Questions in 2nd slide: Will u observe a precipitate form after adding NaCl in solution w/ final concentration of 1M? Gi

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Questions in 2nd slide:
Will u observe a precipitate form after adding NaCl in solution w/ final concentration of 1M?
Give the value of the ksp after adding 1M NaCl.
I have provided a sample solution.
Two solutions of PbCl₂ are prepared. In Solution A, 0.01 g of PbCl₂ is dissolved in water to make 100 mL of solution while in Solution B, 1.00 g of PbCl2 is dissolved in water to make 100 mL of solution. Fill in the table and show your computations where they are needed. Results M of each ion in a saturated solution of PbCl₂ A. 0.01 g PbCl₂ [Pb²+] = 1.62x10² [CI] = 3.24x10-² B. 1.00 g PbCl₂ [Pb²+] = 1.62x10-² [CH] = 3.24x10-2² Calculated Kop Computations: Will you observe a precipitate form after adding NaCl in solution with a final concentration of 0.10 M? Prove your answer by showing your computations below. What is the value of the Ksp after adding 0.10 M NaCl?
What is the value of the Kap after adding 0.10 M NC? Justify your answer above Wil you observe a precipitate form after adding NaCl in solution with a final concentration of 100 M? Prove your answer by showing your computations below What is the value of the Kap after adding 1,00 M NAC the reaction PDC121) P(+ Cl(aq) is endothermic give some predictions as to what you will observe in the two solutions if you hear them and if you heat them and add NaCl stansiy
Will you observe a precipitate form after adding NaCl in solution with a final concentration of 1.00 M ? Prove your answer by showing your computations below AgCl(s) Ag (aq) Cl(aq) Initial 1.00 M Change Equilibrium 1.00+x Ksp = 1.82x10=[Ag][CH] 1.82x100x(1.00+ x) 0=x² +1.00x -1.82x100 The two roots are x,-1.8x10 and x,-1. We take the first root as the sensible answer. Thus, the solubility of AgCl in the presence of 0.1 M NaCl is 1.8x10 M. Converting this to grams. g AgCl = 1.8x101 (0.12) (14.321) -2.58x10 g