Question

In: Chemistry

1.What is the pH at the equivalence point when 0.100 M weak acid HA (Ka =...

1.What is the pH at the equivalence point when 0.100 M weak acid HA (Ka = 1.48 x 10 - 4) is titrated with 0.050 M KOH?

2.Calculate the pH of a solution made by mixing 50.00 mL of 0.100 M KCN with 4.33 mL of 0.425 M strong acid HCl. HCN pKa = 9.21

3.Strong bases, NaOH and KOH can not be used as primary standards because of the presence of ______________ A.carbonate B.water C.adsorbed water

please explain each step by step, thank you

Solutions

Expert Solution

queen_honey_blossom answered 8 months ago
Next > < Previous

Related Solutions

The pH at the equivalence point when a 0.20 M weak base (Ka = 9.1 x...
The pH at the equivalence point when a 0.20 M weak base (Ka = 9.1 x 10-7) is titrated with a 0.20 M strong acid is: a) pH = 3.5 b) pH = 1.7 c) pH = 2.9
Calculate the pH at the equivalence point for the titration of 1.288 M HA (a weak...
Calculate the pH at the equivalence point for the titration of 1.288 M HA (a weak acid with pKa = 2.16) with 1.288 M NaOH.
Calculate the pH at the equivalence point for the titration of 1.328 M HA (a weak...
Calculate the pH at the equivalence point for the titration of 1.328 M HA (a weak acid with pKa = 6.95) with 1.328 M NaOH.
A 0.30 solution of a weak acid(HA) has a pH of 3.77. What is the Ka?
A 0.30 solution of a weak acid(HA) has a pH of 3.77. What is the Ka?
What is the pH at the equivalence point for the titration of 25.00 mL 0.100 M...
What is the pH at the equivalence point for the titration of 25.00 mL 0.100 M CH3CH2CH2CO2- with 0.1848 M HCl? Species (K values) CH3CH2CH2CO2H (Ka = 1.14E-5) CH3CH2CH2CO2- (Kb = 2.63x10-10
part 1 - A 0.100 M solution of an acid, HA, has a pH=2.00. What is...
part 1 - A 0.100 M solution of an acid, HA, has a pH=2.00. What is the value of Ka of this acid? part 2 - We treat Kw as a fixed value, even though it, like all equilibrium constants, varies with temperature. The pH of pure water at 50 oC is 6.630. What is Kw at this temperature?
The pH at the half-equivalence point is 3.15 in an acid-base titration. What is the Ka...
The pH at the half-equivalence point is 3.15 in an acid-base titration. What is the Ka of the acid? What are the components of an acid-base buffer? What do these buffers do?
What is the pH at the equivalence point when 50.00 mL of 0.112 M hydroxyacetic acid...
What is the pH at the equivalence point when 50.00 mL of 0.112 M hydroxyacetic acid is titrated with 0.0580 M KOH? (Assume Ka = 1.47 ✕ 10−4, and Kw = 1.01 ✕ 10−14.)
What is the approximate pH at the equivalence point of a weak acid-strong base titration if...
What is the approximate pH at the equivalence point of a weak acid-strong base titration if 25 mL 21) of aqueous formic acid requires 29.80 mL of 0.0567 M NaOH? Ka =1.8 × 10-4 for formic acid. A) 2.46 B) 8.12 C) 11.54 D) 5.88
Calculate the pH at the equivalence point for the titration of 0.100 M methylamine (CH3NH2) with...
Calculate the pH at the equivalence point for the titration of 0.100 M methylamine (CH3NH2) with 0.100 M HCl. The Kb of methylamine is 5.0
ADVERTISEMENT
Subjects
ADVERTISEMENT
Latest Questions
ADVERTISEMENT