Which of the following buffers will best prevent changes in pH when 100 µl of 1.0 M HCl is added toa solution initially at pH 7.25?BufferAcetateBicineCAPSHEPESPhosphateTris0.1 M HEPES0.01 M HEPESO 0.1M Bicine0.1 M Acetate Buffer0.01 M Bicine0.01 M Acetate Bufferchemical formacid; liq. (17.4 M)base; Na-acetate-3H₂OK₂HPO4free baseTris-HCIKH₂PO4F.W. (g/mol)60.05136.08163.19221.3238.3174.2121.14157.6136.10pka at 20 °C4.764.768.3510.407.552.1212.328.308.307.21

A buffer is a solution of a weak acid and salt of its conjugate base or a weak base and salt of its…

Which of the following buffers will best prevent changes in pH when 100 μl of 1.0 M HCl is added to a solution initially at pH 7.25? Buffer Acetate Bicine CAPS HEPES Phosphate Tris 0.1 M HEPES 0.01 M HEPES 0.1M Bicine 0.1 M Acetate Buffer 0.01 M Bicine O 0.01 M Acetate Buffer chemical form acid; liq. (17.4 M) base; Na-acetate-3H₂O K₂HPO4 free base Tris-HCI KH₂PO4 F.W. (g/mol) 60.05 136.08 163.19 221.3 238.3 174.2 121.14 157.6 136.10 pka at 20 °C 4.76 4.76 8.35 10.40 7.55 2.12 12.32 8.30 8.30 7.21

Which of the following buffers will best prevent changes in pH when 100 μl of 1.0 M HCl is added to a solution initially at pH 7.25? Buffer Acetate Bicine CAPS HEPES Phosphate Tris 0.1 M HEPES 0.01 M HEPES 0.1M Bicine 0.1 M Acetate Buffer 0.01 M Bicine O 0.01 M Acetate Buffer chemical form acid; liq. (17.4 M) base; Na-acetate-3H₂O K₂HPO4 free base Tris-HCI KH₂PO4 F.W. (g/mol) 60.05 136.08 163.19 221.3 238.3 174.2 121.14 157.6 136.10 pka at 20 °C 4.76 4.76 8.35 10.40 7.55 2.12 12.32 8.30 8.30 7.21

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.20QAP

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Similar questions

Given three acid-base indicatorsâ€”methyl orange (end point at pH 4), bromthymol blue (end point at pH 7), and phenolphthalein (end point at pH 9)â€”which would you select for the following acid-base titrations? (a) perchloric acid with an aqueous solution of ammonia (b) nitrous acid with lithium hydroxide (c) hydrobromic acid with strontium hydroxide (d) sodium fluoride with nitric acid
An aqueous buffer solution of volume 100 cm3 consists of 0.20 M CH3COOH and 0.20 M NaCH3CO2. pKa value of CH3COOH is 4.75. (a) Predict the pH value of this solution. 3 sig. fig. (b) Predict the pH value after adding 5.92 mmol NaOH (note, not mM. Volume is not 1 L) to this buffer solution assuming volume is not changed. 3 sig. fig.
a.) A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results are given in the graph attached. (i) What is the approximate pKa of the acid? (ii) What specific value from the graph is needed, in addition to the information in part (a) above, to calculate the molar concentration of the NaOH(aq) ? (iii) Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated is less than the concentration of its conjugate base.
A solution contains Na2CO3 and NaHCO3. 10 mL of the solution required 2.5 mL of 0.1 M H2SO4 for neutralisation using phenolphthalein as indicator. Methyl orange is then added when a further 2.5 mL of 0.2 M H2SO4 was required. The amount of Na2CO3 and NaHCO3 in 1 litre of the solution is: (a) 5.3g and 4.2g (b) 3.3g and 6.2g (c) 4.2g and 5.3g (d) 6.2g and 3.3g
The acid-base indicator "Thymol Blue" has two transition ranges as listed below (with the corresponding acid dissociation constants): 7. Ka AcidColour BaseColour Thymol Blue 1 Thymol Blue 2 2.24 x 102 Red Yellow 1.26 x 10 Yellow Blue What colour would you expect it to be at the following pH values? Briefly justify your answers. (a) (b) (c) (d) 0.9 5.2 7.8 10.7
The pKa of a weak acid acid HA is 4.47. Consider the titration of 100 mL of 200 mM HA (aq.) with 200 mM NaOH (aq). Draw a graph representing this titration that includes the following labeled points/regions, which are deliberately out of order. (A) pH=7| (B) Starting point (0 mL NaOH added)' (C) Region where the pH approaches 13.30 (D) Equivalence point| (E) Buffered region" (F) Halfway point And determine the pH and mL NaOH added for points B, D, and F
A 250-mL buffer solution contains 0.0510 mole of KH2PO4 and 0.0875 mole of K2HPO4. (a) Calculate the molar concentrations of H2PO4–and HPO42–, respectively, in thesolution. (b) What is the pH of the solution? (H2PO4– has Ka = 6.2 x 10–8) (c) Write a net ionic equation for the buffering reaction against a strong acid by this buffer. (d) If 0.012 mole of hydrochloric acid (HCl) is added to the solution, create a reaction table to show the buffering reaction and calculate the molar concentration of H2PO4–and HPO42–, respectively, in the resulting solution after the buffering reaction. (e) What is the pH of the resulting solution?
In which case medium in Equivalent point is expected to be neutral: titration of H2SO4 by KOH titration of NH3 H2O by HCl; titration of Na,B40, by HCl; titration of HCOOH by KOH;
16,2 Describe the effect on pH (increase, decrease, or no change) that results from each of the following addi- tions: (a) potassium acetate to an acetic acid solu- tion; (b) ammonium nitrate to an ammonia solution; (c) sodium formate (HCOONA) to a formic acid (HCOOH) solution; (d) potassium chloride to a hy- drochloric acid solution; (e) barium iodide to a hy- droiodic acid solution.
Which is the best solution to buffer at pH = 10.50? (A) A buffer solution containing 0.25 M H2CO3 and 0.45 M Na2CO3; (Ka (H2CO3) = 4.3 x 10–7) (B) A buffer solution containing 0.25 M NaHCO3 and 0.45 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11) (C) A buffer solution containing 0.12 M NaHCO3 and 0.22 M Na2CO3; (Ka (HCO3–) = 5.6 x 10–11) (D) A buffer solution containing 0.12 M NH4Cl and 2.2 M NH3; (Ka (NH4+) = 5.6 x 10–10)
6
Caleulate the pH of the following two buffer solu- tions: (a) 2.0 M CH;COONA/2.0 M CH3COOH, (b) 0.20 M CH;COONA/0.20 M CH;COOH. Which is the more effective buffer? Why? 16.12