Briefly explain how the graphs for two titration curves for a
weak acid-strong base and strong...
Briefly explain how the graphs for two titration curves for a
weak acid-strong base and strong acid-strong base are similar
before and at the equivalence point.
Weak base/ Strong acid titration curve question.
1) In the titration of .0400 M weak base B of 50 ml with .100 M
HCl. What is the solution pH before any HCl is added?
2) In the titration of .0400 M weak base B of 50 ml with .100 M
HCl. What is the solution pH after 10 ml HCl is added?
3) In the titration of .0400 M weak base B of 50 ml with .100 M
HCl. What...
1) A pH meter is standardized at what three pHs?
2) The initial pH of the acetic acid-NaOH titration curve was _________.
3) Explain which of the following indicators would be appropriate for a weak acid-strong base titration?
Indicator
pH of color change
Bromcresol green
3.8 - 5.4
Bromothymol blue
6.0 - 7.6
Phenolphthalein
8.0 - 9.6
Consider the titration of a weak base (B- ) with a strong acid
(HCl). Draw (this can be hand drawn) a pH (not pOH) vs mL HCl graph
(it will not look the same as the one in question #13; if you start
with a weak base, will the pH be low or high? As H+ is added, will
the pH increase or decrease?). Label the titration curve with
letters A-E, and describe the relative quantities of the
dissociated base...
Ten
Titration of Weak Acid with Strong Base
A titration involves adding a reactant of known quantity to a
solution of another reactant while monitoring the equilibrium
concentrations. This allows one to determine the concentration of
the second reactant. The equation for the reaction of a generic
weak acid HA with a strong base is
HA9(aq)+OH-(aq)
----->
A-(aq)+H2O(l)
A certain weak acid, HA, with a Ka value of
5.61x10-6, is titrated with NaOH
Part A
A solution is made by...
Weak Acid - Strong Base Titration
Calculate the pH at the given amounts below in the titration.
You are titrating 35.0 mL of .15 M HNO2 with .1 M NaOH
until you reach 100 mL of NaOH added.
For this problem the Ka value is 4.6 x 10-4
a) 0.00 mL NaOH added
b) 30.0 mL NaOH added
c) 60.0 mL NaOH added
d) 100.0 mL NaOH added
What is the pH of a weak acid strong base titration after each
of the following additions? Ka for HF is 3.5 x 10-4.
a. 10.0 mL of 0.250 M NaOH added to 15.0 mL of 0.400 M HF
b. 25.0 mL of 0.250 M NaOH added to 35.0 mL of 0.1785 M HF
c. 20.0 mL of 0.250 M NaOH added to 20.0 mL of 0.350 M HF
Please show your work so I can better understand this. thanks!...
Consider a titration curve for a weak base and a strong acid.
Suppose both phenolphthalein and bromocresol green are present in
the solution. What color changes would occur at pH 10, pH 7, and pH
3?
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