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⁺]
14. 30.0 mL of 0.150 M KASO, is mixed with 20.0 mL of 2.00 M AgNO, and a precipitate forms. What are the equilibrium (Ag+] and [AsOd") in the resulting solution?
(References A solution contains 4.4 x 10-5 M Na,PO. What is the minimum concentration of AgNO, that would cause precipitation of solid Ag, PO (K =1.8 x 10 Concentration - Su An Try Another Version memorie
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.
A solution contains 5.2 x 10-M Na, PO4. What is the minimum concentration of AgNO, that would cause precipitation of solid Ag, PO, (K = 1.8 x 10-18)? Concentration M Submit Answer Try Another Version 6 item attempts remaining
Part A A 110.0-mL sample of a solution that is 2.7 x 10- M in AgNO, is mixed with a 230.0-mL sample of a solution that is 0.11 M in NaCN. For Ag(CN)2,Kf = 1.0 x 1021 After the solution reaches equilibrium, what concentration of Ag+ (aq) remains? Express your answer using two significant figures. IVO ACV O O ? [Ag +) =
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
4. Precipitation reactions a. 200 mL of 0.125M CuClz is mixed with 300mL of 0.10M Na,PO. i. ii. ili. Write a balanced chemical and ionic equation for this reaction Determine the concentration of all the ions Find the mass of the precipitate. b. 75mL of 0.100M Na COs is added to 125mL of unknown molarity of NiCI2 (aq). If 0.594 g of NicOs solid was precipitated i. Determine the initial molarity of NiCh ii. Find the final molarity of Cl...
Let's say that the cell compartment for Ag+/Ag contains 100.0 mL of 1.0 M solution. Add 100.0 mL of 1.0 M NaCl to that compartment. Ksp of AgCl is 1.6 x 10^-10 so the Qsp > Ksp and solid AgCl will precipitate out of solution. This silver chloride is in equilibrium with its ions according to the Ksp equilibrium. Calculate [Ag+] (HINT: it will be very small) and then use your result to calculate the cell potential to the hundredths...
1) A 110 mL solution of 0.340 M HCl(aq) is mixed with a solution of 330 mL of 0.150 M HNO3(aq). The solution is then diluted to a final volume of 1.00 L. How many moles of H+ are present in the final solution? 2) When 38.0 mL of 0.1250 M H2SO4 is added to 100 mL of a solution of Pblu, a precipitate of PbSO4 forms. The PbSO4 is then filtered from the solution, dried, and weighed. If the...
Ksp = [Ba²+][10,1 2. 10. mL of 0.10 M Ba(NO), is mixed with 10. mL of 0.10 M KIO,, a precipitate forms. for barium a. Which ion will still be present at appreciable concentration in the equilibrium mixture if K iodate is very small? b. What would that concentration be? 3. Lead chloride, PbCly, is slightly soluble with K equal to 1.7 x 10. a. What is the solubility of lead chloride in pure water? b. What would the solubility...