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Q: For an acid with a pKa of 5.00, what is the pKb of its conjugate base?
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Q: . For the following acid-base reaction, i) complete the acid-base reaction by writing the products…
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1) High pKa value means weak acid,
low pKa value means strong acid.
2) Strong acid have weak conjugate base
and Weak acid have strong conjugate base.
And a conjugate base is always a stronger nucleophile.
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- What is the conjugate acid of acetamide and its pka value?Acetic acid can also react as a very weak base (pKb = 20). Two different sites on acetic acid might become protonated to give the conjugate acid. Draw both of these possible conjugate acids, and explain (resonance) why the correct one is more stable. Calculate the pKa of this conjugate acid.Treatment of indene with NaNH2 forms its conjugate base in a Brønsted– Lowry acid–base reaction. Draw all reasonable resonance structures for indene's conjugate base, and explain why the pKa of indene is lower than the pKa of most hydrocarbons.
- Treatment of indene with NaNH2 forms its conjugate base in a Brønsted–Lowry acid–base reaction. Draw all reasonable resonance structures for indene’s conjugate base, and explain why the pKa of indene is lower than the pKa of most hydrocarbons.Calculate the pKa of a acid at 25°C if its conjugate base has a pKb = 1.19Arrange the compounds in each set in order of increasing base strength. consult Table 4.1 for pKa values of the conjugate acid of each base.
- explain in great detail why the pKa values are what they are and compare them among the three compounds. The conjugate acids that are protonated are drawn in red for each compound. Which one based on the pKa is most acidic and what does that tell you about how basic their lone pairs are?What percent of acetic acid is present in the acidic form at pH 5.0, assuming a pKa of 4.8?The pKa of our product is ~ 2-3 units lower than the pKa of phenol. Draw all possible resonance structures of the conjugate base of the product, and use these to explain why our product is so much more acidic than phenol.
- Which acid do you think would have the lower pKa value: HBrO4, HBrO3, HBrO2, or HBrO? Explain your answer.Verify that the equilibrium position for the reaction between phenol and hydroxide ion is on the right by comparing the pKa value of the acid on the left with that of the acid on the right. Which acid is stronger? do the same for the reaction of phenol with hydrogen carbonate ionWhich is the conjugate base in each of the pairs below?