if 300. mL of 1.50 M Mg(nNO3)2 produces 400. mL of AgNO3, what is the concentration in M?
if 300. mL of 1.50 M Mg(nNO3)2 produces 400. mL of AgNO3, what is the concentration...
3. For a mixture of 12.0 mL of 0.0040 M AgNO3 and 8.0 mL of 0.0025M K CrO4, a colorimetric measurement of Cro42 in the equilibrium supernatant liquid found its concentration to be 1.50 x 10^M. Calculate the Ksp of AgzCrO4.
A 50.0-mL sample of 0.00200 M AgNO3 is added to 50.0 mL of 0.0100 MNalo3. What is the equilibrium concentration of Ag in solution? (Ksp for Ado3 is 3.0 x 10-8.) Concentration mol/L
Given the Concentration (M) being 5.39x10^-5 M, what is the concentration in mg/mL? 0.25 = 2187x + 0.1322 (0.25 – 0.1322) = 2187x .1178 = = X 2187 x = 5.386374028x10-5 ~5.39x10-5M
16. What is the limiting reactant when 1.50 g of lithium and 1.50 g of nitrogen combine to form lithium nitride, a component of advanced batteries, according to the following unbalanced equation? Li+N, — LizN 17. What is the concentration of NaCl in a solution if titration of 15.00 mL of the solution with 0.2503 M AgNO, requires 20.22 mL of the AgNO3 solution to reach the end point? AgNO3(aq) + NaCl(aq) AgCl(s) +NaNO (aq) 18. In a common medical...
70.5 mg of K3PO4 (F.W.: 212.27 g/mol) is added to 15.0 mL of 0.0500 M AgNO3 yielding 0.0980 g of precipitate Ag3PO4 (F.W.: 418.58 g/mol) What is the % yield?
A solution contains 0.60 M NH4OH and 1.50 M NH4Cl. What is the maxiumum concentration of Mg2+ that can be present in such a solution without precipitating Mg(OH)2? (Ksp for Mg(OH)2 = 9.0 x 10^12; Kb fro NH4OH= 1.8 x 10^-5)
Will a precipitate (ppt) form when 300. mL of 5.0 x 10–5 M AgNO3 are added to 200. mL of 2.5 x 10–7 M NaBr? Answer yes or no, and identify the precipitate if there is one.
Suppose that 10.00 mL HCl of unknown concentration is neutralized by 20.00 mL of a 1.50 M NaOH solution. Determine the concentration of the HCl solution 1.50 M HCI 3.00 M HCI 0.0750 M HCI 0.150 M HCI
titration: 2. If 45.0 mL of 1.50 M Ca(OH)2 are needed to neutralize 25.0 mL of HI of unknown concentration, what is the molarity of the HI? How many mL of 0.100 M NaOH are needed to titrate 20.0 mL of 0.100 M H2SO4?
if 25.00 ml of 0.275 M solution of AgNO3(aq) is mixed with 25.00 ml of 0.300 M CaCl2(aq), what will be the reaction? What is the final concentration of all of the ions after the two solutions are mixed?