A solution of 50.0 mL of 0.20 M H2SO4 is titrated with 1.0 M of LIOH. H₂SO4 + 2LIOH → Li₂SO4 + 2H₂O What volume of LiOH is required to neutralize the acid completely? Vol LiOH = [?] mL Hint: Be careful of the mole ratios! Vol LiOH (mL) Enter

3. In a solution containing H;O* ions at a concentration of 0.003 mol.L', what is the concentration of OH ions? a) 0.003 mol.L·'. b) 3 x 10-12 mol.L·'. c) 11.5 mol.L·'. d) 10-7 mol.L'. e) There is no OH.

A student makes a solution using the following volumes of stock solutions. mL 0.019 M Fe(NO3)3 3.37 What would the student record for the initial [Fe³+] for this solution? Solution 1 mL 0.10 M HNO3 4.00 ImL 0.036 M KSCN 6.81

A solution contains 0.036 M Ag+ and 0.031 M Pb²+. If you add Cl¯, AgCl and PbCl₂ will begin to precipitate. What is the concentration of Cl required, in molarity, when AgCl precipitation begins? concentration of Cl- = What is the concentration of Cl required, in molarity when AgCl precipitation is 99.99% complete? concentration of Cl- = What is the concentration of Cl required, in molarity when PbCl₂ precipitation begins? concentration of Cl- = What is the concentration of Cl required, in molarity when PbCl₂ precipitation is 99.99% complete? concentration of Cl- = Finally, give the Cl- concentration range in which Ag+ can be completely separated from Pb²+ by precipitation. Give the lowest CI concentration for the separation of Ag+ from Pb²+. concentration of Cl- = Give the highest Cl¯ concentration for the separation of Ag+ from Pb²+. concentration of Cl- = M M M M M M

< Question 39 of 41 The addition of 0.3800 L of 1.150M KCI to a solution containing Ag* and Pb?+ ions is just enough to precipitate all of the ions as AgCl and PbCL,. The total mass of the resulting precipitate is 62.10 g. Find the masses of PbCl, and AgCl in the precipitate. mass of PbCl,: mass of AgCl: A solution contains Al and Co. The addition of 0.3823 L of 1.654 M NAOH results in the complete precipitation of the ions as Al(OH), and Co(OH),. The total mass of the precipitate is 22.83 g. Find the masses of Al+ and Co+ in the solution. mass of Al3+. mass of Co+.

Solid potassium hydroxide is slowly added to 150 mL of a 0.0538 M iron(II) acetate solution. The concentration of hydroxide ion required to just initiate precipitation is  M.

A solution contains 7.27x103 M lead nitrate and 1.16x102 M calcium acetate. Solid ammonium sulfate is added slowly to this mixture. What is the concentration of lead ion when calcium ion begins to precipitate? [Pb2*] =| M

1. A solution contains 1.16×10-2 M potassium sulfate and 1.26×10-2 M potassium bromide. Solid silver nitrate is added slowly to this mixture. What is the concentration of bromide ion when sulfate ion begins to precipitate? [bromide] = M   2. A solution contains 8.84×10-3 M cobalt(II) acetate and 8.03×10-3 M silver nitrate. Solid sodium carbonate is added slowly to this mixture. What is the concentration of cobalt(II) ion when silver ion begins to precipitate? [Co2+] = M   3. A solution contains 5.20×10-3 M ammonium sulfite and 5.12×10-3 M sodium sulfide. Solid calcium acetate is added slowly to this mixture. What is the concentration of sulfite ion when sulfide ion begins to precipitate? [sulfite] = M

What mass of Fe(OH)3 will be obtained when 100. mL of 0.240 M FeClz is mixed with 200. mL of 0.182 MNAOH? |g Fe(OH)3

If 350 mL of some Pb(NO3)2 solution is mixed with 550 mL of 3.20 x 10−2 M NaCl solution, what is the maximum concentration of the Pb(NO3)2 solution added if no solid PbCl2 forms? (Assume Ksp = 2.00 x 10−5 M at this temperature.) Enter the concentration in M.