A solution is 5.0 x 10-5 M in each of these ions: Agt, s02-, Cl-, and...
A solution is 5.0 x 10-M in each of these ions: Ag+, so -, Cl, and co . Which precipitate will form? Ag2SO4 (Ksp = 1.12 x 10-5) AgCl (Ksp = 1.77 x 10-10 Ag2CO3 (Ksp = 8.46 x 10-12)
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...
If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Ag2CrO4 ( Ksp = 1.2×10?12), Ag2CO3 ( Ksp = 8.1×10?12), or AgCl ( Ksp = 1.8×10?10)? Problem 17.75 A solution contains three anions with the following concentrations: 0.20 M Cro 0.10 M CO and 0.010 M Cl Part A If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Aga Cro4 Ksp 1.2 x...
A solution is prepared in which the Ag+ ion concentration is 2.5 x 10-3 M and the Cl- ion concentration is 3.2 x 10-4 M. Which of the following statements is true given that the Ksp for AgCl is 1.8 x 10^-10? A)No AgCl(s) will precipitate because Qsp<Ksp. B)No AgCl(s) will precipitate because the Ksp value indicates that AgCl is infinitely soluble in water. C)A precipitate of AgCl(s) will form because Qsp>Ksp. D)Insufficient data is given to make a prediction...
5). Calculate the maximum concentration (in M) of silver ions (Ag+) in a solution that contains 0.00125 M of CO32-. The Ksp of Ag2CO3 is 8.46×10-12.
16. A solution consists of 0.1M in Br-, CO32-, and 1. Which compound will precipitate first as AgNO3 is added to the solution? What concentration of Agt is necessary to begin the precipitation of each anion? AgBr (s), Ksp = 5.35 x 10-13 Ag2CO3 (s), Ksp = 8.46 x 10-12 Agl (s), Ksp = 8.52 x 10-17
Ksp of AgCl = 1.77x10^-10 Ksp of PbCl2 = 1.70x10^-5 thanks! A solution contains 0.036 M Ag+ and 0.032 M Pb2+. If you add CI", AgCl and PbCI, will begin to precipitate. What is the concentration of Cl" required, in molarity, when AgCl precipitation begins? concentration of Cl" = What is the concentration of Cl required, in molarity when AgCl precipitation is 99.99% complete? concentration of Cl" = What is the concentration of CI required, in molarity when PbCl, precipitation...
A solution contains 0.021 M Cl? and 0.017 M I?. A solution containing copper (I) ions is added to selectively precipitate one of the ions. At what concentration of copper (I) ion will a precipitate begin to form? What is the identity of the precipitate? Ksp(CuCl) = 1.0 × 10-6, Ksp(CuI) = 5.1 × 10-12. please show work! A) 4 .8 × 10-5 M, CuCl B) 3 .0 × 10-10 M, CuI C) 3 .0 × 10-10 M, CuCl D)...
please answer all 4 SP TCalculate the molar solubility of AgBr (Ksp - 5.0 x 1013) in a 0.17 M CaBr2 solution. CaBr is 100% soluble. +2 Ca +28r 6 CaBiz 4. The following pictures represent solutions of AgCl, which may also contain ions other than Ag+ and Cl- which are not shown. Gray spheres represent Ag' ions and dotted spheres represent Cl' ions. If solution (1) is a saturated solution of AgCl, which of solutions (1-4) represents the solution...
Question 6 0 / 1.5 pts To 0.500 L 1.00 x 10-MAgNO3 solution, 5.0 x 10-6 mole of NaCl solid is added. Ksp for AgCl is 1.6 x 10-10. What is Asp of AgCl? Will AgCl form precipitate? 5.0 x 10-11, no precipitate