A 25.0 mL volume of a 0.200 M N2H4 solution (Kb = 1.70 x 10-6) is...
A 25.0 mL volume of a 0.200 M N2H4
solution (Kb = 1.70 ×
10−6) is titrated to the equivalence point
with 0.100 M HCl. What is the pH of this solution at the
equivalence point? The titration is:
N2H4 + HCl
N2H5+ + Cl−
Consider the following Bronsted-Lowery acid-base reaction: HC1O2 + N(CH3)3 = [HN(CH3)3]* +C102 Which two substances represent Bronsted-Lowery bases in this reaction? a HC1O2 and [HN(CH3)31* O b. N(CH3)3 and [HN(CH3)31+ c. N(CH3)3 and C102 d. (HN(CH3)3]* and C102 e HCIO2 and N(CH3)3
24. A 25.0 mL volume of a 0.200 M N,H& solution (K 1.70x10 titrated to the equivalence point with 0.100 M HCl. What is the pH of this solution at the equivalence point? The titration is a. 4.70 b. 8.23 c. 7.00 d. 9.30
24. A 25.0 mL volume of a 0.200 M N,H& solution (K 1.70x10 titrated to the equivalence point with 0.100 M HCl. What is the pH of this solution at the equivalence point? The titration is...
A 50.0 mL sample of 0.350 M N2H4 (Kb = 9.51 x 10-7) is titrated with 0.500 M HBr. Calculate: a. the pH after adding 10.00 mL of HBr b. the pH at one-half the equivalence point c. the pH after adding 20.00 mL of HBr d. the volume required to reach the equivalence point e. the pH at the equivalence point f. the pH after adding 45.00 mL of HBr
A volume of 100 mL of a 0.390 M HN O 3 solution is titrated with 0.800 M KOH . Calculate the volume of KOH required to reach the equivalence point. Express your answer to three significant figures and include the appropriate units.
You have 40.00 mL of a 0.300 M aqueous solution of the weak base C6H5NH2 (Kb = 4.00 x 10-10). This solution will be titrated with 0.300 M HCl. (a) How many mL of acid must be added to reach the equivalence point? (b) What is the pH of the solution before any acid is added? (c) What is the pH of the solution after 10.00 mL of acid has been added? (d) What is the pH of the solution...