a solution contains Al^3+ and Co^2+ the addition of 0.3471 L of 1.814 M NaOH results...

a solution contains Al^3+ and Co^2+ the addition of 0.3471 L of 1.814 M NaOH results in the complete precipitation of ions as Al(OH)3 and Co(OH)2 the total mass of the precipitate is 22.28g find the masses of Al^3+ and Co^2+ in the solution

Expert Solution

queen_honey_blossom answered 8 months ago

A solution contains Al 3 + and Co 2 + . The addition of 0.3488 L...

A solution contains Al 3 + and Co 2 + . The addition of 0.3488 L of 1.779 M NaOH results in the complete precipitation of the ions as Al ( OH ) 3 and Co ( OH ) 2 . The total mass of the precipitate is 22.32 g . Find the masses of Al 3 + and Co 2 + in the solution.

A solution contains Al3+ and Co2+. The addition of 0.3628 L of 1.714 M NaOH results...

A solution contains Al3+ and Co2+. The addition of 0.3628 L of 1.714 M NaOH results in the complete precipitation of the ions as Al(OH)3and Co(OH)2. The total mass of the precipitate is 21.96 g. Find the masses of Al3+and Co2+ in the solution.

A solution contains Cr3+ ion and Mg2+ ion. The addition of 1.00 L of 1.52 M...

A solution contains Cr3+ ion and Mg2+ ion. The addition of 1.00 L of 1.52 M NaF solution is required to cause the complete precipitation of these ions as CrF3(s) and MgF2(s). The total mass of the precipitate is 50.4 g . Determine the mass of Cr3+ in the original solution.

A 0.1000 M NaOH solution was employed to titrate a 25.00-mL solution that contains 0.1000 M...

A 0.1000 M NaOH solution was employed to titrate a 25.00-mL solution that contains 0.1000 M HCl and 0.0500 M HOAc. a) Please determine the pH of the solution after 27.00 mL of NaOH is added. Ka, HOAc = 1.75*10-5 b) what's the solution pH at the second equivalence point?

3)Suppose a solution is prepared by dissolving 15.0 g NaOH in 0.150 L of 0.250 M...

3)Suppose a solution is prepared by dissolving 15.0 g NaOH in 0.150 L of 0.250 M nitric acid. What is the final concentration of OH- ions in the solution after the reaction has gone to completion. Assume that there is no volume change when adding the grams of NaOH.

A 1.00 L solution contains 5.00x106-5 M Cu(NO3)2 and 1.00x10^-3 M ethylenediamine. What is the concentration...

A 1.00 L solution contains 5.00x106-5 M Cu(NO3)2 and 1.00x10^-3 M ethylenediamine. What is the concentration of Cu2+ (aq) in the solution

1. What is the pH of a solution that contains 8.025 x 10-4 M NaOH? 2....

1. What is the pH of a solution that contains 8.025 x 10-4 M NaOH? 2. Calculate the pH for a 9.21 x 10-7 M solution of Ba(OH)2. 3. Calculate the pOH for a 5.541 x 10-6 M solution of Ba(OH)2. 4. Calculate the pH for a solution with a hydronium concentration of 4.52 x 10-3 M.

A 1.00 L solution contains 2.00×10-4 M Cu(NO3)2 and 2.500×10-3 M ethylenediamine (en). The Kf for...

A 1.00 L solution contains 2.00×10-4 M Cu(NO3)2 and 2.500×10-3 M ethylenediamine (en). The Kf for Cu(en)22+ is 1.00×1020. What is the concentration of Cu2+(aq ) in the solution?

A 1.00 L solution contains 2.00 X 10^-4 M Cu(No3)2 and 1.2 x 10^-3 M Ethylenediamine...

A 1.00 L solution contains 2.00 X 10^-4 M Cu(No3)2 and 1.2 x 10^-3 M Ethylenediamine (en). The Kf for Cu(en)2 2+ is 1.0X10^20 What is the concentration of Cu 2+ (aq) in the solution?

A cell is constructed using a piece of Al in a 1.00 M Al(NO3)3 solution and...

A cell is constructed using a piece of Al in a 1.00 M Al(NO3)3 solution and a piece of Cu submerged in a Cu(NO3)2 solution. Calculate the cell potential. Write the overall reaction. Which piece of metal gains mass and which loses mass? Which reaction occurs at the anode and which reaction occurs at the cathode? If the above cell was constructed using 0.250 M Al(NO3)3 and 0.300 M Cu(NO3)2, calculate the cell potential. Then calculate Delta G.

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