Question
In: Chemistry
A titration involves adding a reactant of known quantity to a solution of an another reactant...
A titration involves adding a reactant of known quantity to a solution of an 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 HA(aq)+OH−(aq)→A−(aq)+H2O(l) A certain weak acid, HA, with a Ka value of 5.61×10−6, is titrated with NaOH. A solution is made by titrating 9.00 mmol (millimoles) of HA and 1.00 mmol of the strong base. What is the resulting pH? More strong base is added until the equivalence point is reached. What is the pH of this solution at the equivalence point if the total volume is 59.0 mL ?
Solutions
Expert Solution
HA(aq) + OH−(aq) -----------------> A−(aq) + H2O(l)
9.00 1.00 0 0
8.00 0.00 1.00
pKa = -log (5.61 x 10^-6) = 5.25
pH = pKa + log [salt / acid]
= 5.25 + log [1.00 / 8.00]
pH = 4.35
b)
here salt is formed .
salt concentration = 9 / 59 = 0.1525 M
pH = 7 + 1/2 (pKa + log C)
= 7 + 1/2 (5.25 + log 0.1525)
pH = 9.22
queen_honey_blossom answered 2 years agoRelated Solutions
Ten Titration of Weak Acid with Strong Base A titration involves adding a reactant of known...
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...
To convert from a given quantity of one reactant or product to the quantity of another...
To convert from a given quantity of one reactant or product to
the quantity of another reactant or product: First, convert the
given quantity to moles. Use molar masses to convert masses to
moles, and use Avogadro's number (6.02×1023 particles per mole) to
convert number of particles to moles. Next, convert moles of the
given reactant or product to moles of the desired reactant or
product using the coefficients of the balanced chemical equation.
For example, in the chemical equation...
To convert from a given quantity of one reactant or product to the quantity of another...
To convert from a given quantity of one reactant or product to
the quantity of another reactant or product:
First, convert the given quantity to moles. Use molar masses to
convert masses to moles, and use Avogadro's number (6.02×1023
particles per mole) to convert number of particles to moles.
Next, convert moles of the given reactant or product to moles of
the desired reactant or product using the coefficients of the
balanced chemical equation. For example, in the chemical
equation...
The iodine clock reaction involves reacting an aqueous solution of potassium iodate with another solution containing...
The iodine clock reaction involves reacting an aqueous solution
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Outline of procedure: Dilute bleach solution A 1/10. Prepare analyte for titration by adding 10mL of...
Outline of procedure:
Dilute bleach solution A 1/10.
Prepare analyte for titration by adding 10mL of diluted bleach
solution, indicator and 5mL of 2 M HCl.
Titrate the analyte with 0.05524 M Na2S2O3.
Average volume of Na2S2O3 added = 31.25 mL
Question: Calculate the percent of sodium
hypochlorite in the original bleach bottle using your averaged
result. Show the calculation for solution A only. Which bleach
solution is the more potent cleaning agent?
A precipitation titration was performed by adding 0.20 M Ag+ (from standard silver nitrate solution) from...
A precipitation titration was performed by adding 0.20 M Ag+
(from standard silver nitrate solution) from a buret into 40.0 mL
mixture of 0.10 M I- (as NaI) and 0.10 M Cl- (as NaCl). Calculate
the concentration of Ag+, I-, Cl-, Na+, and NO3- when (a) 0.0 mL,
(b) 10.0 mL, (c) 20.0 mL, (d) 30.0 mL, (d) 40.0 mL, and (d) 50.0 mL
of Ag+ were added. (Given Ksp AgI = 8.3 x 10-17 and Ksp AgCl = 1.8...
An indirect titration is a titration which requires the presence of another species to determine the...
An indirect titration is a titration which requires the presence
of another species to determine the endpoint. When triiodide (I3-)
is used to determine the concentration of formaldehyde in solution,
a back titration is used.
For what reason is a direct titration not used?
What is the third species that is added to the titration?
_________________________
Describe how the other two species present during the titration
work in conjunction to allow the analyst to determine the
formaldehyde concentration
Distinguish between...
Converting between quantities To convert from a given quantity of one reactant or product to the...
Converting between quantities
To convert from a given quantity of one reactant or product to
the quantity of another reactant or product:
First, convert the given quantity to moles. Use molar masses to
convert masses to moles, and use Avogadro's number
(6.02×1023particles per mole) to convert number of particles to
moles.
Next, convert moles of the given reactant or product to moles of
the desired reactant or product using the coefficients of the
balanced chemical equation. For example, in the...
1- In the titration between potassium iodate and the sodium thiosulfate solution, if the titration is...
1- In the titration between potassium iodate and the sodium
thiosulfate solution, if the titration is not performed immediately
after the addition of the sulfuric acid, how would this likely
affect the calculated concentration of your diluted sodium
thiosulfate solution?
2- Why did the titrations performed need to be started
immediately after adding the sulfuric acid?
3- A sample of bleach was analyzed as in this procedure. The
only procedural difference is that the student weighed out the
bleach solution...
A titration is performed by adding .435M KOH to 80ml of .205M HC3H5O2. A) Calculate the...
A titration is performed by adding .435M KOH to 80ml of .205M
HC3H5O2.
A) Calculate the pH before the addition of any KOH?
B) Calculate the pH after the addition of 7.54ml of KOH?
C) Calculate the volume of base needed to reach the equivalence
point?
D) Enter the pH of the solution at the equivalence point of the
titration?
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