The following Ka values are given for the benzoic acids below: 38.10-5 - 29.10-5- 6.10-5 - 3,4.10-5 Assign the Ka values for each benzoic acid, justifying your answer. COOH COOH OCH3 COOH NO₂ COOH CN
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- Nitric acid (HNO3) is a strong acid that completely ionizes when dissolved in water (pKa = -1.30). Calculate the pH of 10 mg/L HNO3. a. Unlike nitric acid, butyric acid (CH3CH2CH2COOH) is a weak acid (pKa = 4.8). Calculate the pH of a solution when 90% of the CH3CH2CH2COOH is dissociated. b. Briefly explain how you can use the pKa values of these two molecules to determine that nitric acid is a strong acid, while butyric acid is a weak acid.Aniline C6H5NH2 has a base dissociation constant (Kb) of 4.3 × 10-10. What is the conjugate acid of aniline and what is its acid dissociation constant (Ka)? (SHOW CALCULATION)Benzoic acid (C6H5C02H) has Ka =6.3 x 10-5 a) What is the value of Kb for the benzoate ion (C6H5C02-)? b) What is the h30+ concentration of a O, 10 mol/dm3 solution of benzoic acid? c) What is the pH of the solution in (b) above?
- Taking Ka for acidic acid as 1.8 x 10-5, calculate H3O+ , using the known concentraions of acidic acid and soudium acecate contained in reaction mixtures 1 and 4. Reaction mixture time (s) Acidic acid concentration (mol/L) sodium acetate concentration (mol/L) calculated H3O+ concentration 1 237 0 1 x 10 -5 4 236 1 x 10 -4 1 x 10 -5Write equations for the following acid-base reactions. Label the conjugate acids and bases, and show any inductive stabilization. Predict whether the equilibrium favors the reactants or products. Try to do this without using a table of pKa values, (a) CH3CH2OH + CH3NH- (b) F3CCOONa + Br3C¬COOH(c) CH3OH + H2SO4 (d) NaOH + H2S(e) CH3NH3+ + CH3O- (f) BrCH2CH2OH + F3C¬CH2O-(g) NaOCH2CH3 + Cl2CHCH2OH (h) H2Se + NaNH2(i) CH3CHFCOOH + FCH2CH2COO- (j) CF3CH2O- + FCH2CH2OHGiven a Ka value of 1.3 X 10-10 for phenol (a benzene with an alcohol group on it-aromatic alcohols are acidic-who knew?), what is its pKa? 7.20 8.75 6.80 9.89
- Phthalic acid and isophthalic acid have protons on two carboxy groupsthat can be removed with base. (a) Explain why the pKa for loss of thefirst proton (pKa1) is lower for phthalic acid than isophthalic acid. (b)Explain why the pKa for loss of the second proton (pKa2) is higher forphthalic acid than isophthalic acid.According to the Evan's pKa table, phenol has a pKa of 9.95. p-Nitro and m-nitrophenol have pKas of 7.14 and 8.35 respectively. Using resonance structures, explain the observed trends in the acidity of these molecules.Given that Ka for acetic acid is 1.8 * 10-5 and that for hypochlorous acid is 3.0 * 10-8, which is the stronger acid?
- Calculate delt G for a.) CH3NH2(aq) + H2O (l) -> CH3NH3+ (aq) + OH-(aq) T= 25C kp= 4.4x 10-4 b.) Pbl2(s) + Pb2+(aq) +2I-(aq) T= 25C Kp= 8.7x10-9Given the Ka values (in parentheses) for the following acids: HSO4– (Ka= 1.2 x 10–2); HNO2 (Ka= 4.0 x 10–4); HC2H3O2 (Ka= 1.8 x 10–5); Calculate Kc values for the following acid-base equilibria: (a) HSO4–(aq) + C2H3O2–(aq) ⇌ HC2H3O2(aq) + SO42–(aq) (b) HC2H3O2(aq) + NO2–(aq) ⇌ HNO2(aq)+ C2H3O2–(aq)A) Phenol Red is a weakly acidic dye which is yellow in the HA form and red in the A form. What concentration of Phenol Red is required to obtain an absorbance of 0.50 at 550 nm at pH 7.8? Note: ε550 of A = 2.5 x 104 M-1 cm-1; ε550 of HA = 0; pKa = 7.8. B) What would the absorbance of the solution in part (a) be if the pH was 8.8?
