Question

If 25.31 mL of 0.0500 M NaOH solution are required to reach the equivalence point of an acid-base titration of 40.0 mL of 7-Up, how many moles of NaOH were required?

Based on your answer to the previous question, how many moles of citric acid are in the 40.0 mL of 7-Up?

Answer #1

thanks and hope you like the answer

How many mL of the NaOH solution needs to be added to reach the
equivalence point of the hydrochloric acid-sodium hydroxide
titration?
Only given information is 50cm3 base was added at 0.1 M to 25cm3
of HCl at 0.1M. I have created a graph in excell but I'm unsure if
I need it to work this out? Help on the method would be great thank
you.

What volume of 0.5 M NaOH is needed to perform the titration of
30 mL of 0.1 M H3PO4? Question options: a) V = 12 mL b) V = 6 mL c)
V = 18 mL d) V = 30 mL he 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: Question options: a) pH = 2.9 b) pH = 1.7 c) pH =...

1a) How many mL of (7.03x10^-1) M HCOOH would it take
to reach the equivalence point in the titration of (4.200x10^1) mL
of (4.070x10^-1) M KOH?
1b)What is the pH at exactly 1/2 of the volume
required to reach the equivalence point in the titration of
(4.810x10^1) mL of (4.050x10^-1) M HCNwith (6.87x10^-1) M
KOH?
1c)What is the pH at 0.00 mL of titrant in the titration of 50.00
mL of 0.400 M B (a generic base with Kb =...

Consider the titration of 40.0 mL of 0.250 M HF with 0.200 M
NaOH. How many milliliters of base are required to reach the
equivalence point? Calculate the pH at the following points:
a)After the addition of 10.0 mL of base
b)Halfway to the equivalence point
c)At the equivalence point
d)After the addition of 80.0 mL of base

A 25.00 mL sample of a solution required 21.40 mL of 0.1185 M
NaOH to reach the visual endpoint. How many moles of H+
were present in the aliquot? Give your answer to
four decimal places.

When 0.100 M NaOH is titrated with 25.00 mL 0.0500 M HBr, which
of the following is correct for this titration?
A. Initially the pH will be less than 1.00.
B. The pH at the equivalence point will be 7.00.
C. It will require 12.50 mL of NaOH to reach the equivalence
point.
When 0.100 M NaOH is titrated with 25.00 mL 0.0500 M HBr, which
of the following is correct for this titration?
A. Initially the pH will be...

In an acid base titration experiment, 50.0 ml of a 0.0500 m
solution of acetic acid ( ka =7.5 x 10^-5) was titrated with a
0.0500 M solution of NaOH at 25 C. The system will acquire this pH
after addition of 18.75 mL of the titrant:
answer is 4.535

A 25 mL aliquot of an HCl solution is titrated with 0.100 M
NaOH. The equivalence point is reached after 21.27 mL of the base
were added. Calculate the concentration of the acid in the original
solution, the pH of the original HCl solution and the original NaOH
solution

A 20.00-mL sample of formic acid (HCO2H) is titrated with a
0.100 M solution of NaOH. To reach the endpoint of the titration,
30.00 mL of NaOH solution is required. Ka = 1.8 x
10-4
What is the pH of the solution after the addition of 10.00 mL of
NaOH solution?
What is the pH at the midpoint of the titration?
What is the pH at the equivalence point?

Determine the volume in mL of 0.12 M NaOH(aq) needed to reach
the equivalence (stoichiometric) point in the titration of 27 mL of
0.16 M HF(aq). The Ka of HF is 7.4 x 10-4

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