5) A solution contains 1.0 x 102 mol of Kl and 0.10 mol of KCl per...
A solution is 0.10 M Cl and 0.10 M I- . Silver nitrate is slowly added to precipitate the silver halide. Ksp(AgCl) = 1.77 x 10-10; Ksp(AgI) = 8.52 x 10-17 (A) Which solid will precipitate first? (B) What will be the [Ag+ ] when the first solid begins to precipitate? (C) What [Ag+ ] is required in order to precipitate AgCl? (D) What will be the [I- ] when the AgCl starts to precipitate? (E) What percentage of the...
I need help please To a solution containing 0.15 M Ci- ion and 0.15 M Br- ion, you add some solid AgNO3. Ksp for AgCl is 1.6 * 10^-10 and for AgBr is 5.0*10^-13. the addition of solid doesn't change the total volume. a) which component AgCl or AgBr precipitates first? b) what is the concentration of the first anion to precipitate when the silver halide of the second anion starts to precipitate?
Let's say that the cell compartment for Ag+/Ag contains 100.0 mL of 1.0 M solution. Add 100.0 mL of 1.0 M NaCl to that compartment. Ksp of AgCl is 1.6 x 10^-10 so the Qsp > Ksp and solid AgCl will precipitate out of solution. This silver chloride is in equilibrium with its ions according to the Ksp equilibrium. Calculate [Ag+] (HINT: it will be very small) and then use your result to calculate the cell potential to the hundredths...
1. In which solution will aluminum hydroxide, Al(OH)3, be least soluble? The solutions are similar except that they have the following pH values: Hint: Common ion effect. Which two ions dictate acidity and basicity? a. 3 b. 7 c. 9 d. 11 2. Potassium perchlorate has a solubility product constant of 10-2. Which is true about the following solution of KClO4: [K+] = 0.01 M, [ClO4 −] = 0.01 M a. Ksp < Q and no precipitation occurs b....
The Ksp of AgCl at 25 °C is 1.6 x 10-10. Consider a solution that is 1.0 x 10-2 M in CaCl2 and 1.0 x 10-8 M in AgNO3. A. Q> Ksp and a precipitate will form. B.Q> Ksp and a precipitate will not form. OC.Q<Ksp and a precipitate will not form. D.Q<Ksp and a precipitate will form. E. The solution is saturated.
Which compound will precipitate first when solid silver nitrate (AgNO3) is slowly added to a solution containing 0.0120 M each of carbonate and chloride ions? Show your calculation to justify your answer. Assume the volume does not change appreciably when the silver nitrate is added. Ksp values: AgCl, 1.6 X 10^-10 Ag2CO3, 8.1 X 10^-12
4. A solution contains 0.018 mol each of I–, Br–, and Cl–. Use the Ksp values given below to determine how much AgCl(s) precipitates out when this solution is mixed with 200 mL of 0.24 M AgNO3. NOTE: This question isn’t as difficult as it looks. It’s really just stoichiometry. Ksp AgI = 1.5 x 10–16 Ksp AgBr = 5.0 x 10–13 Ksp AgCl = 1.6 x 10–10 A) 5.0 g B) 3.3 g C) 2.6 g D) 0.0 g...
please help me with these 2 questions A scientist adjusts the pH of a solution to prevent the precipitation of solid Fe(OH)2 in an aqueous solution of 0.0010 M Fe(CIO3)2(aq). What is his target pH? Ksp, Fe(OH), = 1.8 x 10-15 5. Solid AgNO3 is added in tiny amounts to a 1.00-L solution containing 0.10 M NaCl, 0.10 M NaBr, and 0.10 M Nal. Given: Ksp.Agci" 1.6 x 10-10, Ksp.AgBr - 5.0 X 10-13. Kapagi - 15 10-16 Which silver...
We prepare a solution with the following ion concentrations: [Ag+] = 1.0 x 10-6 M and [Cl-] = 1.0 x 10-2 M. If Ksp for AgCl = 1.8 x 10-10, determine which of the following is true. a. a precipitate forms b. a precipitate does not form c. the system is at equilibrium d. not enough information is given to decide
41 A solution is made 0.10 molar in Mo2+, 0.10 molar in NH3, and 1.0 molar in NH,CI. ill Mg(OH)2 precipitate? 42 How many grams of ammonium chloride must be added to 100 ml of 0.050-molar ammonium hydroxide to revent the precipitation of ferrous hydroxide, Fe(OH)2, when the NH4CI- NH4OH mixture is added to 100 ml of 0.020-molar FeCl2? Assume that the addition of solid NH4Cl produces no volume change 43 The Ksp of calcium phosphate, Ca3(PO4)2, is 1.3 X...