A solution is prepared by mixing 47.00 mL of 0.024 M AgNO3 with 11.00 mL of...

Question

Question

A solution is prepared by mixing 47.00 mL of 0.024 M AgNO₃ with 11.00 mL of 1.0×10^-3M Na₂CO₃. Assume that volumes are additive.

Calculate [Ag⁺], [CO₃^2–], [Na⁺], and [NO₃^–] after equilibrium is established.

[Ag+]=

[CO₃²⁺]=

[Na+]=

[NO₃^-]=

science chemistry

Answer 1

Similar Homework Help Questions

Calculate pH when: solution prepared by mixing 112.0mL of 1.3x10^-3 M HCL and 444.0 mL of...

Calculate pH when: solution prepared by mixing 112.0mL of 1.3x10^-3 M HCL and 444.0 mL of M HClO4 (assume that volumes are additive) Solution prepared by mixing 1120 mL of 1.3 10-3 M HCl and 444.0 mL of 1.0-103 MHCIO, (Assume that volumes are additive ) Express your answer using two decimal places. pH- Submt Request Answer ide Feedback
A buffer solution is prepared by mixing 23.6 mL of 0.398 M sodium dihydrogen citrate with...

A buffer solution is prepared by mixing 23.6 mL of 0.398 M sodium dihydrogen citrate with 36.6 mL of 0.881 M sodium hydrogen citrate A table of pKa values can be found here 1. Calculate the pH (to two decimal places) of this solution Assume the 5% approximation is valid and that the volumes are additive. Submit Answer Tries 0/3 2. Calculate the pH (to two decimal places) of the buffer solution after the addition of 24.9 mL of a...
What is the result of mixing 25.0 mL of 0.0010 M NaCl solution with 75.0 mL...

What is the result of mixing 25.0 mL of 0.0010 M NaCl solution with 75.0 mL of 0.0050 M AgNO3 solution? Assume volumes are additive.

B. A solution formed by mixing 54.0 mL 0.40 M CH&NH Cl (ag) and 46.0 mL 0.65 M CHsNH: (ag). Assum...

b. A solution formed by mixing 54.0 mL 0.40 M CH&NH Cl (ag) and 46.0 mL 0.65 M CHsNH: (ag). Assume volumes are additive. b. A solution formed by mixing 54.0 mL 0.40 M CH&NH Cl (ag) and 46.0 mL 0.65 M CHsNH: (ag). Assume volumes are additive.
What is the pH of the solution obtained by mixing 30.00 mL of 0.250 M...

What is the pH of the solution obtained by mixing 30.00 mL of 0.250 M HCl and 30.00 mL of 0.125 M NaOH? We assume additive volumes. What is the pH of a solution that is 0.75 M in sodium acetate and 0.50 M in acetic acid? (ka for acetic acid is 1.3x10-5.) Calculate the pH of a solution prepared by mixing 15.00 ml of 0.10 M NaOH and 30.00 mL of 0.10 M benzoic acid solution. (Benzoic acid is monoprotic; its...
For questions 17 and 18. A solution is prepared by mixing 150.0 mL of 1.0 x...

For questions 17 and 18. A solution is prepared by mixing 150.0 mL of 1.0 x 10 M AgNO3 with 200mL of 5.0M Na S O The stepwise formation equilibria are Ag +S203 Ag (S2O3) Ag(S2O3) +S20, Ag(S20s)2 17. What is the concentration of Ag(S203) in solution (5 points): A. 3.8x 10 B. 1.8 x 10 18 C. 4.3x 10 D. 5.6 x 10 K1 7.4 x 10 K2 3.9 x 104

4- (a) Calculate the concentration of Cd2+ ion in a solution prepared by mixing 2.0 mL...

4- (a) Calculate the concentration of Cd2+ ion in a solution prepared by mixing 2.0 mL of 1 M CA(NO3)2 solution with 1.0 L of 4.0 M NH3 solution. [Assume that the volume does not change after the addition of 2.0 ml of 1 M Cd(NO3)2] (b) Will you be able to see Ca(OH)2(6) precipitate in the solution? (Kr for Ca(NH3)42+ = 1.0 x 107, Kb for NH3 = 1.8 x 10-5; Ksp for Ca(OH)2 = 5.9 x 10-15 Cd2+...
What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3COOH...

What is the pH of a solution prepared by mixing 25.00 mL of 0.10 M CH3COOH with 25.00 mL of 0.050 M CH3COONa? Assume that the volume of the solutions are additive and that Ka = 1.8 x 10-5 for CH3COOH.
What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3...

What is the pH of a solution prepared by mixing 50.00 mL of 0.10 M NH3 with 5.00 mL of 0.10 M NH4Cl? Assume that the volume of the solutions are additive and that Kb = 1.8 × 10-5 for NH3. (Select One) 10.26 or 11.13

Suppose that 51.0 mL of 0.11 M AgNO3 is added to 50.0 mL of 0.048 M...

Suppose that 51.0 mL of 0.11 M AgNO3 is added to 50.0 mL of 0.048 M NaCl solution. (a) What mass of AgCl will form? g AgCl the tolerance is +/-2% (b) Calculate the final concentrations of all of the ions in the solution that is in contact with the precipitate. [Ag+] = × 10 M [NO3−] = × 10 M [Na+] = × 10 M [Cl−] = × 10 M (c) What percentage of the Ag+ ions have precipitated?...