Concept explainers
At a certain temperature, K = 1.1 × l03 for the reaction
Calculate the concentrations of Fe3+, SCN− , and FeSCN2+ at equilibrium if 0.020 mole of Fe(NO3)3 is added to 1.0 L of 0.10 M KSCN. (Neglect any volume change.)
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Chapter 12 Solutions
Chemistry: An Atoms First Approach
- Although silver chloride is insoluble in water, it readily dissolves upon the addition of ammonia. AgCl(s)+2NH3(aq)Ag(NH3)2+(aq)+Cl(aq) a What is the equilibrium constant for this dissolving process? b Ammonia is added to a solution containing excess AgCl(s). The final volume is 1.00 L and the resulting equilibrium concentration of NH3 is 0.80 M. Calculate the number of moles of AgCl dissolved, the molar concentration of Ag(NH3)2+, and the number of moles of NH3 added to the original solution.arrow_forwardSuppose that solid AgCl and AgI are placed in 1.0 L water in separate beakers. Some, but not all, of each solid compound dissolves. In which beaker is the silver ion concentration, [Ag+], larger? Does the volume of water in which each compound dissolves affect the equilibrium concentration?arrow_forwardA saturated solution of silver oxalate. Ag2C2O4. contains 6.9 105-M C2O42 at 25 C. Calculate the Ksp of silver oxalate at that temperature, assuming that the ions do not react with water and the dissociation is complete.arrow_forward
- Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes in the initial concentrations of the common ions can be neglected. (a) AgCl(s) in 0.025 M NaCl. (b) CaF2(s) in 0.00133 M KF. (c) Ag2SO4(s) in 0.500 L of a solution containing 19.50 g of K2SO4. (d) Zn(OH)2(s) in a solution buffered at a pH of 11.45arrow_forwardSufficient sodium cyanide, NaCN, was added to 0.015 M silver nitrate, AgNO3, to give a solution that was initially 0.108 M in cyanide ion, CN. What is the concentration of silver ion, Ag+, in this solution after Ag(CN)2 forms? The formation constant Kf for the complex ion Ag(CN)2 is 5.6 1018.arrow_forwardSolubility is an equilibrium position, whereas Ksp is an equilibrium constant. Explain the difference.arrow_forward
- The solubility of silver sulfate, Ag2SO4, in water has been determined to be 8.0 g/L. What is the solubility in 0.45 M sodium sulfate, Na2SO4?arrow_forwardCrystals of AgBr can be removed from black-and-white photographic film by reacting the AgBr with sodium thiosulfate. AgBr(s)+2S2O32(aq)[Ag(S2O3)2]3(aq)+Br(aq) a What is the equilibrium constant for this dissolving process? b In order to dissolve 2.5 g of AgBr in 1.0 L of solution, how many moles of Na2S2O3 must be added?arrow_forwardAt 20 C, a saturated aqueous solution of silver acetate, AgCH3CO2, contains 1.0 g of the silver compound dissolved in 100.0 mL of solution. Calculate Ksp for silver acetate. AgCH3CO2(s)Ag+(aq)+CH3CO2(aq)arrow_forward
- For the reaction CdC2O4+4NH3(aq)Cd(NH3)42+(aq)+C2O42(aq) (a) calculate K. (Ksp for CdC2O4 is 1.5108.) (b) calculate [NH3] at equilibrium when 2.00 g of CdC2O4 are dissolved in 1.00 L of solution.arrow_forwardWrite the expression for the equilibrium constant and calculate the partial pressure of CO2(g), given that Kp is 0.25 (at 427 C) for NaHCO3(s) NaOH(s) + CO2(g)arrow_forwardWhen 1.55 g of solid thallium(I) bromide is added to 1.00 L of water, the salt dissolves to a small extent. TlBr(s)Tl+(aq)+Br(aq) The thallium(I) and bromide ions in equilibrium with TlBr each have a concentration of 1.9 103 M. What is the value of Ksp for TlBr?arrow_forward
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