In saturated solution, []Ag+] = [Cl-] = 1.25 * 10^-5 M
gCl ........> Ag+ + Cl-
Ksp = [Ag+][Cl-]
or
Ksp = 1.25 * 10^-5 * 1.25 * 10^-5
or
Ksp = 1.56 * 10^-10 (answer)
A saturated AgCl solution was analyzed and found to contain 1.25 x 10-5 M Ag+ ions....
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)
Silver chloride, AgCl, is a sparingly soluble solid. Answer the following questions about a saturated solution prepared by placing solid silver chloride in a 1.94 x 10-5 M NaCl(aq) solution. At some temperature, the silver ion concentration, [Ag+], was found to be 6.24 x 10-6 M. (a) What is the concentration of chloride ions, [CI – ], in the resulting solution? XM (b) What is the molar solubility of silver chloride, AgCl, in 1.94 x 10-5 M NaCl? 4.9 6.24e-6...
1. What ions can be found in a saturated solution of Caco? The saturated solution of Ca CO₂ tochd that culcrmccartron and Carborate clos) son is as follows CaCO₃(aq)-> (a + cual tozcaada Asso Saturated solither ofcacą has cat and coz 2. What is the K, expression for a saturated solution of Ca,(PO)? (a3(PO4)2 ₃ 3 cat? tz Pou3 35 25 KSP=35] [25]? = 2753x452 - Ksp = 108 55 3. What is the K expression for a solution of...
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...
A sample solution containing sulfate ions (SO42−) was analyzed and was found to contain 2.5 mol of sulfate ions (SO42−). Calculate the equivalent of sulfate ions (SO42−) present in the soluti
A saturated solution of Ag2CO3 has a Ag+ concentration of 2.57 x 10-4 M. Calculate Ksp for Ag2CO3.
10 L of a saturated solution of calcium fluoride, CaF2, was evaporated and found to contain 4.28 millimoles (mmol) fluoride. What is the value of Ksp? CaF2(s) -> <- ca2+ (aq) +2 F- (aq) How did Ksp= [Ca2+] [F-]2 become Ksp= [s] [2s]2= 4s3 Cause I thought it was only Ksp= [s] [s]2 = s3 and why 4.28x10-3 have to devide by 10 and why the [F-] = 4.28 x 10-4 have to eqautes to 2 to have s= 2.14x10-4...
answer these please 17. The solubility of AgCl is 0.000 013 mol/L. Calculate the Ksp for AgCl. 18. If the concentration of chloride ion remaining in solution after silver chloride has been precipitated is 0.2 M, what is the concentration of the silver ion? Kap of AgCl is 2.8 X 10-10 19. What is the experimental Ksp of CaCO3 if the residue after evaporation of a 1.00 L saturated solution is found to have a mass of 0.006 90 g?...
A solution is 5.0 x 10-5 M in each of these ions: Agt, s02-, Cl-, and CO2- Which precipitate will form? AgCl (K sp = 1.77 x 10-19 Ag2CO3 (Ksp = 8.46 x 10-13) Ag2SO4 (Ksp = 1.12 x 10-5)
AgCl (s) + --> <-- Ag + (aq) + Cl- (aq) Shown above is information about the dissolution of AgCl in water at 298 K. In a chemistry lab a student wants to determine the value of s, the molar solubility of AgCl, by measuring [Ag+] in a saturated solution prepared by mixing excess AgCl and distilled water. How would the results of the experiment be altered if the student mixed excess AgCl with tap water (in which [Cl-] =...