What is the pH of a solution that results from diluting 0.30 mol of CH.CO-H and

Question

What is the pH of a solution that results from diluting 0.30 mol of CH.CO-H and 0.20 mol of NaCH CO2 with water to a volume of 1.0 L? (K, of CH COH 1.8x 10) a. 4.35 b. 4.57 c. 4.74 d. 4.92 e. 5.14 2. Which of the following conditions is/are met at the equivalence point of the titration of a monoprot strong acid with a monoprotic weak base? 1. 2. 3. a. only b. 2 only c. 3 only d. 1 and 2 e. 1 and 3 The moles of acid added from the buret equals the initial moles of base. The pH of the solution is equal to 7.00 at the equivalence point. The pH of the solution is less than 7.00 at the equivalence point. 33. The Kp of Agl is 8.5 x 10 1" at 25 °C. Calculate the molar solubility of Agl in 0.0045 M KI(aq) at 25 °C. a. 1?9 × 10-14 mol/L b. 3.8 10-12 mol/L c. 9.2 x 10 mol/L. d. 1.4×10-7 mol/L c. 2.0 x 10 mol/L 34. Which of the following statements is/are CORRECT? I. 2. Spontaneous changes occur in the direction that leads away from equilibrium. The second law of thermodynamics states that there is maximum disorder in a perfect crystal at 0 K 3. In a spontaneous chemical reaction the entropy of the universe always increases. a. 1 only b. 2 only c. 3 only d. 1 and 3 e. 1, 2, and 3 35. Which one of the following processes involves the largest increase in the entropy of the system? a. 3 H2(g)+N2g2 NHs(g) b. N2(g) 2 02(g)2 NO(g) c. 2 Ag O(s)4 Ag(s) +0g) d. CaO(s) + CO2(g)-> CaCO i(s) e, 2 Na(s) + Cl2(g) ? 2 NaCl(s)

Explanation / Answer

Ans 1

Molarity of acid CH3CO2H = moles/Volume

= 0.30 mol / 1L = 0.30 M

Molarity of base NaCH3CO2 = moles/Volume

= 0.20 mol / 1L = 0.20 M

Acid dissociation constant Ka = 1.8*10^-5

pKa = - log Ka = - log ( 1.8*10^-5) = 4.74

From the Henderson-Hasselbalch equation

pH = pKa + log [base / Acid]

= 4.74 + log (0.20/0.30)

= 4.57

Option B is the correct answer

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