General Chemistry
Improve your experience by picking them
Calculate the pH at the equivalence point of a 0.125 M solution of (CH3)2NH (dimethylamine) titrated with 0.125 M HCl. A volume of 0.125 M HCl equal to that of 0.125 M (CH3)2NH was used to achieve equivalence. Determine the suitable indicator for the said titration. The Ka for (CH3)2NH2+ is 1.86×10−11.
A 25.0 mL sample of 0.080 M (CH3)3N (Kb = 6.4×10–5) is titrated with 0.040 M HBr solution. What is the pH after 15.0 mL of the titrant has been added?
A 25.0 mL sample of 0.080 M (CH3)3N (Kb = 6.4×10–5) is titrated with 0.040 M HBr solution. What is the pH after 51.0 mL of the titrant has been added?
What is the pH at the equivalence when 0.150 M pyridine (C5H5N) is titrated with 0.150 M HCl solution?
What is the pH of the solution of 15.0 mL of 0.113 M aniline titrated with 5.0 mL of 0.156 M HNO3?
What is the pH of the solution of 15.0 mL of 0.113 M trimethylamine titrated with 2.0 mL of 0.156 M HNO3?
Calculate the pH at the equivalence point for the titration of a 75 mL sample of a 0.212 M C2H5NH2 solution with 0.12 M HBr.
Calculate the pH at the equivalence point for the titration of a 50.0 mL sample of 0.125 M NH3 with 0.120 M HCl.
What is the pH of the solution of 15.0 mL of 0.113 M trimethylamine titrated with 20.0 mL of 0.156 M HNO3?
Consider the titration of a 50.0 mL of 0.25 M aniline (C6H5NH2) solution with 0.125 M HBr. What is the pH of the solution before adding any acid?
Is the following solution acidic or basic? A solution is made by mixing 2.43 g of acetic acid (CH3COOH) in 25.0 mL of 1.43 M NaOH solution.
What is the pH of a solution prepared by mixing 30.0 mL of 0.200 M pyridine with 45.0 mL of 0.250 M HCl?
A 20.0 mL sample of 0.200 M triethylamine (Kb = 5.3 x 10–4) is titrated against 0.250 M HNO3 solution. What is the pH of the solution at the equivalence point?
Consider the titration of a 25.0-mL sample of 0.175 M CH3NH2 with 0.150 M HBr. Determine each quantity.
c. the pH at 5.0 mL of added acid
A 1.0-L buffer solution is 0.125 M in HNO2 and 0.145 M in NaNO2. Determine the concentrations of HNO2 and NaNO2 after the addition of each substance: a. 1.5 g HCl
Determine the predominant form of B for the titration of a 25.0 mL 0.15 M solution of a weak monoprotic base, B, with a 0.15 M solution of a strong monoprotic acid, HA, at the equivalence point
At the half-equivalence point, what is the pH of the titration of 15 mL of 0.183 M aniline with 0.15 M HNO3?
When 12.5 mL of 0.125 M weak base B is titrated with 0.125 M monoprotic strong acid HA, is the pH at the equivalence point less than, equal to, or greater than 7?
Calculate the volume (in mL) of 0.125 M HBr required to titrate 34.5 mL of 0.135 M CH3NH2 to the equivalence point.
Consider a weak base (B) that can only accept one proton from an acid. A 0.15 M solution of a monoprotic strong acid (HA) was used to titrate 50.0 mL of a 0.20 M solution of B. Calculate the amount (in mol) of HA needed to reach the equivalence point.
The image below shows the titration of a weak base with a strong acid.
How much acid was added for the equivalence point to be reached? What is the pH at this point?