1) Will a precipitate form when 0.150 L of 0.10 M Pb(NO3)2 and 0.100 L of...
Pre-lab Questions for Experiment #11 1) Will a precipitate form when 0.150 L of 0.10 M PHNO The K, for Polis 1.2 x 10-)(Show your calculatio) . 100 L 0,30 M N e w Lof 1 2) Calculate whether a precipitate will form if 2.00 mL of 60 M N aredided to (Show your calculations) -1.8 x 10 and K [FeOH) - 1610) INH! 10 0 4 (Given that N oir 3) Solid silver chromate is added to pure water...
Pre-lab Ouestions for Experiment #11 Determination of the Son Produc t for a Spargely Sole Sale 1) Will a precipitate form when 0.150 Lofo OM N O, and 0.100 L of 0.20 M Nacia (The K. for PbClis 1.2 x 10-)(Show your calculations) 2) Calculate whether a precipitate will form if 2.00 mL of 0.60 MNH, are added to 1.0 L of 1 (Show your calculations) form if 2.00 mL of 0.60 M NH, are added to 1.0 L of...
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...
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?
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?...
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...
#9 and #10 Thank you solubility of the slightly soluble salt The solubility of AgCl is the same in a 1.0 M NH, solution vs. in pure water because the Ksp of AgCl is a constant at 25°C. D) 9. Calculate the molar solubity of AgBrts) in 0.500 M NH, at 25°C. Kup of AgBr is 1.8 x 10-5, K of Ag(NHs)2" is 1.7 x 10 A) 8.7 x 104 M B) 1.2x 10-3 M C) 4.2 x 10-7 M...
Part B please. Part A Silver chloride is only slightly soluble in pure water at 25 C AgCI(s) Ag (ag)+CI (aq) K-1.8 x 10 1 Calculate the concentration of Ag and Cl in a solution that is saturated with AgCl e, the system is at equilibrium and there is still solid AgCl visible). Express your answers using two significant figures, separate your answers by a comma. [Ag+],[Cl-)- 1.3×10-5 1.3×10-5 mol Li Previous An Correct Part B The addition of ammonia...
2. With the precipitate (AgCl) still present in the test tube, add aqueous ammonia. The precipitate should disappear. This means that silver chloride is soluble in ammonia solution. It is soluble because silver ion and ammonia form a complex called diamminesilver (I) chloride, [Ag(NH3)2]Cl which in solution exists as [Ag(NH)2]* and Cl ions. You could have guessed that this would have happened if you looked over the Table A values of Kr at the end of this lab (and you...
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...