Calculate the pH at 25 °C of a 0.44 M solution of lidocaine HCI (C14H2]NONH,CI). Note that lidocaine (C 4H2 NONH) is a weak base with a p K, of 7.94. Round your answer to 1 decimal place.
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- The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2. What is the pH of a 0.15 molar solution of this acid?Calculate the pH of a solution prepared by dissolving 1.15g of sodium acetate, CH3COONa, in 95.5 mL of 0.10 M acetic acid, CH3 COOH(aq). Assume the volume change upon dissolving the sodium is negligible. Ka of CH3COOH is 1.75 x 10-5.Calculate the pH of a solution that is prepared by diluting 0.140 moles of sodium benzoate to 1.00 litre in water. (The Ka of C6H5COOH is 6.3x10-5).
- For part, b would the calculations be the same for NO3^- (aq) and CO^2+ (aq), meaning those species PH would also equal 0?The pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar concentration of CH3COOH, if its acid ionization constant is Ka = 1.8×10–5?The pH of an aqueous solution of pyridine (C5H5N) is 10.0 at room temperature. What is the initial molar concentration of C5H5N, if its base ionization constant is: Kb = 1.7×10–9?
- Given that methylamine, CH3NH2, has a Kb of 4.4 x 10-4, what is the pH of a 0.20 M aqueous solution of methylamine?Acidic water can be treated with basic substances to increase the pH, although such a procedure is usually only a temporary cure. Calculate the minimum mass of lime, CaO, needed to adjust the pH of a small lake 1V = 4 * 109 L2 from 5.0 to 6.5. Why might more lime be needed?8. (a) HA(aq) is a weak acid with a dissociation constant, Ka, of 8.8 x 10−12. What is the pH of a 0.022 M solution of A−(aq)? The temperature is 25 ◦C. (b) For the reaction A(g) =A(l), the equilibrium constant is 0.666 at 25.0 ◦C and 0.222 at 75.0 ◦C. Making the approximation that the entropy and enthalpy changes of this reaction do not change with temperature, at what temperature will the equilibrium constant be equal to 0.777?
- calculate the pH of a solution prepared by dissolving 1.45g of sodium acetate, CH3COONa, in 99.0mL of 0.10M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75x10^-5Calculate the pH of a solution prepared by dissolving 1.75 g of sodium acetate, CH3COON,, in 53.5 mL of 0.15 M acetic acid, CH3COOH(aq). Assume the volume change upon dissolving the sodium acetate is negligible. Ka of CH3COOH is 1.75 x 10-5.What is the pH of 0.836 M anilinium hydrochloride (C6H5NH3CL) solution in water, given that Kb for aniline is 3.83 x 10-4?