Find the pH of a solution made by adding 40 mmoles of KOH to 1.50 L of 0.025M nicotinic acid (pKa1 = 2.03, pKa2 = 4.82). Assume no change in volume on mixing.
1)
moles of nicotinic acid = 1.50 x 0.025 = 0.0375
moles of KOH = 40 mmol = 0.0400
H2A + KOH -------------> HA- + H2O
0.0375 0.0400 0 0
0 0.0025 0.0375
HA- + KOH -------------> A2- + H2O
0.0375 0.0025 0 0
0.035 0 0.0025
pH = pKa2 + log [base / acid]
= 4.82 + log [0.0025 / 0.035]
pH = 3.67
Find the pH of a solution made by adding 40 mmoles of KOH to 1.50 L...
Find the pH of a solution prepared by adding 1.0 L of 0.10 M butyric acid to 0.50 L of 0.10 M NaOH. (Ka = 1.5 x 10-5) A. 12.69 B. 7.00 C. 2.41 D. 4.82 E. 13.35
What is the pH of a solution containing 0.831 mol L-1 of a diprotic acid with pKA1 = 4.62 and pKA2 = 8.62 ? H2A + H2O ⇌ H3O+ + HA- pkA1 HA- + H2O ⇌ H3O+ + A2- pkA2
Calculate the volume, in liters, of 1.548 M KOH that must be added to a 0.117 L solution containing 10.78 g of glutamic acid hydrochloride (H3Glu Cl–, MW = 183.59 g/mol) to achieve a pH of 10.36. Glutamic acid (Glu) is an amino acid with pKa values of pKa1 = 2.23, pKa2 = 4.42, pKa3 = 9.95.
What is the pH of a solution made by mixing 0.611 moles of HBr and 0.287 moles of KOH, where the resulting volume of the solution is 50.0 L?
What is the pH of a solution made by mixing 0.438 moles of HBr and 0.304 moles of KOH, where the resulting volume of the solution is 50.0 L?
A 15 L buffer solution is 0.250 Min HF and 250 M in Ne Calculate the pH of the solution after the addition of 0.0500 moles of sold NOH. Assume no volume change upon the addition of base. The K, for HF 35 x 104 351 3.54 3.46 3.63 Which of the following is TRUE? An effective buffer has a [base)(acid] ratio in the range of 10 -100. A buffer can not be destroyed by adding too much strong base....
Find the pH of a formic acid solution that was is prepared by adding 0.280 g of formic acid to a volumetric flask and bringing the final volume to 1.44 L by adding water
A buffered solution is made by adding 40.0 g NH4 Cl to 1.00 L of a 0.65-M solution of NH3. Calculate the pH of the final solution. (Assume no volume change.) (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 MindTap Reader. You should not use the OWLv2 References' Tables to answer this question as the values will not match.) pH =
What is the molarity of a solution made by dissolving 1.50 g of KOH in enough water to make 1.5 L of solution?
A buffered solution is made by adding 80.08 NH, Cl to 1.00 L of a 0.65-M solution of NH, Calculate the pH of the final solution (Assume no volume change.) (This problem requires values in your textbook's specific appendices, which you can access through the OWLv2 Mind Top Reader. You should not use the OWLv2 References Tables to answer this question as the values will not match.) pl -