Consider the titration of 30.0 mL of 0.20 M nitrous acid by adding 0.0500 M aqueous ammonia to it. The pH at the equivalence point is _____. (Note: This is the titration of a weak acid with a weak base.)
(a) greater than 7
(b) equal to 7
(c) less than 7
(d) cannot be determined without more data (not including Ka and Kb)
(e) is impossible to predict
We need at least 10 more requests to produce the answer.
0 / 10 have requested this problem solution
The more requests, the faster the answer.
Consider the titration of 30.0 mL of 0.20 M nitrous acid by adding 0.0500 M aqueous...
A. Match each type of titration to its pH at the equivalence point. Weak acid, strong base Strong acid, strong base Weak base, strong acid pH less than 7 pH equal to 7 pH greater than 7 B. A 56.0 mL volume of 0.25 M HBr is titrated with 0.50 M KOH. Calculate the pH after addition of 28.0 mL of KOH. C. Consider the titration of 50.0 mL of 0.20 M NH3 (Kb=1.8 x 10^-5) with 0.20 M HNO3....
A student is asked to determine the value of Ka for nitrous acid by titration with potassium hydroxide. The student begins titrating a 48.3 mL sample of a 0.360 M aqueous solution of nitrous acid with a 0.216 M aqueous potassium hydroxide solution, but runs out of standardized base before reaching the equivalence point. The student's last observation is that when 53.2 milliliters of potassium hydroxide have been added, the pH is 3.603. What is Ka for nitrous acid based...
A student is asked to determine the value of Ka for nitrous acid by titration with barium hydroxide. The student begins titrating a 33.0 mL sample of a 0.437 M aqueous solution of nitrous acid with a 0.204 M aqueous barium hydroxide solution, but runs out of standardized base before reaching the equivalence point. The student's last observation is that when 24.4 milliliters of barium hydroxide have been added, the pH is 3.663. What is Ka for nitrous acid based...
In a titration of 41.42 mL of 0.3164 M nitrous acid with 0.3164 M aqueous sodium hydroxide, what is the pH of the solution when 41.42 mL of the base have been added?
1)A 10.0 mL sample of 0.25 M NH3(aq) is titrated with 0.20 M HCl(aq) (adding HCl to NH3). Determine which region on the titration curve the mixture produced is in, and the pH of the mixture at each volume of added acid.Kb of NH3 is 1.8 × 10−5.Henderson–Hasselbalch equation:Part a):1) After adding 10 mL of the HCl solution, the mixture is [ Select ] ["at", "before", "after"] the equivalence point on the titration curve.2) The pH of the solution after...
5. What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL of an aqueous weak acid requires 29.80 mL of 0.0567 M NaOH? Ka = 3.2 x 10-4 for the weak acid.
pH after titration question A 30.1 mL sample of a 0.540 M aqueous nitrous acid solution is titrated with a 0.306 M aqueous barium hydroxide solution. What is the pH after 9.91 mL of base have been added?
what is the pH of a titration if 12.5 mL of 0.0500 M NaOH solution is added to 40.00 mL of 0.100 M solution of nitrous acid (HNO2) Ka=6.0 x 10-4?
A 40.0 mL solution of 30.0 M of succinic acid (aq) is titrated with 0.300 M of KOH. Find the pH of the solution. (pKa=4.2). A) initially B) 1/2 way to the equivalence point C) at the equivalence point D) 1.00 mL past the equivalence post 2) sketch the titration curve that results from above titration. Label A) only a weak base present. B) Buffer. C) Only a weak acid present. D) Strong base in excess. E) pH = pKa
Calculate the pH of a 0.383 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4) and the equilibrium concentrations of the weak acid and its conjugate base. pH = [HNO2 ]equilibrium = M [NO2- ]equilibrium = M