2-aminoethanol is a weak base with a pkb=4.50. What is the pH of a 0.150 M 2-aminoethanol solution?
2-aminoethanol is a weak base with a pkb=4.50. What is the pH of a 0.150 M 2-aminoethanol solution?
What is the pKb of a weak base KA if the pH of a 0.079-M solution of KA is 9.40?
1. If a buffer solution is 0.150 M in a weak base (K,.710 what is the pH? and 0.430 M in its conjugate acid Number 2. If a buffer solution is 0.250 M in a weak acid (K what is the pH? 5.1 x10) and 0.550 M in its conjugate base, Number pH-
3) a) What is the pKb for a weak base if the pH of a 0.125M solution of this weak base was found to be 8.16? 4) When a weak acid is added to water to make a 0.250M solution, the acid was found to be 1.5% ionized. What is the Ka and pKa of this weak acid? 5) At 60°C, Kw = 9.6x10-14 (Kw increases as the temperature increases). a) For pure water at 60°C, what is the [H+] and pH....
Morphine is a weak base. A 0.150 M solution of morphine has a pH of 10.5. Calculate Kb for morphine 2. 2
Part A) Amphetamine (C9H13N) is a weak base with a pKb of 4.2. Calculate the pH of a solution containing an amphetamine concentration of 205 mg/L. Express your answer to two decimal places. Part B) Find the pH of a 0.150 M solution of a weak monoprotic acid having Ka= 0.20. Express your answer to two decimal places. B2) Find the percent dissociation of this solution. Express your answer using two significant figures.
A 0.150 M solution of a weak base has a pH of 11.22. Determine Kb for the base. Express your answer using two significant figures.
A 0.150 M solution of a weak base has a pH of 11.20. Part A Determine Kb for the base. Express your answer using two significant figures.
1.The pH of a 2.65×10-3 M solution of a weak base is 9.17. Calculate pKb for this base to two decimal places. 2.Determine the mass (in g) of sodium butanoate (NaC3H7COO) that must be added to 78.9 mL of 0.609 M butanoic acid to yield a pH of 6.43. Report your answer to 3 significant figures. Assume the volume of the solution does not change and that the 5% approximation is valid.
The pOH of a 0.20 M solution of a weak base is 2.72. What is the Kb and pKb for this base?
Consider a weak base that has a pKb of 4.2. • What is the pKa of this solution? • What is the pH of a 0.2 M solution of this base? • If you were to mix 50 mL of the 0.2 M base with 50 mL of a 0.1 M solution of its conjugate acid, what would the pH of this buffer be, and what is its effective buffering range?