4- (a) Calculate the concentration of Cd2+ ion in a solution prepared by mixing 2.0 mL...
QUESTION 3 A solution is prepared by mixing 30.0 mL of 0.60 M Ba(NO3)2 and 30.0 mL of 0.60 M Ca(NO3)2. Sodium fluoride is added to the mixture. Assume there is no volume change from the addition of sodium fluoride. Which compound precipitates first and at what concentration of F will we first see the precipitate form? Ksp BaF2 = 1.8 x 107 and Ksp CaF2 = 1.5 x 10-10 1. BaF2; 3.6 × 10-3M 2. CaF2; 7.2 10-4 M...
The Ksp of Cd(OH)2 is 5.9x10^-15 and the Kf of Cd(NH3)4^2+ is 1.0x10^7. Use these values to determine if Cd(OH)2 precipitate will form in a solution made by mixing 1.0 mL of 1.0M aqueous Cd(NO3)2 with 1.0 L of 5.0M aqueous NH3. The Kb for ammonia is 1.8x10^-5 Kf if K of formation. This is not given info. we’ re supposed to know this for this problem
5. A solution is made by mixing 200.0 ml of 1.5 x 10-4 M Cu(NO3)(aq) with 250.0 ml of 0.20 M NH3(aq). Calculate the concentration of copper ion (Cu? (aq)) in the solution when it reaches equilibrium. (Kr for [Cu(NH3)4]2+ = 1.7 x 1013)
What is the pH of the resulting solution if 95 mL of 0.514 M methylamine, CH3NH2, is added to 115 mL of 0.85 M HCI? Assume that the volumes of the solutions are additive. K = 2.70 x 10 for CH NH. CH:NH, (aq) + H(aq) = CH NH3(aq) | CHINH, H CHỌNH What is the pH of a solution prepared by mixing 75 ml of 0.38 M acetic acid and 50 mL of 0.58 M sodium acetate are mixed....
A solution prepared by mixing 100 mL of 0.10 M NaOH 140 mL of 0.10 M HCl 100 mL of 0.10 M NH3 has a pH of: Kb (NH3) = 1.8 x 10-5 A. 9.08 B. 4.57 C. 7.00 D. 4.92 E. 9.43
A solution of 50.0 mL of 0.045 M Ca(NO,), is prepared. What volume (in mL) of 1.90 M NaOH must be added to the calcium nitrate solution to begin to precipitate solid Ca(OH), from the solution? K = 6.5 x 10 Hint: Solid Ca(OH), will begin to precipitate at the point where an equilibrium exists between the solid and aqueous ions. The volume of NaOH required, will be very small so you don't have to consider the dilution of the...
Calculate the pH of a solution obtained by mixing 25.00 mL of 0.13 M NH3 with 25.00 mL of 5.0×10-2 M HCl. Kb for NH3 is 1.8×10-5.
Calculate the pH of a solution made by mixing 100.0 mL of 0.874 M NH3 with 100.0 mL of 0.100 M HCl. (Kb for NH3 = 1.8 10
What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 5.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3. (Select One) 10.26 or 11.13
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.