Consider the insoluble compound silver hydroxide, AgOH. The silver ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Ag(NH3)2*, Kf = 1.6x107. Be sure to specify states such as (aq) or (s). K =
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- Consider the insoluble compound cobalt(II) hydroxide , Co(OH)2 . The cobalt(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of Co(OH)2 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Co(NH3)62+ , Kf = 7.7×104 . Be sure to specify states such as (aq) or (s). + + K =Consider the insoluble compound silver chloride , AgCl . The silver ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of AgCl (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Ag(NH3)2+ , Kf = 1.6×107 . Be sure to specify states such as (aq) or (s). + + K =We began the chapter with an informal discussion of how the mineral fluorite (as shown) is formed. Fluorite, CaF2, is a slightly soluble solid that dissolves according to the equation: CaF2(s) ⇌ Ca2+(aq) + 2F−(aq)The concentration of Ca2+ in a saturated solution of CaF2 is 2.15 × 10–4 M; therefore, that of F– is 4.30 × 10–4 M, that is, twice the concentration of Ca2+. What is the solubility product of fluorite?
- Consider the insoluble compound cobalt(II) carbonate , CoCO3 . The cobalt(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of CoCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Co(NH3)62+ , Kf = 7.7×104 . Be sure to specify states such as (aq) or (s). + + K =For the chemical reaction that occurs when the precipitate forms, write a balanced, net-ionic equation for the reaction, and explain why the reaction is best represented by a net-ionic equation. Explain the purpose of drying and weighing the filter paper with the precipitate three times. In the filtrate solution, is [K+] greater than, less than, or equal to [NO3−] ? Justify your answer. Calculate the number of moles of precipitate that is produced in the experiment. Calculate the mass percent of I− in the tablet. In another trial, the student dissolves a tablet in 55.0 mL of water instead of 50.0 mL of water. Predict whether the experimentally determined mass percent of I− will be greater than, less than, or equal to the amount calculated in part (e). Justify your answer. A student in another lab also wants to determine the I− content of a KI tablet but does not have access to Pb(NO3)2 . However, the student does have access to 0.20 M AgNO3 , which reacts with I−(aq)…Write a balanced net ionic equation to show why the solubility of Cu(OH)2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid.Be sure to specify states such as (aq) or (s). + + K =
- Give the chemical equation for the dissociation of Mg3(PO4)2? b.) What is the molar solubility of Mg3(PO4)2? c.)What are the equilibrium concentration of the ions?Calculate the Molar Solubility at 25.0 oC of an aqueous solution of calcium phosphate, Ca3(PO4)2, given that its Ksp = 1.20 x 10–26 at 25.0 oC.Consider the insoluble compound cobalt(II) carbonate , CoCO3 . The cobalt(II) ion also forms a complex with ammonia . Write a balanced net ionic equation to show why the solubility of CoCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction.For Co(NH3)62+ , Kf = 7.7×104 . Be sure to specify states such as (aq) or (s).
- In photography, unexposed silver bromide was removed from film by soaking the film in a solution of sodium thiosulfate, Na2S2O3. Silver ion, Ag+, forms a soluble complex with the thiosulfate ion, S2O3-2, that has a formula of Ag(S2O3)2-3, and the formation of the complex causes the AgBr in the film to dissolve. The formation of the complex has a Kf of 2.0 x 10^13 while the Ksp of AgBr is 5.0 x 10^-13. How many grams of AgBr will dissolve in 125 mL of 1.20 M Na2S2O3 solution?In aqueous solution, the solubility of the alkali metal ions is given as follows: Li ˂ Na ˂ Rb˂Cs. Give reason for this trend.Carbonates, phosphates, borates, and arsenates—except those of the ammonium ion and the alkali metals—are insoluble. They tend to just be solids and not dissolve much in water. Write (on paper) the expression for the equilibrium constant for the reaction represented by the equation 3Ba2+(aq)+2PO43−(aq)⇌Ba3(PO4)2(s) The solid doesn't have a concentration, so use the number 1 in its place. Please answer the following question in the text box below. You can be brief. Is Kc > 1, Kc < 1, or Kc ≈ 1? Explain your answer. Consider: how likely is the reverse reaction? Would you expect insoluble ionic compounds to have a high or low concentration of dissolved ions at equilibrium?