Concept explainers
(a)
Interpretation:
The equilibrium constant of various acid-base reactions has to be calculated.
Concept introduction:
An integer that shows the correlation between quantity of starting material and product of a reversible reaction present at equilibrium is called equilibrium constant.
To give: Equilibrium constant of strong acid reacts with strong base.
(b)
Interpretation:
The equilibrium constant of various acid-base reactions has to be calculated.
Concept introduction:
An integer that shows the correlation between quantity of starting material and product of a reversible reaction present at equilibrium is called equilibrium constant.
To give: equilibrium constant of strong acid reacts with weak base(
(c)
Interpretation:
The equilibrium constant of various acid-base reactions has to be calculated.
Concept introduction:
An integer that shows the correlation between quantity of starting material and product of a reversible reaction present at equilibrium is called equilibrium constant.
To give: equilibrium constant of weak acid (acetic acid) reacts with strong base.
(d)
Interpretation:
The equilibrium constant of various acid-base reactions has to be calculated.
Concept introduction:
An integer that shows the correlation between quantity of starting material and product of a reversible reaction present at equilibrium is called equilibrium constant.
To give: Equilibrium constant of weak acid (acetic acid) reacts with weak base (
Want to see the full answer?
Check out a sample textbook solutionChapter 17 Solutions
CHEMISTRY:ATOMS FIRST-W/ACCESS>CUSTOM<
- 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 ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2. What is the pH of a 0.15 molar solution of this acid?arrow_forwardAn organic acid(HA) has a molecular weight of 100. g mol^-1, a Kow=5.6 and a Ka=2.7x10^-2. If originally 2.0g of the acid is dissolved in 100mL of octanol (there is no dissociation in octanol), which is then placed in contact with 100mL of water, what will be the pH of the water? (consider the equilibrium processes to be sequential and unrelated chemically)arrow_forward
- Calculate the pH and pOH of a solution resulting from dissolving 0.75 grams of perchloric acid in enough water to obtain a final solution of 1500 mL. Take into account that for each mole of perchloric acid it dissociates in the aqueous medium, releasing 1 mole of hydrogen ions.arrow_forwardA 0.025 M solution of an unknown organic acid has a pH of 3.23. 2.1 By means of a full calculation, determine the value of the ionisation constant of the conjugatebase of this acid..- You may use “HA” to denote the formula of the acid.- You may make certain assumptions to simplify your calculations2.2 A certain amount of the sodium salt of the conjugate base of the acid was added to the system.Will the pH of the resulting solution increase or decrease, compared to the original given value? Explain your answer in a short sentence or two.arrow_forwardAt 250°C, the equilibrium constant for the dissociation of water is 10–11.16. At this temperature, what is the pH of a neutral solution?arrow_forward
- What is the significance of the Henderson-Hasselbalch equation in acid-base chemistry, and how does it relate to the pH of a solution?arrow_forwardThe pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar concentration of CH3COOH, if its acid ionization constant is Ka = 1.8×10–5?arrow_forwardCalculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in 95.5 mL of 0.10 M acetic acid, CH3 COOH(aq). Assume the volume change upon dissolving the sodium is negligible. Ka of CH3COOH is 1.75 x 10-5.arrow_forward
- Acidic water can be treated with basic substances to increase the pH, although such a procedure is usually only a temporary cure. Calculate the minimum mass of lime, CaO, needed to adjust the pH of a small lake 1V = 4 * 109 L2 from 5.0 to 6.5. Why might more lime be needed?arrow_forwardCalculate the pH of the following acid solutions at 25 °C: (a) 1.0 x 10-4 M H3BO3(aq) (boric acid acts as a monoprotic acid), (b) 0.015 M H3PO4 (aq), (c) 0.10 M H2SO3(aq). Values for the successive acidity constants for each of these acids are given in the below table.arrow_forwardThe 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 aseither 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.arrow_forward
- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStaxChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage LearningGeneral Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning