(a)
Interpretation:
Using the buffer index expression, the value of the buffer index for acetic acid buffer needs to be determined.
Concept introduction:
The buffer index is defined as the ratio of the increase in the concentration/amount of the strong acid or base added to the buffer with a change in the pH value. When a strong acid or base is added to the buffer solution, the change in the buffer index can be represented as follows:
Here,
(b)
Interpretation:
The pH of the buffer after the addition of strong acid needs to be determined.
Concept introduction:
The buffer index is defined as the ratio of the increase in the concentration/amount of the strong acid or base added to the buffer with a change in the pH value. When a strong acid or base is added to the buffer solution, the change in the buffer index can be represented as follows:
Here,
(c)
Interpretation:
A graph between buffer index and pH needs to be plotted indicating the minimum and maximum buffer indices.
Concept introduction:
The buffer index is defined as the ratio of the increase in the concentration/amount of the strong acid or base added to the buffer with a change in the pH value. When a strong acid or base is added to the buffer solution, the change in the buffer index can be represented as follows:
Here,
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Chapter 17 Solutions
EBK GENERAL CHEMISTRY
- The simplest amino acid is glycine, H2NCH2CO2H. The common feature of amino acids is that they contain the functional groups: an amine group, -NH2, and a carboxylic acid group, -CO2H. An amino acid can function as either an acid or a base. For glycine, the acid strength of the carboxyl group is about the same as that of acetic acid. CH3CO2H, and the base strength of the amino group is slightly greater than that of ammonia, NH3. (a) Write the Lewis structures of the ions that form when glycine is dissolved in 1 M HCl and in 1 M KOH. (b) Write the Lewis structure of glycine when this amino acid is dissolved in water. (Hint: Consider the relative base strengths of the -NH2 and -CO2- groups.)arrow_forwardThe titration of 100.mL of 0.100 M NH3 (in the flask) with 0.200 M HCL (in the burette) was carried out. Calculate the pH solutions at the following volumes of HCL addedarrow_forwardConsider the titration of a 50.00 mL sample of 0.100 M ethylamine, C2H5NH2, with 0.100 M HCl (aq., 25 oC). The Kb C2H5NH2 = 6.41 x 10–4. What is the pH after 25.00 mL of HCl has been added?arrow_forward
- Define and explain the significance of the equivalence point of a titration. Identify the role of the indicator in this context.arrow_forwardWhich statement describes the action of a buffer composed of acetic acid (CH3COOH) and sodium acetate (NaCH3COO)? How does a buffer resist change in pH upon addition of a strong acid? By titration, it is found that 73.3 mL of 0.189 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq). Calculate the concentration of the HCl solution.arrow_forwardIn a titration, the equivalence point is the moment at which the number of moles of H+ from the acid that has been added is equal to the number of moles of OH- from the base that has been added. Remember that in a molecule like H2SO4, there are 2 moles of H+ per mole of H2SO4. 16.31 mL of 0.100M H2SO4(aq) is placed in a beaker. After 17.98 mL of NaOH is added to the beaker, the equivalence point is reached. What is the concentration (M) of the NaOH solution?arrow_forward
- A chemistry graduate student is given 450. mL of a 0.50M trimethylamine ((CH3)N) solution. Trimethylamine is a weak base with K₁=7.4 × 10¯ª. What mass of (CH3)NHBr should the student dissolve in the (CH3)2N solution to turn it into a buffer with pH = 11.20? You may assume that the volume of the solution doesn't change when the (CH3) NHBr is dissolved in it. Be sure your answer has a 3 unit symbol, and round it to 2 significant digits. ? 10: 000arrow_forwardA chemistry graduate student is given 500. mL of a 1.80M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,= 4.9 x 10 – 10 What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH =9.70? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 国 国 回arrow_forwardWhat is the molar solubility (in mols/L)of silver chloride in 2.00 M NH3(aq) given that Kgp of AGCI = 1.77x10-10 and Kf of Ag(NH3)2* is 1.70×107? Express your answer in decimal notation rounded to three significant figures.arrow_forward
- A chemistry graduate student is given 500. mL of a 1.50M chlorous acid (HClO₂) solution. Chlorous acid is a weak acid with K=1.1 × 10 KClO₂ should the student dissolve in the HClO₂ solution to turn it into a buffer with pH = 1.87? You may assume that the volume of the solution doesn't change when the KClO₂ is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. 1 85°F Explanation Partly sunny 3 Check S x10 X с % 5 T F6 Q Search F7 & L 1 F8 a * O F9 F10 © 2023 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Acces % Co 楽- F11 *+ F12 PrtSc W + What mass of Insert ^ Delete Backspacearrow_forwardA chemistry graduate student is given 450. mL of a 1.70M hydrocyanic acid (HCN) solution. Hydrocyanic acid is a weak acid with K,= 4.9 × 10 ". What mass of KCN should the student dissolve in the HCN solution to turn it into a buffer with pH = 8.97? You may assume that the volume of the solution doesn't change when the KCN is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits.arrow_forwardOne drop, 0.200 cm3, of 1.00 mol dm-3 of aqueous sodium hydroxide, NaOH, solution is added to 25.0 cm3 of a phosphate buffer that is 0.040 mol dm-3 in KH2PO4(aq) and 0.020 mol dm-3 in K2HPO4(aq). Calculate the resulting pH of the solution given that the second acid dissociation constant, pKa2, for phosphoric acid is 7.21.arrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax