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- 1) Calculate the pH (aq., 25 °C) of a 0.073 M Novocaine (C13H21O2N2CI) solution, which is the salt of the base procaine and hydrochloric acid. The pKb of procaine = 5.155. oltion (lom 2) Calculate the pH (aq., 25 °C) of a 0.100 M potassium hypochlorite solution. The pKa of hypochlorous acid = 7.54.You are given two glasses of water that have different temperatures. The temperature of the first glass is at 298 K, while the second glass has a temperature of 303 K. It has been determined that the Kw value for the second glass of water is 1.47 x 10-¹4. Which of the following statements is true? (a) The pH of the room temperature glass is higher, but both glasses have the same acidity. (b) The room temperature glass of water has a higher pH, and is more basic than the other glass of water. (c) Both glasses of water are neutral, so both will have a pH of 7.00. (d) The room temperature water has a lower pH, so is more acidic. (e) The warmer glass of water has a lower pH, and is more acidic than the other glass of water.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?
- You prepared 500 mL buffer solution that contains 0.50 moles monoprotic weak acid (HA) and 0.30 moles conjugate base (NaA). The solution has a pH of 4.20. (a) What is the Kp of the conjugate base, NaA? (b) What is the pH of the buffer solution after adding 400 mL of 0.30 M H,SO4? pH = pKa – log(THA), [A*]6. (i) Define pH in words. The strong acid HClag has a pH value of 1, use the following equation for a strong acid: HClaa Hog + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H+] Clea (ii) Use the above expression to deduce the pH of HCl (ag) given the concentration of the acid to be 4.5 mol/dm³ pH =Calculate the pH of a 18 M NaCH3COO(aq) (sodium acetate salt of acetic acid) at 25oC. The acid ionization constant for acetic acid is Ka= 1.8×10–5. Enter your answer with correct units and significant figures.
- Sodium lactate is the sodium salt of lactic acid.a) Use Acid-Base Properties of Salt Solutions, to explain if sodium lactate, NaC3H5O3(aq), is acidic or basic?b) Use ICE table to determine what is the pH of a solution that contains 0.75mol/L lactic acid, HC3H5O3(aq) (Ka = 1.4 x 10-4), and 0.25mol/L sodium lactate, NaC3H5O3(aq) ?6. (i) Define pH in words. The strong acid HClahas a pH value of 1, use the following equation for a strong acid: H+, + and convert the following expression to deduce the hydrogen ion concentration: pH = -log10 [H*] (ii) Use the above expression to deduce the pH of HCL (ag) given the concentration of the acid to be 4.5 mol/dm3 pH =so Please don't provide handwritten solution
- What is the pH of a buffer solution that contains 0.305 M of a fictitious weak acid and 0.469 M of its conjugate base? The pK a of the acid is 4.275.The pH of a 0.016-Maqueous solution of p-toluidine (CH3 CH,NH3 ) is 8.60. Calculate Kp. K, =What is the molarity of a 12.46 mL sulfuric acid solution of 18.22 mL of 0.100 M potassium hydroxide is required to reach the endpoint as indicated by a titration? Given attached equation