small amount of HCl(aq) is added to this buffer system 1- NO3 + H₂0 OH¹ + HNO3 the pH rises only a little since the equilibrium shifts left the pH does not change since the buffer uses up all the HCl(aq) the pH drops only a little since the equilibrium shifts right the pH drops only a little since the equilibrium shifts left

small amount of HCl(aq) is added to this buffer system 1- NO3 + H₂0 OH¹ + HNO3 the pH rises only a little since the equilibrium shifts left the pH does not change since the buffer uses up all the HCl(aq) the pH drops only a little since the equilibrium shifts right the pH drops only a little since the equilibrium shifts left

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...

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Similar questions

Which of the following is true of a buffer solution that contains equivalent amounts of acid and conjugate base? The pH will always be greater than 7, regardless of the acid and conjugate base. The pH of the solution will be equal to the pKa of the acid. The pH of the solution will be equal to Kw. The pH will be equal to the concentration of the conjugate base. The pH will be equal to the concentration of the acid.
What is the hydronium ion concentration in a 0.100 M solution of ammonium nitrate, NH4NO3, a salt composed of NH4+ and NO3−? Which is the stronger acid, C6H5NH3+ or NH4+? . Concentration NH4+ H2O H3O+ NH3 Initial Change Equilibrium
Which mixture of equal volumes of the following solutions will produce a buffer solution? A. 0.5 M CH3COOH and 0.5 M NH4Cl B. 1.0 M NH3 and 0.5 M HNO3 C. 0.5 M NH4Cl and 0.5 M NaOH D. 0.5 M CH3COOH and 1.0 M NaOH E. 0.5 M CH3COOH and 0.5 M NaOH
Which one of the following pairs of compounds would be able to function as a buffer? HBr and Br- HNO3 and NO3- NaBr and Br- KOH and OH- HNO2 and NO2-
Arrange the following solutions in order of increasing hydroxide ion concentration (lowest to highest): a buffer solution with a pH of 11.0 0.5 M HCl 0.1 M HNO3 a solution of HNO2 with a pH of 4.0 water
What is the pH of a solution resulting from 5.00 mL of 0.011 M HCl being added to 50.00 mL of pure water? 3.00 1.12 12.88 2.17 11.88
Which of the following solutions has the lowest pH? Group of answer choices 0.3 M Sodium Hydroxide 0.3 M Lactic Acid (Ka = 1.4 x 10-4) 0.3 M Propionic Acid (Ka = 1.3 x 10-5) 0.3 M Iodic Acid (Ka = 1.6 x 10-1)
Determing the effect of adding BASE to the Given solutions
Which of the following has the lowest pH? 3.9x10-3 M HPO42- (Ka3=4.2x10-13) 0.00010 M H3BO3 (Ka=5.8x10-10) 1.2x10-6M C6H5NH2 (Kb=4.3x10-10) pure water
original buffer solution has a pH of 4.76 diluted HCl solution and original buffer solution has a pH of 4.69 diluted NaOH solution and original buffer solution has a pH of 4.83 H20 and original buffer solution has a pH of 4.76 Calculating the pH of the buffer solution when strong base is added: 1a)Write the equation for the chemical reaction showing the neutralization of strong base (OH-) with the buffer. b)Calculate the moles of strong base and buffer components initially present when 5.00 mL of 0.100M NaOH is added to 25.0mL of buffer solution. Based on the chemical equation written above in 3a, determine the moles of each component remaining after reaction has gone to completion (before equilibrium has been re-established c)Calculate the pH of the buffer system once equilibrium has been re-established. State any simplifying assumptions and then check that the simplifying assumptions were valid. Use the Henderson-Hasselbalch equation for this calculation.
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Answer the questions by writing the correct letter of your answer. Explain your answer briefly in 1 or 2 When a strong acid is added to a non-buffered solution with a pH of 8, the pH of the solution decreases to a pH of 3. When the same strong acid is added to a buffered solution with a pH of 8, the pH of the solution will most likely a. increase b. decrease to pH 7 c. decrease to pH 3 d. remain at pH 8