2. The weak base B (Kb = 1.0 * 10-5) equilibrates between water (phase 1) and...
2. The weak base B (Kb = 1.0 * 10-5) equilibrates between water (phase 1) and benzene (phase 2). (a) Define the distribution coefficient, D, for this system. (b) Explain the difference between D and K, the partition coefficient. (c) Calculate D at pH 8.00 if K = 50.0,(d) Will D be greater or less at pH 10 than at pH 8? Explain why.
Solute A has a partition coefficient K = 2 for an extraction between water (phase 1) and benzene (phase 2). If 100 mL of a 0.01M solution of A in water is extracted one time with 300 mL benzene, what fraction will be extracted?
signment Score: 465/500 Resources G Give Up? Hint Check Answe Question 1 of 5 > Attempt 6 Consider the equilibration of a weak base B (Ks = 6.53 x 10-5) between water (phase 1) and benzene (phase 2). Which expression represents D, the distribution coefficient? B represents the unprotonated form of the base and BH represents the protonated form of the base. Which expression represents K, the partition coefficient? B represents the unprotonated form of the base and BH+ represents...
1)If the Kb of a weak base is 1.3 × 10-6, what is the pH of a 0.13 M solution of this base? 2) A certain weak base has a Kb of 7.40 × 10-7. What concentration of this base will produce a pH of 10.33?
1. If the Kb of a weak base is 7.4×10−6, what is the pH of a 0.39 M solution of this base? 2. A certain weak base has a Kb of 7.10×10−7 What concentration of this base will produce a pH of 10.30?
1.) If the Kb of a weak base is 3.4 x 10^-6, what is the pH of a 0.11M solution of this base? 2.) A certain weak base has a Kb of 7.00 x 10^-7. What concentration of this base will produce a pH of 10.16?
Solute X has a partition coefficient of 4.5 between water (phase 1) and chloroform (phase 2). The solute is initially dissolved in 50.0 mL. It is then extracted with 10.0 mL portions of chloroform. How many extractions must be performed for < 0.1% of X to remain in the water phase, i.e., > 99.9% of X has been transferred to the aqueous phase.
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....
Ammonia, NH3, is a weak base with a Kb value of 1.8×10−5. Part A What is the pH of a 8.50×10−2 M ammonia solution? Part B What is the percent ionization of ammonia at this concentration?
A certain weak base B has a base-ionization constant Kb of 6.6 × 10–4 at 25°C. If strong acid is added to a solution of B, at what pH will [B] = [BH+]? Hint: This is a buffers problem. Select one: a. 8.5 b. 7.0 c. 10.8 d. 3.2