You have 1L of the previous buffer (0.042 mol of NaH, PO, and 0.058 mol of NasHPO), If you add 1.Oml of 10.0M NaOH to this buffer, what would be the final pH? (Note: although the final volume after the addition of NaOH solution would be 1001ml (1.001L). you can ignore this volume change in the calculation.) You have to show your calculation process.

You have 1L of the previous buffer (0.042 mol of NaH, PO, and 0.058 mol of NasHPO), If you add 1.Oml of 10.0M NaOH to this buffer, what would be the final pH? (Note: although the final volume after the addition of NaOH solution would be 1001ml (1.001L). you can ignore this volume change in the calculation.) You have to show your calculation process.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 12QAP: A buffer is prepared by dissolving 0.062 mol of sodium fluoride in 127 mL of 0.0399 M hydrofluoric...

See similar textbooks

Similar questions

Which of these buffers involving a weak acid HA has the greater resistance to change in pH? Explain your answer. (i) [HA] =0.100 M = [A] (ii) [HA] = 0.300 M = [A]
A buffer is prepared using the butyric acid/butyrate (HC4H7O2/C4H7O2)acid-base pair. The ratio of acid to base is 2.2 and Ka for butyric acid is1.54105. (a) What is the pH of this buffer? (b) Enough strong base is added to convert 15% of butyric acid to the butyrate ion. What is the pH of the resulting solution? (c) Strong acid is added to the buffer to increase its pH. What must the acid/base ratio be so that the pH increases by exactly one unit (e.g., from 2 to 3) from the answer in (a)?
Fifty cm3 of 1.000 M nitrous acid is titrated with 0.850 M NaOH. What is the pH of the solution (a) before any NaOH is added? (b) at half-neutralization? (c) at the equivalence point? (d) when 0.10 mL less than the volume of NaOH to reach the equivalence point is added? (e) when 0.10 mL more than the volume of NaOH to reach the equivalence point is added? (f) Use your data to construct a plot similar to that shown in Figure 14.10 (pH versus volume NaOH added).
Can someone please explain why and how the step 1 was done? What was its purpose? Why was only the pKa2 value was used in the second step 2? I don't understand shortcuts and I would appreciate it if it's explained step by step. This was the solution to my previous question in which I asked: What is the pH of a buffer prepared by mixing 100 mL 0.050 mM NaH2PO4 and 25 mL 0.075 mM Na2HPO4? (pKa1=2.2; pKa2= 7.21; pKa3=12.7)
A 1.00 L volume of buffer is made with concentrations of 0.350 M sodium formate (NaHCOO) and 0.550 Mformic acid (HCOOH). (Ka of HCOOH is 1.8 x 10^-4)a. Calculate the initial pH of this bufferb. What is the pH after the addition of 0.0050 mol HCl?c. How about after the addition of 0 0050 mol NaOH[For parts b and c, assume that volume doesn t change in the addition process and that neutralization proceeds to completion]
A solution is made by dissolving 0.1283 g of the acid form of the buffer TRIS (molecular mass = 157.60 g/mol) along with 0.1975 g of the basic form of TRIS (molecular mass = 121.136 g/mol). The pK a of TRIS is 8.08. A very small amount of potassium dihydrogen phosphate is added (not enough to cause any change in the pH). What is the fractional amount of the potassium dihydrogen phosphate that is in the PO 4 3- form? Phosphoric acid is a triprotic acid with pK a1 = 2.16, pK a2 = 7.21 and pK a3 = 12.32.
A solution is prepared by dissolving 0.23 mol of lactic acid and 0.27 mol of sodium lactate in water sufficient to yield 1.00 L of solution. The addition of 0.05 mol of HCl to this buffer solution causes the pH to drop slightly. The pH does not decrease drastically because the HCl reacts with the ________ present in the buffer solution. The Ka of lactic acid is 1.4 ⋅10-4. A. H3O+ B. H2O C. lactate ion D. lactic acid E. This is a buffer solution: the pH does not change upon addition of acid or base.
A buffer solution that is 0.473 M in HCN and 0.473 M in NaCN has a pH of 9.40. The addition of 0.01 mol of OH^- to 1.0 L of this buffer would cause the pH to _________ : increase slightly, increase by 2 units, decrease slightly, decrease by 2 units or not change. The capacity of this buffer for added H3O^+ could be increased by the addition of 0.175 mol _________of the: weak acid or of the salt.
The pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of Na in 2.00 L of solution is 5.881. The dissociation constant Ka of HA is 5.66×10−7 A. What is the pH after 0.150 mol of HCI is added to the buffer from Part A? Assume no volume change on the addition of the acid. B. What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.
a. What is the pH of a buffer prepared by adding 0.708 mol of the weak acid HA to 0.305 mol of Na in 2.00 L of solution? The dissociation constant Ka of HA is 5.66×10^−7. b. What is the pH after 0.150 mol of HCI is added to the buffer from Part A? Assume no volume change on the addition of the acid. c. What is the pH after 0.195 mol of NaOH is added to the buffer from Part A? Assume no volume change on the addition of the base.
Consider a buffer solution that contains 0.55 M NH2CH2CO2H and 0.35 M NH2CH2CO2Na. pKa(NH2CH2CO2H)=9.88. a. Calculate the change in pH if 0.155 g of solid NaOH is added to 250 mL of this solution. b. If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer. c. Calculate its pH.
You are tasked with making a buffer solution containing equal amounts of propionic acid from a 99.5 wt% solution (d = 0.993 g/mL, FW = 74.08 g/mol) and sodium propionate (solid, FW = 96.06 g/mol). What concentration of the buffer must be prepared to prevent a change in the pH by more than 0.5 pH units after the addition of 10.00 mL of 3.00 M HCl to 100.0 mL of the buffer solution? The Ka for propionic acid is 1.76 x 10-5.