The pKa of MOPS is 7.20. Draw the equilibrium involved in the dissociation of the proton. 1. Suppose you dissolve 0.200 mol of MOPS in 1.00 Lof water. Calculate the pH of the solution. е. g. Use the pKa of MOPS to determine the ratio [A]/[HA] at pH 6.95. h. If you have 0.200 mol of MOPS dissolved in water, would you add NaOH or HCl to reach a pH of 6.95? And how many moles of the acid or base would you need to add? If you use a 100 mM MOPS buffer at pH 6.95 for a biochemical reaction which produces a maximum of 10 mM H*, which pH would you predict at the end of the reaction? i.

The pKa of MOPS is 7.20. Draw the equilibrium involved in the dissociation of the proton. 1. Suppose you dissolve 0.200 mol of MOPS in 1.00 Lof water. Calculate the pH of the solution. е. g. Use the pKa of MOPS to determine the ratio [A]/[HA] at pH 6.95. h. If you have 0.200 mol of MOPS dissolved in water, would you add NaOH or HCl to reach a pH of 6.95? And how many moles of the acid or base would you need to add? If you use a 100 mM MOPS buffer at pH 6.95 for a biochemical reaction which produces a maximum of 10 mM H*, which pH would you predict at the end of the reaction? i.

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter13: Acids And Bases

Section: Chapter Questions

Problem 9RQ: What is a salt? List some anions that behave as weak bases in water. List some anions that have no...

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What is a salt? List some anions that behave as weak bases in water. List some anions that have no basic properties in water. List some cations that behave as weak acids in water. List some cations that have no acidic properties in water. Using these lists, give some formulas for salts that have only weak base properties in water. What strategy would you use to solve for the pH of these basic salt solutions? Identify some salts that have only weak acid properties in water. What strategy would you use to solve for the pH of these acidic salt solutions? Identify some salts that have no acidic or basic properties in water (produce neutral solutions). When a salt contains both a weak acid ion and a weak base ion, how do you predict whether the solution pH is acidic, basic, or neutral?
he pka of MOPS is 7.20. Draw the equilibrium involved in the dissociation of the proton. f. Suppose you dissolve 0.200 mol of MOPS in 1.00 L of water. Calculate the pH of the solution. g. Use the pka of MOPS to determine the ratio [A']/[HA] at pH 6.95.
3. The pH of an acid solution is 6.20. Calculate the Ka for the acid. The initial acid concentration is 0.010 M. 4. What is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.26 at equilibrium? 5. Calculate the percent ionization of benzoic acid having the following concentrations: (a) 0.20 M, (b) 0.00020 M. 6. Calculate the percent ionization of Ammonium hydroxide, NH4OH at the following concentrations: (a) 0.60 M, (b) 0.0046 M, (c) 0.00028 M. Comment on the trends. 7. A 0.040 M solution of a monoprotic acid (HA) is 14% ionized. Calculate the ionization constant, Kc of the acid.8. (a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka = 3.0 x 10-4 .(b)The pH of gastric juice in the stomach of a certain individual is 1.00. After a few aspirin tablets have been swallowed, the concentration of acetylsalicylic acid in the stomach is 0.20M. Calculate the % ionization of the acid under these conditions.…
2. Write the equilibrium reaction (with water) of the following compounds and their corresponding Ka/Kb expression. a. HCN b. CH3NH₂ 3. Calculate the pH of the following solutions: a. 0.050 M HNO3 (K₁ = 24) b. 0.050 M HNO2 (K₂ = 4.0x104)
The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this problem: Write the acid dissociation equilibrium for the generic acid “HA” Set up an ICE chart ( with x = the concentration of H3O+ at equilibrium) Write the expression for Ka. Fill this in with the concentrations of H3O+, A- and HA at equilibrium, in terms of x. What is x? Can you find it from the given information? You should be able to use the pH to get the concentration of H3O+, which is x. Do this. Now that you know x, plug in into the Ka expression and find Ka.
3. Pyridine is a weak base with a Kb 1.7 x 109. If 0.300 moles of pyridine is added to 1.00 L o water, what will be the equilibrium concentrations of the species below: [Pyridine] = а. [Pyridine-H'] (the pyridinium ion) b. [OH-= С.
The experimental pH of a 0.25 M solution of potassium hydrogen phosphate, K2HPO4, is 10.25. a. Is the solution acidic, basic, or neutral? B. Write the balanced net ionic equilibrium reaction. Identify the acid, base, conjugate acid, and conjugate base. Write the cquilibrium expression Kb for the reaction. C. Look up the theoretical pKafrom the CRC Handbook. Please give me all questions solution fast
A 0.050 M solution of sodium meta-toluate (NaTol) has a pH of8.47. a. What is the Kb of meta-toluate ion?b. What is the Ka of meta-toluic acid (HTol)?
How much (in g) of Calcium hydroxide is required to increase the pH of a 100mL solution containing 0.1M each of acetic acid and sodium acetate by 1 pH unit? (Ka for acetic acid is 1.8 x 10-5; MW for Calcium hydroxide is 74.09 g/mol) а. О.606 g b. 5.52 x 10°g с. 0.818 g d. 0.303 g -5
1. A solution of 10.0 g each of formic acid (HCO₂H) and potassium formate (KCO₂H) dissolved in 1.0 L of water. Calculate the pH. The K, of formic acid is 1.8 x 10. a. Solve this problem using an ICE table. b. Solve this problem using the Hendersen-Hasselbalch Equation.
1. Write a chemical equation for the dissociation of the hypochlorite ion, ClO-1, in water to make a basic solution. 2. The Ka for benzoic acid (HC7H5O2), is 6.5 x 10-5. Calcuklate pH of a 0.10 M benzoic acid solution. 3. Calculate the pH of a 0.24 M solution of weak base A-1 that has a Kb of 2.5 x 10-6.
H. | || The percent ionization of chloroacetic acid is less than that of fluoroacetic acid. :*-C-C-ö-H The percent ionizations cannot be compared without knowing the concentrations of the two acids. The structure of haloacetic acids, XCH,COOH (where X is The percent ionizations cannot be compared without knowing the pH of the solution. either F, Cl, Br, or 1), is shown above. The dissociation constants and molar masses of four haloacetic acids are listed in the table below. The percent ionization of chloroacetic acid is greater than that of fluoroacetic acid. Acid pK. K. Molar Mass(g/mol) CLEAR ALL Fluoroacetic acid 2.59 2.57 x 10–3 78.0 Chloroacetic acid 2.87 1.35 x 10–3 94.5 Bromoacetic acid 2.90 1.26 x 10-3 138.9 lodoacetic acid 3.18 6.61 × 10-4 185.9 An aqueous solution contains small but equal concentrations of both chloroacetic and fluoroacetic acids. Which statement comparing the percent ionizations of the two acids in the solution is true? エーO-