Which of the following is the minimum amount of moles of NaOH that must be added to a 1 L solution that contains 4.3 x 10–6 M Cd2+ for the sparingly soluble salt Cd(OH)2 (Ksp = 2.5 x 10–14) to crystallize?
Which of the following is the minimum amount of moles of NaOH that must be added...
Determine the minimum number of moles of Na2SO4 that must be added to 5.00 mL of a 2.00 x 10' M BaSO4 solution to precipitate BaSO4. Ksp (BaSO4)= 1.08 10-10 a. 1.98 x 105 mol b. 4.00 x 10'mol C. 2.70 x 10 mol d. 6.53 x 106 mol
Let us assume that Cd(OH)2(s) is completely insoluble, which signifies that the precipitation reaction with NaOH(aq) (presented in the transition) would go to completion. Cd2+(aq)+2NaOH(aq) → Cd(OH)2(s)+2Na+(aq) If you had a 0.450 L solution containing 0.0190 M of Cd2+(aq), and you wished to add enough 1.31 M NaOH(aq) to precipitate all of the metal, what is the minimum amount of the NaOH(aq) solution you would need to add? Assume that the NaOH(aq) solution is the only source of OH−(aq) for the...
Question 30 (2.5 points) How many moles of Ca(NO3)2 must be added to 1.0 L of a 0.203 MKF solution to begin precipitation of CaF2? For CaF2, Ksp = 4,0 10-11 4.9 x 10-16 02x10-10 O 16 x 10-12 09.7x10-46 3.1 10-6
Question 12 7 pts Given the following Ksp values, if a solution contains 0.100 M each of Cu2+, Cd2+ and Sc3+, which ion would be present in a precipitate last if NaOH is slowly added to the solution? Ksp Cu(OH)2 = 2.2 x 10-20 Ksp Ca(OH)2 = 7.2 x 10-15 Ksp Sc(OH)3 = 8.0 x 10-25 Cd2+ All three precipitate out at the same time None of them would precipitate O Scat O Cu²
Question 6 (Extra Credit Challenge): When the sparingly soluble salt lead fluoride, PbF2, is added to an acidic solution with [H+] = 1.6 x 10–4 M, the resulting concentration of [Pb2+] after the salt dissolves is determined to be 7.75 x 10–5 M. (a) Determine the equilibrium constant for the dissolving of PbF2 in an acidic solution of H3O+ and (b) given Ka = 6.8 x 10–4, use the value determined in part a to calculate the Ksp for PbF2...
What quantity (moles) of NaOH must be added to 1.0 L of 1.8 M HC2H3O2 to produce a solution buffered at pH = 4.00? Ka = 1.8×10-5
need help with all parts of question 2. thank you :) equivalence points and the pH at the half equivalence points for the three titration regions. Question 2 Part A Given the Ksp = 2.0 x 10-29 for the sparingly soluble salt, calcium phosphate (Ca3(PO4)2), determine the molar solubility of the salt in a solution that is 0.20 M in calcium perchlorate, Ca(C104)2. Part B The cation, Co2+, is able to form a complex ion, (Co(SCN)4] 2-, with the thiocyanate...
3. Insoluble metal hydroxides can be used as a "buffer" to resist changes in pH. For example, consider the solution that would sul if 0.200 moles of MgCl2 are combined wih0.200 moles of NaOH in a total volume of 1.00 liter a) Determine the concentrations of all ionic species in this solution b) Calculate the pH of this solution c) You could add 0.040 moles of NaOH to the solution in part (a), causing additional Mg(OH)2 to precipitate. Calculate the...
12. What is the solubility (in moles/L) of Cuci in a solution that also contains 0.020 M CUNO; (the latter is fully soluble). (Ksp Cuci - 1.0 x 10-)
a) What molarity of NaOH can be added to a solution of 1.5 x 10-4M Mn(NO3)2, given the Ksp of Mn(OH)2 = 1.6 x 10-13 b) Use equilibrium equations to explain why Cu(Cl)2 is more soluble in a solution of sodium cyanide than in pure water, given that it forms the complex ion Cu(CN)42-.