. The results are shown in the last column of the table. What is the approximate pH of the solution containing HX? Calculate the approximate value of Ka for HX. Indicator Color of Hln Color of ln pKa of Hln Color of 1.0 M HX Bromphenol blue Yellow Blue 4.0 Blue Bromcresol purple Yellow Purple 6.0 Yellow Bromcresol green Yellow Blue 4.8 Green Alizarin Yellow Red 6.5 Yellowarrow_forward
- Calculate the molar solubility of Sn(OH)2 in a buffer solution containing equal concentrations of NH3 and. NH4+.arrow_forwardUnder what circumstances, if any, does a sample of solid AgCl completely dissolve in pure water?arrow_forwardA solution is 1.5 104 M Zn2 and 0.20 M HSO4. The solution also contains Na2SO4. What should be the minimum molarity of Na2SO4 to prevent the precipitation of zinc sulfide when the solution is saturated with hydrogen sulfide (0.10 M H2S)?arrow_forward
- Calculate the molar solubility of AgBr in 0.035 M NaBr (KSP=51013).arrow_forwardCalculate the solubility of aluminum hydroxide, Al(OH)3, in a solution buffered at pH 11.00.arrow_forwardSolid silver iodide, AgI, can be dissolved by adding aqueous sodium cyanide. Calculate Knet the following reaction. AgI(s)+2CN[Ag(CN)2](aq)+I(aq)arrow_forward
- Which metal sulfides can be precipitated from a solution that is 0.01 M in Mn2+, Zn2+, Pb2+ and Cu2+ and 0.10 M in H2S at a pH of 1.0? Explain.arrow_forwardCalculate the pH for a solution that contains 3.0*10-3M CsOH (aq)arrow_forwardA volume of 50 mL of 1.8 M NH3 is mixed with an equal volume of a solution containing 0.95 g of MgCl2. What mass of NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2?arrow_forward
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