Calculate the number of milliliters of 0.766 M
Ba(OH)2 required to precipitate all of
the Cr3+ions in 151 mL
of 0.486 M CrBr3
solution as Cr(OH)3. The equation for
the reaction is:
2 CrBr3(aq) +
3 Ba(OH)2(aq)
2
Cr(OH)3(s) + 3
BaBr2(aq
Calculate the number of milliliters of 0.766 M Ba(OH)2 required to precipitate all of the Cr3+ions...
Calculate the number of milliliters of 0.440 M Ba(OH)2 required to precipitate all of the Fe3+ ions in 119 mL of 0.764 M FeCl3 solution as Fe(OH)3. The equation for the reaction is: 2FeCl3(aq) + 3Ba(OH)2(aq) —>2Fe(OH)3(s) + 3BaCl2(aq) ml Ba(OH)2
Calculate the number of milliliters of 0.433 M
Ba(OH)2 required to precipitate all of
the Fe3+ ions in 156
mL of 0.487 M
Fe2(SO4)3
solution as Fe(OH)3. The equation for
the reaction is:
Fe2(SO4)3(aq) +
3Ba(OH)2(aq) 2Fe(OH)3(s)
+ 3BaSO4(aq)
_______ mL Ba(OH)2
Calculate the number of milliliters of 0.664 M Ba(OH)2 required to precipitate all of the Al3+ ions in 154 mL of 0.408 M AlCl3 solution as Al(OH)3. The equation for the reaction is: 2AlCl3(aq) + 3Ba(OH)2(aq) 2Al(OH)3(s) + 3BaCl2(aq) _____mL Ba(OH)2
Calculate the number of milliliters of 0.687 M Ba(OH)2 required to precipitate all of the Mg2+ ions in 196 mL of 0.499 M MgSO4 solution as Mg(OH)2.
Calculate the number of milliliters of 0.648M KOH required to precipitate all of the Fe2+ ions in 169 mL of 0.536 M FeBr2solution as Fe(OH)2. The equation for the reaction is: FeBr2(aq) + 2KOH(aq) = Fe(OH)2(s) + 2KBr(aq) ____ mL KOH
[References Use the References to access important values if eded for this question Calculate the number of milliliters of 0.473 M Ba(OH), required to precipitate all of the N ions in 193 ml. of 0.758 M NISO solution as NKOND, The equation for the reaction is NISO (aq) + Ba(OH)2(aq) —+NI(OH),(5) Bas (aq) VT Ba(OH)2 Submit Answer Try Another Version 1 ltem attempt remaining
Consider the neutralization reaction 2 HNO, (aq) + Ba(OH),(aq) — 2H,O(1) + Ba(NO),(aq) A 0.110 L sample of an unknown HNO, solution required 42.9 mL of 0.200 M Ba(OH), for complete neutralization. What is the concentration of the HNO, solution? concentration: 0.039 Zinc reacts with hydrochloric acid according to the reaction equation shown. Zn(s) + 2 HCl(aq) — ZnCl2(aq) + H,(9) How many milliliters of 5.50 M HCl(aq) are required to react with 2.95 g of an ore containing 43.0%...
2. A precipitate is formed when 2.27 L of 0.0820 M Ba(OH)2 are mixed with 3.06 L of 0.0664 M N^2SO4 based upon the equation below Ba(OH)2(aq)Na2SO4(aq) > BaSO4(s) + 2 N2OH(aq) What is the mass of the precipitate formed from the Ba(OH)2? (Show all work) What is the mass of the prccipitatc formcd from thc Na2SO4? (Show all work) What is the limiting reactant? What is the theoretical yield of the precipitate?
4.82 (a) How many milliliters of 0.120 M HCI are needed to com- pletely neutralize 50.0 mL of 0.101 M Ba(OH)2 solution? (b) How many milliliters of 0.125 M H2SO4 are needed to neutralize 0.200 g of NaOH? (c) If 55.8 mL of a BaCl2 solution is needed to precipitate all the sulfate ion in a 752-mg sam- ple of Na2SOs, what is the molarity of the BaCl2 solution? (d) If 42.7 mL of 0.208 M HCl solution is needed...
For the reaction Ba(OH)2 (s) -- Ba2+ (aq) + 2 OH (aq) a precipitate will form if Q< K. Select one: True False Into a solution of 0.10 M KBr and 0.10 M KCYOA you add 0.050 M silver nitrate dropwise until a precipitate forms. Ksp for Ag2Cronis 9.0 x 10-12. Ksp for AgBr is 5.0 x 10-13. Which of the following will precipitate first? Select one or more: a. silver chromate b. no precipitate will form C. silver bromide...