Given that HO(CH2)2COOH has a pKa = 4.5 and HO(CH2)2 NH3 has a pKa = 9.5, answer the following: %3D %3D What pH would you make the water layer in order to cause both compounds to dissolve in it? Water should have pH 6.5 - 7.5. Water should have pH 4.5 - 9.5. Water should have pH 4.5 - 7.5. Water should have pH 6.5 - 9.5. What pH would you make the water layer in order to cause the acid to dissolve in the water layer and the amine to dissolve in the ether layer? Express your answer using one decimal place. ΑΣφ ? pH > What pH would you make the water layer in order to cause the acid to dissolve in the ether layer and the amine to dissolve in the water layer? Express vour answer using one

Given that HO(CH2)2COOH has a pKa = 4.5 and HO(CH2)2 NH3 has a pKa = 9.5, answer the following: %3D %3D What pH would you make the water layer in order to cause both compounds to dissolve in it? Water should have pH 6.5 - 7.5. Water should have pH 4.5 - 9.5. Water should have pH 4.5 - 7.5. Water should have pH 6.5 - 9.5. What pH would you make the water layer in order to cause the acid to dissolve in the water layer and the amine to dissolve in the ether layer? Express your answer using one decimal place. ΑΣφ ? pH > What pH would you make the water layer in order to cause the acid to dissolve in the ether layer and the amine to dissolve in the water layer? Express vour answer using one

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section16.7: Calculations With Equilibrium Constants

Problem 16.5CYU: What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M...

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At what pH is the concentration of a compound, with a pKa = 3.7, 10 times greater in its acidic form than in its basic form?
Consider the acid HXOy where X is a halogen that is less electronegative than oxygen. Which of the following gives the relationship between Ka of the acid and the value of y and gives the correct reasoning? As y increases the value of Ka increases because the conjugate base of the acid becomes less stable. As y increases the value of Ka increases because the conjugate base of the acid becomes more stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes less stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes more stable.
For an acid HA with a pKa of 5.2, what is the ratio of the concentration of the conjugate base to that of the acid at pH 7.2.
Given a buffer solution with the pH of 6.5 and pKa of 5.9, calculate the ratio of conjugate base to acid of this buffer solution (show step-by-step).
4. Calculate pH of water solution of Hydrosulphuric acid with concentration of 0,050 M (pKa=6.99)
Calculate the pH at 25°C of a 0.68 M solution of potassium butanoate (KC3H7CO2). Note that butanoic acid (HC3H7CO2) is a weak acid with a pKa of 4.82.
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In my slide, there is a table summarizing the pKa values for different acids. (1) when ranking the acidity level (how strong the acids are), a low pKa means high acidity. Why is that? (2) Calculate the phosphoric acid solution pH when the ratio of [H2PO4-]/[H3PO4] is 0.8.
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What is the pKb of an unknown weak acid if the pH of the solution was measured to be 4.52. when [HA]=0.540 and [A-]=0.580.
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A dilute (~0.10 M) butanoic acid solution (aka butyric acid) has a pH of 4.6. To the nearest hundredth of a unit, what is the ratio of the acidic form to basic form of the molecules at this pH? (The pKa of butanoic acid is 4.82.)