What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH₂Cl) in enough water to form 2.50L of solution. The K₂ of ammonia is 1.76 x 10-5. How many moles of sodium hypobromite, NaBro, should be added to 1.00 L of 0.050 M hypobromous acid, HBrO, to form a buffer solution of pH 8.80? Assume no volume change when the NaBrO is added. K. of HBrO is 2.50 x 10.⁹ How many grams of sodium lactate, NaC3H₂O3, should be added to 1.00L of 0.150M lactic acid, HC3H₂O3, to form a buffer solution with a pH of 3.90? Assume no volume change when the sodium lactate is added. K. of lactic acid is 1.40 x 10-4.

What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH₂Cl) in enough water to form 2.50L of solution. The K₂ of ammonia is 1.76 x 10-5. How many moles of sodium hypobromite, NaBro, should be added to 1.00 L of 0.050 M hypobromous acid, HBrO, to form a buffer solution of pH 8.80? Assume no volume change when the NaBrO is added. K. of HBrO is 2.50 x 10.⁹ How many grams of sodium lactate, NaC3H₂O3, should be added to 1.00L of 0.150M lactic acid, HC3H₂O3, to form a buffer solution with a pH of 3.90? Assume no volume change when the sodium lactate is added. K. of lactic acid is 1.40 x 10-4.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

A buffer solution is formed by adding 0.150 moles of solid strontium acetate, Sr(C₂H₃O₂)₂, to 500.0 ml of 0.400 M acetic acid, HC₂H₃O₂ solution. You may assume that the change in volume is negligible upon addition of the solid.Calculate the pH of the buffer solution.Calculate the pH of the buffer solution after the addition of 7.50 ml of 2.00 M NaOH. Acetic Acid: pKa = 4.75 Ka=1.76E-5 M.w.=60.05 g/mol
Let’s build a buffer using hypobromous acid (HBrO, Ka = 2.3×10−9) and hypobromite ion (BrO−). If [HBrO] is 0.100 M, then what concentration of hypobromite ion is needed to achieve pH = 8.50
2. What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4CI) in enough water to form 2.50L of solution. The Kb of ammonia is 1.76 x 10-5.
Calculate the pH of a buffer solution prepared by dissolving 0.78 mole of sodium fluoride (NaF) and 1.0 mole of hydrofluoric acid (HF) in enough water to make 1.0 liter of solution. [Ka(HF) = 6.8 x 10-4]
A buffer contains 0.035 mol of boric acid (pKa = 9.15) and 0.015 mol of sodium borate per liter. (a) Calculate the pH of the buffer.(b) Calculate the pH when 2.5 mL of 0.50 M HCl is added to 0.5 L of the buffer.(c) Calculate the pH when 2.5 mL of 0.50 M HCl is added to 0.5 L of pure water.
The pKa of the weak acid HA is 4.49. If 0.17 mL of a 1.00 M solution of hydrochloric acid are added to a solution made by mixing 20.00 mL of 0.100 M HA and 10.00 mL of 0.100 M NaOH, what is the pH of the solution after the acid is added?
A buffer solution is prepared by dissolving 1.700 g of ammonium chloride (NH4Cl) into 100.00 mL of a 0.170 M solution of ammonia (NH3). The Kb of ammonia is 1.8 x 10−5. What is the pH of the solution?
A buffer solution is made that is 0.368 M in HCN and 0.368 M in KCN. If Ka for HCN is 4.00 × 10-¹0, what is the pH of the buffer solution? pH = Write the net ionic equation for the reaction that occurs when 0.088 mol HCl is added to 1.00 L of the buffer solution. (Use the lowest possible coefficients. Omit states of matter. Use H3O+ instead of H+) + +
Calculate the pH of a buffer formed by mixing 85.0 mL of 0.130 M lactic acid, HC3H503, with 95.0 mL of a 0.150 M solution of sodium lactate, NaC3H5O3. The Ka of lactic acid is 1.40 x 10-4.
Consider the buffer system of ammonia, NH3, and ammonium ion NH4+. (Ka= 5.6 x 10-10). a) What is the pH of a buffer solution prepared by adding 30.0g of ammonium chloride (NH4Cl) to 600 mL of .400 M ammonia? b) What is the pH of the solution after 100.0 mL of 2.0 M NaOH are added to the solution from part (a)? c) What is the pH of the solution after 100.0 mL g 1.0 M HCl are added to the solution from part (a)? d) What is the pH of the solution after 30g of NaOH are added to the solution from part (a)?
A buffer solution is made by dissolving 0.230 moles of sodium hypochlorite in 1.00 L of 0.220 M hypochlorous acid. What is the pH of the solution after 0.0100 moles of sodium hydroxide is added? (The K a of HClO is 2.9 × 10 −8.)
A buffer solution is prepared by dissolving 1.000 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.100 M solution of acetic acid. Then 3.00 mL of a 2.00 M solution of sodium hydroxide is added to the acetic acid/sodium acetate buffer solution. The Ka of acetic acid is 1.8 × 10−5. What is the pH of the solution after adding NaOH?