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 about whether a precipitate will form or not.
E) No AgCl(s) will precipitate because Qsp>Ksp.
A solution is prepared in which the Ag+ ion concentration is 2.5 x 10-3 M and...
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
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)
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...
8) Calculate the following for 2.0 L solution containing [Ag+] = 0.100 M and [Pb2+] = 0.100 M. Assume no volume changes. (AgCl Ksp = 1.8 x 10-10, PbCl2 Ksp = 1.8 x 10-5). a) At what [Cl-] will each salt precipitate? b) What percent of the Ag+ has precipitated before the Pb2+ begins to precipitate? c) How much sodium chloride must be added (in grams) to precipitate a maximum AgCl before before any PbCl2 begins to precipitate?
What is the maximum concentration of Ag+ in HM 1x10-6 M) to precipitate Ag3PO4 without precipitating AgCl in a solution that is 0.005 M CI- and 0.005 M PO43-? AgCl Ksp 1.6 x 10 10 Ag3PO4 Ksp= 1.8 x 10-18
Predict Precipitation Question Consider the following equilibrium: Ag, PO, (s) 3 Ag (aq) + PO(aq) If the concentration of the Ag ion at a certain point is 6.3 x 10 M, and Ksp=9.1 x 104, will a precipitate form? - Select the correct answer below: Oyes, because Q> K yes, because Q < K no, because o> K no, because < K Predict Precipitation Question Consider the following equilibrium: Ag, PO, (s) 3 Ag (aq) + PO(aq) If the concentration...
In an ammonia solution, the silver ion, Ag, forms the colorless, but soluble diamminesilver(I) complex ion, Ag(NH3)2. If ammonia is added to a solution that contains an AgCI precipitate, the solid dissolves completely. Write a net-ionic equation for the equilibrium involved and explain the shift that takes place. Choose the best answer. AgCl(s) +2 NH3(a)Ag(NH3)2 (aa) C(aq) Adding ammonia to AgCl(s) dissolves the solid by displacing chloride ions with ammonia molecules, forming a soluble complex ion Ag (a2 NH3(aq) Ag(NH32...
2. Consider a solution of 1.3 x 10-3 M AgNO3 mixed with an equal amount of 3.2 x 10-4 M KCI. Will a precipitate form? Explain your answer. The Ksp of AgCl is 1.8 x 10-10
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-] =...
You prepare a solution by mixing 400.0 mL of 1 x 10-4 M Mg(NO3)2 and 500.0 mL of 1.00 x 10-4 M NaF. What is the observed outcome? For MgF2, Ksp = 6.4 x 10-9. A. A precipitate forms because Qsp > Ksp. B. No precipitate forms because Qsp > Ksp. C. No precipitate forms because Qsp = Ksp. D. No precipitate forms because Qsp < Ksp. E. A precipitate forms because Qsp < Ksp.