If Q K_sp, solid___ until Q = K_sp Will a precipitate {Mg(OH)_2} form when 100.0 ml...
Will a precipitate form when 100.0 mL of 4.6x10^-4M is added to 100.0 mL of 2.2x10^-4 M ? Will a precipitate form when 100.0 mL of 4.6 x 10-4 м Mg(NO3)2 is added to 100.0 mL of 2.2 x 10 M NaOH? The ion product for Mg(OH)2 is Q is Кр. Mg(OH)2 Since than precipitate from the solution
Will a precipitate form when 100.0 mL of 6.8 x 10-4 M Mg(NO3)2 is added to 100.0 mL of 1.2 x 10-4 M NaOH? The ion product for Mg(OH)2 is 1. Since Q is than Ksp, Mg(OH)2 precipitate from the solution.
(greater, less) (will,will not) Will a precipitate form when 100.0 mL of 5.2 x 10-4 M Mg(NO3), is added to 100.0 mL of 1.4 x 10-4 M NaOH? The ion product for Mg(OH), is Q is c than Since Кsp? Mg(OH)2 -- precipitate from the solution.
Will a precipitate of BaSO_3 form if solution of 10 mL 0.050 M Ba(NO_3)_2 is added to 15 mL of a 0.020 M Na_2SO_3? (K_sp = 5.0 times 10^-10) A. Yes, because Q < K B. Yes, because Q > K C. No, because Q < K D. No, because Q > K
Question 33 3 pts Will a precipitate form when 100.0 mL of 0.0010 M calcium nitrate, Ca(NO3)2 is added to 100.0 mL of 0.00050 M sodium hydroxide, NaOH? yes, a precipitate of sodium nitrate will form O yes, a precipitate of Ca(OH)2 will form O no a preciptate will not form
The solubility products for Mg(OH)_2 and Ca(OH)_2 are 8.9 times 10^-12 and 1.3 times 10^-4, respectively Suppose a solution contains both Mg^2+ and Ca^2+ ions, each at 0.10 M in concentration (a) At what pH Mg(OH)_2 starts to from a precipitate? (b) At what pH Ca(OH)_2 begins to from a precipitate? (C) What is the concentration of Mg^2+ when Ca(OH)_2 begins to from precipitate?
Assume the solubility product of Mg(OH)_2 is 1.7 times 10 -^11 at a certain temperature. What minimum OH- concentration must be attained (for example, by adding NaOH) to decrease Mg^2+ concentration in a solution of Mg(NO_3)2 to less than 1.0 times 10^-10 M. (Enter your answer in scientific notation.)
student mixes 39.0 mL of 3.32M Pb(NO_3)_2(aq) with 20.0 mL of 0.00223 M Na_2SO_4(aq). How many moles of PbSO_4(s) precipitate from the resulting solution? K_sp[PbSO_4(s)] = 2.5 times 10^-8 M^2 What are the values of [Pb^+2], [SO_4^2-], [NO_3^-], and [Na^+] after the solution has reached equilibrium at 25degreeC? [Pb^+2] = [SO_4^2-]= [NO_3^-]= [Na^+]=
Does any solid PbCI_2 form when 25 mg of NaCI is dissolved in 0.250 L of 0.12 M Pb(NO_3)_2 ? K_sp for PbCI_2 = 17 times 10^-5 A simple yes or no receives no credit. Show clearly how you determined your answer.
11. Will a precipitate form when 100.0 mL of 0.020 M Pb(NO3)2 is added to 100.0 mL of 0.020 M NaCl? (4 marks) 1 or regions com un to me aromom poucos la o masina