A buffer solution contains 0.25 M NANO, and 0.75 M HNO, at equilibrium (HNO2 K, = 4.5 x 104). Calculate the pH of the original buffer and the new pH of this buffer solution after 0.20 mol of NaOH has been added to 1.00 L of the buffer. (Do not use H-H) Select one: O a. original buffer = 3.35, new pH = 3.26 O b. original buffer = 2.86, new pH = 3.26 O c. original buffer = 3.26, new pH = 3.35 %3D O d. original buffer = 2.86, new pH = 3.35

A buffer solution contains 0.25 M NANO, and 0.75 M HNO, at equilibrium (HNO2 K, = 4.5 x 104). Calculate the pH of the original buffer and the new pH of this buffer solution after 0.20 mol of NaOH has been added to 1.00 L of the buffer. (Do not use H-H) Select one: O a. original buffer = 3.35, new pH = 3.26 O b. original buffer = 2.86, new pH = 3.26 O c. original buffer = 3.26, new pH = 3.35 %3D O d. original buffer = 2.86, new pH = 3.35

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 contains dissolved C6H5NH2 and C6H;NH3CI. The initial concentration of C6H5NH2 is 0.50 M and the pH of the buffer is 4.20. Determine the concentration of C6H5NH3* in the solution. The value of Kb for C6H5NH2 is 3.8 x 10 10. ( PREV 1 3 NEXT > Based on your ICE table and definition of Kb, set up the expression for Kb in order to determine the unknown. Do not combine or simplify terms. Kp 3.8 x 10-10 %3D %3D 5 RESET [0] [0.50] [x] [2x] [4.20] [6.3 x 10-5) [1.6 x 10-10] [3.8 х 1011 [x + 4.20] [x - 4.20] [x + 6.3 x 10-51 [x - 6.3 х 10-5] [x + 1.6 x 101°] [x - 1.6 x 10-10] [x + 3.8 x 10-101 [x - 3.8 x 101°]
Aa.51.
8. Determine the pH at the equivalence point when 65.0 mL of 0.429 M HBrO is mixed with 0.371 M NaOH. Ka = 2.8 x 10 ⁹ Your answer must include an ICE box showing the new equilibrium formed.
The pH of blood plasma is 7.40. Assuming that the principal buffer system in blood is HCO, /H2CO3, A) determine the ratio [HCO,]/[H2CO3] in blood plasma. The ionization con- stant of carbonic acid is K.(H2CO3) = 4.3 x 10-7. B) Based on your result in part (A), how many moles of H2CO3 (assuming that they occupy no volume) would need to be added to 300.0 mL of an aqueous solution that is 0.250 mol L- in NaHCO3 to make a buffer solution of the same pH as blood plasma? To solve the problem you may assume that the solutions behave as ideal dilute solutions (solute-type activity coefficients equal to unity).
01 5 If the dissociation constant of a weak acid is 8.1 x 10-5, at what ratio should you adjust the concentration of the weak acid and its conjugate base in order that has a pH of 4.09? prepare a buffer Oa) 0.100 M veak acid with 0.100 M conjugate base b) 0.100 M weak acid with 0.0100 M conjugate base Oc) 0.100 M weak acid with 0.0500 M conjugate base d) 1.000 M weak acid with 0.0100 M conjugate base e) 0.510 M weak acid with 0.0510 M conjugate base 0 000 О
Determine the resulting pH when 0.003 mol of solid NaOH is added to a 100.0 mL buffer containing 0.13 M HClO and 0.37 M NaClO. The value of Ka for HClO is 2.9 × 10⁻⁸. Determine the moles of the ractant and product after the reaction of the acid and base. (Similar to ICE format but is instead Before (mol), Change (mol), and After (mol) Determine the ICE table for HClO (aq) + H2O - H3O+ + ClO- (aq) Fill in Ka= ? = 2.9 * 10-8 Calculate pH
6. Which of the following processes will increase the pH of a buffer solution prepared by mixing 0.89 mol HCOOH (formic acid) and 0.76 mol HCOONa (sodium formate) into a 1-L solution? Ka (HCOOH) = 1.8 x 104. %3D a) add some NaCl into the buffer solution. b) add some HCl into the buffer solution. c) add some NaOH into the buffer solution. d) add more water into the buffer solution. e) None of the above.
You have 0.600 L of an 0.300 M acetate buffer solution (i.e. [HC;H,O2] + [C,H¿O¿¯] = 0.300 M) at pH 5.30. What will the new pH of the solution be if you add 82.0 mL of 1.000 M HCI to it. Acetic acid has a pKa of 4.74.
What is the pH of a buffer prepared by mixing 5.0 g of ammonia (NH3) and 20.0 g of ammonium chloride (NH4Cl) in enough water to form 2.50L of solution. The K, 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 NaBr is added. K. of HBrO is 2.50 x 10.⁹ How many grams of sodium lactate, NaC3H5O3, 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.
A buffer solution is 0.416 M in H2 S and 0.245 M in NaHS. If K21 for H2S is 1.0 x 10-7, what is the pH of this buffer solution? pH =| A buffer solution is 0.376 M in N.HSO3 and 0.390 M in Na,SOg. If K, for HSO3 is 6.4 × 10-8, what is the pH of this buffer solution? pH =
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 1.47 L buffer solution consists of 0.173 M butanoic acid and 0.299 M sodium butanoate. Calculate the pH of the solution following the addition of 0.060 moles of NaOH. Assume that any contribution of the NaOH to the volume of the solution is negligible. The K, of butanoic acid is 1.52 x 10-. pH =