14. 30.0 mL of 0.150 M KASO, is mixed with 20.0 mL of 2.00 M AgNO,...
When 100 mL of 1.0 M Na₃PO₄ is mixed with 100 mL of 1.0 M AgNO₃, a yellow precipitate forms and [Ag⁺] becomes negligibly small. Which of the following is a correct listing of the ions remaining in solution in order of increasing concentration? (A) [PO₄³⁻] < [NO₃⁻] < [Na⁺] (B) [Na⁺] < [NO₃⁻] < [PO₄³⁻] (C) [Na⁺] < [PO₄³⁻] < [NO₃⁻] (D) [PO₄³⁻] < [Na⁺] < [NO₃⁻] (E) [NO₃⁻] < [PO₄³⁻] < [Na⁺]
375 mL of a 0.150 M aqueous solution of silver (I) nitrate is mixed with 125 mL of a 0.125 M aqueous solution of sodium phosphate. Calculate the mass of precipitate that forms and the final concentration of each ion in the mixed solution. Volumes are additive and the precipitation reaction goes to completion. Can you show all work for calculating the final concentration of each ion in the reaction including Ag, NO3^-1, Na and PO4^-3
A 130.0 mL sample of a solution that is 2.8time 10^-3 M in AgNO, is mixed with a 230 0 - mL sample of a solution that is 0.12 M in NaCN. After the solution reaches equilibrium, what concentration of AG^+ (aq) remains? Express your answer using two significant figures.
if 25.0 mL of 2.00 M K2SO4 is added to 20.0 mL of a 2.00 M Pb(NO3)2 solution what is the mass (in grams) of the precipitate?
Calculate the pH when 10.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 x 10-9)
If 30.0 mL of 0.150 M CaCl2 is added to 31.0 mL of 0.100 M AgNO3, what is the mass of the AgCl precipitate? ?g
Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)
calculate the pH & POH of a mixture containing 20.0 mL of 0.150 m HBr mixed W/ 40.0 mL of water.
If 30.0 mL of 0.150 M CaCl2is added to 29.5 mL of 0.100 M AgNO3, what is the mass of the AgCl precipitate? g
A solution of 100.0 mL of 0.200 M KOH is mixed with solution of 200.0 mL of 0.150 M NiSO_4. (a) Write the balanced chemical equation for the reaction that occurs. (b) What precipitate forms? (c) What is the limiting reactant? (d) How many grams of this precipitate form? (e) What is the concentration of each ion that remains in solution?