Question

100. mL of 0.200 *M*HCl is titrated with 0.250
*M*NaOH. What is the pH of the solution at the equivalence
point?

Can you include the steps please?

Answer #1

Titration of strong acid (HCl) with strong base (NaOH) -

Initial concentration of H^{+} ions = [Concentration]
[Volume]= 0.200 M * 0.100 L = 0.02 mol

At equivalnece point,, moles of H^{+} = moles of
OH^{-} = 0.02 mol

The volume of NaOH added will produce the concentration OH- equal to 0.02 mol (H+ concentration).

Volume of NaoH added = 0.02 mol / 0.25 M = 0.08 L

At equivalence point all the H^{+} ions with react with
OH^{-} ions added.

So, remaining H^{+} concentration in the solution = 0.02
mol -0.02 mol = 0

So, P^{H} = 7.0 (i.e neutral solution) at .equivalence
point.

A - B
100. mL of 0.200 M HCl is titrated with 0.250
M NaOH.
Part A
What is the pH of the solution after 50.0 mL of base has been
added?
Express the pH numerically.
pH =
SubmitHintsMy AnswersGive UpReview Part
Part B
What is the pH of the solution at the equivalence point?
Express the pH numerically.
pH =
SubmitHintsMy AnswersGive UpReview Part

Suppose 25.00 mL of 0.250 M benzoic acid are titrated with 0.200
M NaOH. What is the pH at the equivalence point?

1. A 100 mL solution of 0.200 M HF is titrated with 0.100 M
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200 mL
50 mL
100 mL
300 mL
Cannot determine based on the provided information.
2. A 100 mL solution of 0.200 M NH3 is titrated with
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point?
200 mL
100 mL
50 mL
300 mL
Cannot determine based on the...

A 100 mL solution of 0.200 M Sr(OH)2 is titrated with
0.100 M H3PO4. What is the volume of
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100 mL
200 mL
50 mL
300 mL
133 mL
A 100 mL solution of unknown concentration
H2SO4 is titrated with 200 mL of 0.100 M
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0.100 M
0.050 M
0.020 M
0.200 M
Cannot determine based on the provided information.

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A) 15.0 mL
B) 19.8 mL
C) 20.1 mL
D) 35.0 mL

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a. before the addition of any HCl. ______________ b. halfway to the
equivalence point.______________ c. at the equivalence
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Two 23.0 mL samples, one 0.200 MKOH and the other 0.200 M
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questions regarding these two titrations.
a). What is the volume of added acid at the equivalence point
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b). Predict whether the pH at the equivalence point for each
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c). Predict which titration curve will have the lowest initial
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Consider the titration of 40.0 mL of 0.250 M HF with 0.200 M
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b)Halfway to the equivalence point
c)At the equivalence point
d)After the addition of 80.0 mL of base

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For all of the following questions 20.00 mL of 0.192 M HBr is
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Region 1: Initial pH: Before any titrant is added to our starting
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What is the concentration of H+ at this point in the
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M
What is the pH based on this H+ ion concentration?
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Complete the BCA table below at...

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