Suppose this reaction occurs in a 100.00 mL solution with an initial Al3 + concentration of 1.50x10-3 mol / L. How many moles of urea must be hydrolyzed to supply enough hydroxide to stoichiometrically combine Al3 + and form the precipitate Al (OH) 3?

A) A student completely dissolves 5.16 mol of Ca(OH)2 in water. i) Which equation is the dissociation equation for Ca(OH), in water? (Give the letter choice)| A. Ca(OH) 2 (s) + H 20 ---> CaO(aq) + O 2 (g) + 2 H 2 (g) С. Са(ОН) 2 (s) --> Са 2+ (aq) + 20 2- (aq) + 2H * (aq) В. Cа(ОН) 2 (s) ---> Са 2" (аq) + 2 ОН (аq) D. Ca(ОН) 2 (s) --> CаН 2 (aq) + O 2 (g) ii) How many total moles of ions are released from the 5.16 mol of Ca(OH)2 ? mol of ions B) A sample of FeCl3 is completely dissolved in water. i) Which is the dissociation equation for FeCl3 in water? (Give the letter choice) A. FeCl 3 (s) + H 20 ---> FeCl 2 (aq) + HCI(aq) + OH (aq) C. FeCl (s) ---> Fe 3+ (aд) + Cl 2 (aq) + Cl (aq) 3 В. FeCl 3 (s) + Н20 ---> FEHCI (aq) + ОН " (aq) D. FeCl 3 (s) ---> Fe 3+ (ад) + 3 CI (аq) ii) How many total moles of ions are released if 5.71 x1019 formula units of FeCl3 were completely dissolved? (NOTE: Write answer in sci. notation using "E" or "e" to replace "x 10" & do NOT leave any space between…

Suppose a 250. mL flask is filled with 0.80 mol of SO, and 1.5 mol of SO3. This reaction becomes possible: 3' 2S0,(g) +02(g) = 2SO;(g) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of O,. You can leave out the M symbol for molarity. so, so, 2. initial change equilibrium

An aqueous solution of 0.1 M H2SO4(aq) is added to 0.1 M Na2S(aq) and is allowed to react. From the following, select all of the statements that are true.     The product of the reaction will have a colored supernatant     The product of the reaction will have a colorless supernatant     The reaction will produce water as a product     The reaction will produce a precipitate     The reaction will produce a gas     The reaction will result in an oxidation and/or reduction of one of the reactants

When aqueous solutions of AgNO3 and NaCl are mixed together, the precipitate that will form is Solubility of KCl at 20 oC is 34 g/100 g H₂O. A solution containing 20 g of KCI in 50 g of water at 20 oC is classified as solution. NH3 will dissolve in water because NH3 is a solvent. solute. CCl4 is insoluble in water because water is a

A titration of a 0.7879g sample potassium hydrogen phthalate, KHP (GFW= 204.23g/mole), required 21.25 mL of sodium hydroxide solution to reach the end point. What is the molarity of the solution?

Suppose a 250. mL flask is filled with 1.3 mol of SO, and 1.6 mol of SO3. This reaction becomes possible: 250,(3) +0,(g) = 2so,(3) Complete the table below, so that it lists the initial molarity of each compound, the change in molarity of each compound due to the reaction, and the equilibrium molarity of each compound after the reaction has come to equilibrium. Use x to stand for the unknown change in the molarity of 0,. You can leave out the M symbol for molarity. so, 0, so, initial change equilibrium

the number of moles of Aluminum in 1.3741 g was calculated to be 0.051 moles and that the chemistry student weighed out.  For every mole of Aluminum that you start with, you can create one mole of Alum [KAl(SO4)2 ⋅12 H2O(s)].  What is the theoretical yield before drying the Alum precipitate?

Consider the reaction: HCI(aq) + NH, (ag) – NH,Cl(aq) Where 20.00 mL of 0.100 M NH, (aq) is added to 10.00 mL of 0.200 M HCl(aq). Order the solution components (excluding water) from highest to lowest concentration. O [OH¯] > [NH3] > [Na*] > [Cl¯] > [H,O*] O (CI ] = [NH†] > [NH,] = [H,O*]> [OH¯] O [H,0*)> [Cl¯] > [NH,] > [NH†]> [OH) O [NH]= [OH"] > [H,O*] = [CI¯] > [NH,] O [H,0*] = [CI¯] > [NH,] > [NH ] = [OH] O [NH,CI] = [NH,] = [HCl] O [CI] > [NH†]> [H,O+] > [NH,] > [OH ] O INH,CI] > [NH3] > [HCl] O None of these

A solution contains one or more of the following ions: Ag+, Ca²+, and Cu²+. When sodium chloride is added to the solution, no precipitate forms. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered off and sodium carbonate is added to the remaining solution, producing a precipitate.