Question

In: Chemistry

Question 6 Calculate the pH of a solution prepared by mixing equal volumes of 0.050 M...

Question 6

Calculate the pH of a solution prepared by mixing equal volumes of 0.050 M sodium oxalate, Na2C2O4 (aq), and 0.010 M ammonium chloride, NH4Cl (aq).

For ammonium, Ka = 5.70 × 10–10; for oxalic acid, Ka,1 = 5.60 × 10–2and Ka,2 = 5.42 × 10–5.

Hint #1: Use the charge balance equation as your main equation. Use the mass balance and equilibrium equations to find an expression for each species in terms of [H3O+] or [OH–], then substitute into the charge balance equation.

Hint #2: If no simplifying assumptions are obvious, you can always solve the exact final equation numerically using algebra and Excel. See the pre-exercise for a pair of methods.

Solutions

Expert Solution


Related Solutions

PART A) A solution is prepared by mixing equal volumes of 0.17 M HCl and 0.42...
PART A) A solution is prepared by mixing equal volumes of 0.17 M HCl and 0.42 M HNO3. (Assume that volumes are additive.) Express the pH to two decimal places. PART B) Using the chart Estimate [H3O+] in a 1.5 M solution of each acid. Express the molar concentrations to two significant figures separated by commas. I'm stuck on the one that says very large. For all the other ones I multiplied the Ka by the 1.5M. The answer for...
Calculate the pH of a solution made by mixing 100.0 mL of 0.050 M NH3 with...
Calculate the pH of a solution made by mixing 100.0 mL of 0.050 M NH3 with 100.0 mL of 0.100 M HCl. (K b for NH 3 = 1.8 x 10 –5 )
What is the pH of a solution that results from mixing together equal volumes of a...
What is the pH of a solution that results from mixing together equal volumes of a 0.050 M solution of ammonia and a 0.025 M solution of hydrochloric acid? (pKa of NH4+ = 9.25)
What is the pH of a solution that results from mixing together equal volumes of a...
What is the pH of a solution that results from mixing together equal volumes of a 0.160 M solution of acetic acid and a 0.080 M solution of sodium hydroxide?
11. Calculate the pH of a solution prepared by mixing a) 48.0 mL of 0.212 M...
11. Calculate the pH of a solution prepared by mixing a) 48.0 mL of 0.212 M NaOH and 66.0 mL of 0.187 M HCl b) 69.0 mL of 0.345 M KOH and 125 mL of 0.400 M HC3H5O2 c) 350 mL of 0.130 M NH3 and 400 mL of 0.100 M HCl
Calculate the pH of a solution prepared by mixing a) 25.0 mL of 0.512 M NaOH...
Calculate the pH of a solution prepared by mixing a) 25.0 mL of 0.512 M NaOH and 34.0 mL of 0.187 M HCl b) 46.0 mL of 0.235 M KOH and 50.0 mL of 0.420 M HC3H5O2 c) 400 mL of 0.250 M NH3 and 250 mL of 0.120 M HCl
Calculate the pH of a solution prepared by mixing a) 25.0 mL of 0.512 M NaOH...
Calculate the pH of a solution prepared by mixing a) 25.0 mL of 0.512 M NaOH and 34.0 mL of 0.187 M HCl b) 46.0 mL of 0.235 M KOH and 50.0 mL of 0.420 M HC3H5O2 c) 400 mL of 0.250 M NH3 and 250 mL of 0.120 M HCl
1. Calculate the pH of a solution prepared by mixing 2.50 L of 2.35 M HF...
1. Calculate the pH of a solution prepared by mixing 2.50 L of 2.35 M HF with 4.50 L of 1.56 M NaF. 2. A 4.00-g sample of NaOH is added to 2.00 L of the solution prepared in problem 1. Calculate the pH of the new solution. Assume any volume change is negligible.
4.24 Equal volumes of 0.050 M Ba(OH)2 and 0.040 M   HCl are allowed to react. Calculate...
4.24 Equal volumes of 0.050 M Ba(OH)2 and 0.040 M   HCl are allowed to react. Calculate the molarity of each of the ions present after the reaction. Answer: 0.025  M Ba2+  ; 0.020 M   HCl- ; [H+] = (approx) 0 ; 0.30 M OH-
Calculate the pH of a solution prepared by mixing 300mL of 0.250 m aqueous HF (dens=1.10g/mL)...
Calculate the pH of a solution prepared by mixing 300mL of 0.250 m aqueous HF (dens=1.10g/mL) with 43.6g of an aqueous solution that is 3.6% NaOH by mass. (dens=1.02g/mL).
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT