How many moles of Na2S2O3 are needed to dissolve 0.354 mol of AgBr in a 1.0 L solution if Ksp for AgBr is 3.3×10−13 and Kf for the complex ion [Ag(S2O3)2]3− is 4.7×1013?
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How many moles of Na2S2O3 are needed to dissolve 0.354 mol of AgBr in a 1.0...
How many moles of Na2S2O3 are needed to dissolve 0.65 mol of AgBr in a solution volume of 1.0 L, if Ksp for AgBr is 3.3×10−13 and Kf for the complex ion [Ag(S2O3)3−2] is 4.7×1013? Remember to use correct significant figures in your answer (round your answer to the nearest tenth).
Unexposed silver halides are removed from photographic film when they react with sodium thiosulfate (Na2S2O3, called hypo) to form the complex ion Ag(S2O3)23-. The reaction with silver bromide is: AgBr(s) + 2 S2O32- (aq) ⇌ Ag(S2O3)23- (aq) + Br- (aq) The equilibria that need to be considered are: Ag+ + 2 S2O32- (aq) ⇌ Ag(S2O3)23- (aq) Kf = 4.7 x 1013 AgBr(s) ⇌ Ag+ (aq) + Br- (aq) Ksp = 5.0 x 10-13 What mass of Na2S2O3 is required to...
In black-and-white film developing, excess AgBr is removed from a film negative with “hypo,” an aqueous solution of sodium thiosulfate (Na2S2O3), which forms the complex ion Ag(S2O3)23–. Calculate the solubility of AgBr in 0.71 M hypo. Kf of Ag(S2O3)23– is 4.7×1013 and Ksp of AgBr is 5.0×10–13 Write the overall equation for the Ksp of AgBr and then the Kf of Ag(S2O3)23 − , add the 2 equations thus multiplying the two K values. Do an ICE chart, Enter a...
A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility of calcium iodate in mol/L? (b) What are the concentrations of Ca2+ and IO3 – ion, respectively, in the saturated solution? (c) Calculate the Ksp value for Ca(IO3)2. Part b ) Silver ion, Ag+ , readily forms complex ion, Ag(S2O3)2 3– , with thiosulfate, S2O3 2– , according to the following equation: Ag+ (aq) + 2S2O3 2– (aq) ⇌ Ag(S2O3)2 3– (aq); Kf =...
How many grams of Na,s,o, are needed to dissolve 0.0607 moles of AgClin a 1.0L solution, if Kap for AgClis 1.8 x 10-10 and Ky for the complex ion is 4.7 x 1013) Report your answer with the correct number of significant figures. Provide your answer below:
How many moles of AgBr can dissolve in 1.0 L of 1.0 M NH3? AgBr (s) + 2 NH3 (aq) ? Ag(NH3)2+ (aq) + Br- (aq) Kc=8.0 x 10^-6
The solubility of AgBr in water is 5.74×10-7 M, but increases in the presence of thiosulfate ion. Calculate the solubility of AgBr when the solid is added to a solution that is 0.795 M in thiosulfate ion. For AgBr, Ksp = 3.30×10-13 and for Ag(S2O3)23-, Kf = 2.00×1013. Solubility = M
Why is the answer a? Please show all work Silver ion forms a complex ion with thiosulfate ion, Ag(S203)2, with Kr 2.8 x 1013. How much AgBr (Ksp -5.4 x 10-13) will dissolve in 1.00 L of 0.200 M Na2S,0, solution? (A) 0.089 mol (C) 0.16 mol (B) 0.10 mol (D) 0.78 mol
How many moles of solid sodium fluoride should be added to 1.0 L of a saturated solution of barium fluoride, BaF2, at 25 ∘C to raise the fluoride concentration to 0.029 mol/L ? Express your answer to two significant figures and include the appropriate units. What mass of BaF2 precipitates? You may ignore the hydrolysis of fluoride ion. [Hint: This first part of this problem is most easily solved by first writing down an electroneutrality condition. See pages 721-722 in...
ANSWER ALL PARTS 1. Determine the molar solubility of AgBr in a 0.50 M NH3 solution. The Ksp for AgBr is 5.0 x 10-13 and the Kf for Ag(NH3)2+is 1.7 x 107. 2. How many unpaired electrons are there in the Zn2+ ion in the Zn(NH3)62+ complex ion? 3. Which of the following complex ions will absorb the shortest wavelength of visible light? Ni(CN)64- Ni(NH3)62+ Ni(H2O)62+ NiCl64-