Calculate (to the nearest 0.1%) the proportion of a dose of ebastine (pKa of conjugate acid = 10.3) that will be ionised at pH 7.7. You do not need to include "%" in your answer.
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Calculate (to the nearest 0.1%) the proportion of a dose of ebastine (pKa of conjugate acid = 10.3) that will be ionised at pH 7.7. You do not need to include "%" in your answer.
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- 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.a) If the Kb of a weak base is 4.7E-9, what is the Ka of its conjugate acid? Do not include any units with your answer. Your answer should have two significant figures. For scientific notation use the same as that in the problem (i.e. 3.3E-2 is the same as 3.3 x 10-2). b) Diethylamine, (CH3CH2)2NH, has a Kb of 8.6 x 10-4. What is the pH of a 0.22 M solution of diethylammonium chloride, [(CH3CH2)2NH2]Cl? Your answer should be to two places past the decimal point.The pKas of the conjugate acids of -OH (conjugate acid H2O) and HPO42- (conjugate acid H2PO4-) are 15.7 and 6.8, respectively. First, identify which is the strong base, and which is the weak base. Then, explain how you can use these pKa values to help you identify which compounds will be separated at each step.
- Given that pKb for nitrite ion (NO-2) is 10.85, find the quotient [HNO2]/[NO-2] in a solution of sodium nitrite at (a) pH 2.00; (b) pH 10.00.The pKa of NH4+ is 9.25. Predict whether the acid form (NH4+) or the base form (NH3) is predominant at pH = 7.4. Explain.If the concentration of an acid in solution is 2.2 times larger than the concentration of its conjugate base, and the pH of the solution is 3.5, what is the pKa of the acid? Include the answer to 3 significant figures
- What is the pKa of benzoic acid? What is the molar concentration of sodium benzoate (conjugate base)? What is the molar concentration of benzoic acid (weak acid)?If I’ve got 20.0 grams of tartaric acid with a (first ionization) pKa = 2.91. If I dissolve this into 1.000 Liter of solution what will the pH of the solution be?(a) Given that Ka for acetic acid is 1.8 x 10-5 and that forhypochlorous acid is 3.0 x 10-8, which is the stronger acid?(b) Which is the stronger base, the acetate ion or the hypochloriteion? (c) Calculate Kb values for CH3COO- and ClO-.
- For a solution of formic acid, a weak acid with a pKa of 8.74, at what pH will the concentration of formic acid be equal to the concentration of formate, the conjugate weak base of formic acid. Report the value using 3 significant figures.1) Consider the reaction AH(+) + H₂O → A: + H₂O¹. For the following named acids: 1) draw the structure of the acid, 2) give the approximate pKa of the conjugate acid (±1 pKa unit), 3) give the name of the conjugate base, and 4) draw the structure of the conjugate base. For the purposes of answering this question you may use pKa values evenly divisible by 5. Acetylacetone pKa acid Conj. base acid Conj. base iso-Butyl amine pKa Imidazolium cation pKa sec-butyl oxonium pKa t-Butyl Acetoacetate pKa iso-propanol pka_ Ethyl Acetate pKa Anilinium cation pKaCalculate the pH of a 0.35 M solution of hydrocyanic acid (HCN), which has a pKa of 9.31. Your answer should have 3 significant figures (i.e. 9.99).