Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO,H, pK = 5.0].(a) Which acid has the larger K? (b) Which acid is the stronger acid? (c) Which acid forms thestronger conjugate base? (d) When each acid is dissolved in water, for which acid does theequilibrium lie further to the right?%3DThe pKa values in Table 2.1 span a large range (-7 to 50). The pK, scale is logarithmic.small difference in pK, translates into a large numerical difference, For example, the diffebetween the pK, of NH3 (38) and CH2=CH, (44) is six pKa units. This means that NH, isone million times more acidic than CH,=CH,.

Given, pKa of HCOOH = 3.8 pKa of (CH3)3CCOOH = 5.0 a). Which has the larger Ka value = ? b).…

Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO;H, pK = 5.UJ. (a) Which acid has the larger K? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right?

Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO;H, pK = 5.UJ. (a) Which acid has the larger K? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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A 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.
The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 106 mo mo-when about a tenth of a mole of the acid is L dissolved in a liter of water. The chemical formulae of some acids are listed in the first column of the table below, and in the second column it says whether each acid is strong or weak. Complete the table. List the chemical formula of each species present at concentrations greater than about 10-6 mol/L when about a tenth of a mole of the acid is dissolved in a liter of water. acid strong or weak? species present at 10-6 mol/L or greater when dissolved in water ICIO weak H₂SO, weak IICI strong HCIO, strong ☐ x DO....
25) Consider 0.14 M monoprotic acid (HA) that is 12% ionized. (a) Show the reaction of dissociation (ionization) of HA (b) Calculate the [H+] in the solution. (c) Calculate the Ka of HA.
. The odor of spoiled butter is due in part to butanoic acid (HC4H7O2) which results from the breakdown of the fat in butter. A 0.100M solution of butanoic acid is 1.23% ionized. Write the chemical equation for the ionization of this acid in water. Write the Ka expression for this acid. What is the equilibrium concentration of each product and the reactant?
(a) Define a Lewis acid and a Lewis base. (b) Define an Arrhenius acid and an Arrhenius base. (c) Identify As2O5 as either a Brønsted-Lowry, a Lewis, or an Arrenius acid or base, and justify your answer to part (c) by writing a balanced chemical equation in showing As2O5 added to water.
A solution is made by dissolving 44.1 g of Ba(NO₂)₂ in 500.0 mL of water. (a) Does Ba²⁺ have any acidic or basic properties? (b) Does NO₂⁻ have any acidic or basic properties? (c) As NO₂⁻ is a base, write the basic equilibrium equation that exists in solution (d) What is the value of Kb for NO₂⁻? The Ka of HNO₂ is 4.5 × 10⁻⁴. (e) Determine the pH of the solution
At pH = 3.9, a weak acid has a concentration of 0.75 M. If the pKa = 4.5, what is the concentration of the conjugate base?
Calculate the pH of a solution that is (a) 0.0100 M in HCl and 0.0200M in picric acid. (b) 0.0100 M in HCl and 0.0320 M in benzoic acid. (c) 0.0100 M in NaOH and 0.075 M in Na,CO3. (d) 0.0100 M in NaOH and 0.090M in NH3.
The pKa of a weak acid, HA is 8.60, for a 0.100 M HA solution: (A) it is acidic (B) it is basic (C) pH = 8.60 (D) pH = 4.30
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6. (a) Write an equation where calcium acetate is adding to water. (b) Looking at the equation in (a), is this salt acidic, basic or neutral? (c) Determine the pH of a solution of calcium acetate, Ca(CH₂COO), that is 0.275 M. (Ka for CH₂COOH is 1.8 x 105).