PH= -log[H+]
HCl(aq) -------> H+(aq) + Cl-(aq)
Given: [H+] = 1.6 x 10-2M
PH= -log[H+] = -log[1.6 x 10-2] = -log(1.6) - log(10-2) [since , log(axb) = loga + logb and logab = b loga]
=-0.204-(-2log10) [ log10=1]
PH =2-0.204= 1.795
Be sure to answer all parts. Calculate the pH of a solution that is: 1.6 x...
Be sure to answer all parts. Calculate the pH of 1.00 L of the buffer 0.94 M CHCOONa/0.92 M CH,COOH before and after the addition of the following species. (Assume there is no change in volume.) (a) pH of starting buffer: (b) pH after addition of 0.065 mol NaOH: (c) pH after further addition of 0.117 mol HCI: Prey 10 of 10
Be sure to answer all parts. The pH of a saturated solution of a metal hydroxide MOH is 10.60. Calculate the Kn for this compound x 10 Enter your answer in scientific notation.
Be sure to answer all parts. The pH of an aqueous acid solution is 6.24 at 25°C. Calculate the Ka for the acid. The initial acid concentration is 0.010 M. × 10 (Enter your answer in scientific notation.)
Be sure to answer all parts. The pH of a saturated solution of a metal hydroxide M(OH)2 is 8.950. Calculate the Ksp for this compound. Enter your answer in scientific notation.
Be sure to answer all parts. Determine the pH of a solution at 25°C in which the hydroxide ion concentration is (a) 4.5 x 10-8 M (b) 9.9 x 10-9 M 10-11 M (c)2.5
Be sure to answer all parts. An aqueous solution of a strong base has pH 10.88 at 25°C. Calculate the concentration of base in the solution: (a) if the base is LiOH. [LiOH] = M (b) if the base is Ba(OH)2. [Ba(OH)2] = × 10 M (Enter your answer in scientific notation.)
Be sure to answer all parts. In a 0.25 M solution, a weak acid is 3.6% dissociated. (a) Calculate the [H30+ ], pH, [OH ], and pOH of the solution. [H30+]= M [OH]= X 10 pH = pOH = (b) Calculate Kg of the acid. KA=
Be sure to answer all parts. Calculate the pH of each of the following solutions. (a) 4.1 × 10−4 M Ba(OH)2: × 10 (Enter your answer in scientific notation.) (b) 2.3 × 10−4 M HNO3:
Be sure to answer all parts. Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid: (a) 3.00 ml pH- (b) 29.60 mL pH = (C) 38.00 mL pH-
Be sure to answer all parts. Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after the following additions of acid: (a) 4.00 mL pH = (b) 29.00 mL pH = (c) 36.00 mL pH =