buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104 %3D

buffer solution is prepared by dissolving 4.7 g of nitrous acid, HNO2 , and 13.8 g of sodium nitrite, NaNO2, in 1.0 liter of solution. (a) Calculate the pH of the buffer. (b) Calculate the pH of the solution which results when the following are added to separate 100 mL portions of the buffer: (i) 5.0 mmol of HCI; (ii) 5.0 mmol of NaOH. Ka = 4.5 x 104 %3D

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter15: Complex Ion And Precipitation Equilibria

Section: Chapter Questions

Problem 11QAP: A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M...

See similar textbooks

Similar questions

A buffer is prepared by dissolving 0.0250 mol of sodium nitrite, NaNO2, in 250.0 mL of 0.0410 M nitrous acid, HNO2. Assume no volume change after HNO2 is dissolved. Calculate the pH of this buffer.
You have two different concentrations of a buffer solution, 2.0 M and 0.20 M, to which 0.01 mol HCl has been added. Which of these solutions has the higher buffer capacity? In other words, which would be able to resist pH via the addition of acid longer?
Can HCl, a strong acid, be added to pure water and there be no significant change in pH?
A solution is formed by adding 3.20 grams of solid sodium hypochlorite, NaClO, to 500.0 ml of 0.0750M calcium hypochlorite, Ca(ClO)₂. Calculate the pH of the resulting solution. You may assume that the sodium hypochlorite dissolve completely and that the change in volume is negligible with the addition of the solid.
A buffer solution contains 0.302 M NaHSO3 and 0.438 M K2SO3. If 0.0168 moles of hydrochloric acid are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding hydrochloric acid)...
A buffer solution contains 0.254 M NaHSO3 and 0.348 M Na2SO3. If 0.0285 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding hydroiodic acid)
A buffer is prepared by dissolving 0.80 moles of NH3 and 0.80 moles of NH4Cl in 1.00 L of aqueous solution. If 0.10 mol of NaOH is added to 250 mL of this buffer, what is the pH of the resultant solution? Kb of NH3 = 1.8 x 10–5
For a titration to be effective, the reaction must be rapid and the yield of the reaction must essentially be 100%. Is Kc > 1, < 1, or ≈ 1 for a titration reaction? Kc is the product of all reaction products (choose from: Multiplied by, added to, divided by, subtracted from) the product of the reactants, with all concentrations of reactants and products raised to their respective stoichiometric powers. As the titration proceeds, the amount of reactants (choose from: Increases, decreases, remains the same) and the amount of products (choose from: Increases, decreases, remains the same). Because the value of the numerator is (Choose from much greater than, much less than, approximately equal to) the value of the denominator, the value of Kc will be (Choose from much greater than, much less than, approximately equal to)1 for an effective titration reaction.
A buffer solution contains 0.348 M ammonium chloride and 0.283 M ammonia. If 0.0144 moles of sodium hydroxide are added to 125 mL of this buffer, what is the pH of the resulting solution ? (Assume that the volume change does not change upon adding sodium hydroxide)
A buffer solution contains 0.254 M NaHSO3 and 0.348 M Na2SO3. If 0.0285 moles of hydroiodic acid are added to 250 mL of this buffer, what is the pH of the resulting solution ?
A buffer solution contains 0.289 M KH2PO4 and 0.399 M K2HPO4.If 0.0485 moles of hydroiodic acid are added to 250. mL of this buffer, what is the pH of the resulting solution ?(Assume that the volume does not change upon adding hydroiodic acid)pH =
What is the pH of a buffer solution if you dissolve 300 ml of 1.65M Formic Acid (HCO2H) and 250 ml of 3.66M Sodium Formate (NaHCO2) together? If you were to now add 18 ml of 1.2M NaOH to the buffer solution, what would the new pH be?