Question
In: Chemistry
A 10.00 mL solution of 0.0500 M AgNO3 was titrated with 0.0250 M NaBr in the...
A 10.00 mL solution of 0.0500 M AgNO3 was titrated with 0.0250 M NaBr in the cell: S.C.E.(saturated calomel electrode) titration solution Ag (s). (Ksp AgBr(s) = 5.0e-13)
Find the cell voltage (v) when the volume of titrant added is 5.00 ml.
Find the equivalence volume (ml) of titrant added.
Calculate the cell voltage (v) when the volume of titrant added is 24.58 ml
Calculate the cell voltage (v) at the equivalence point.
.
Solutions
Expert Solution
Solution.
The scheme of the cell is S.C.E.|| titration solution | Ag(s)
Therefore, the cell voltage is 
When 5 mL of the titrant is added, the concentration of silver ions is
The cell voltage is 
The equivalence volume of titrant added can be found as
The cell voltage at the equivalence point will be determined by a solubility of AgBr.
The cell voltage is 
When 24.58 mL of titrant has been added, the concentration of bromide-ions is
The concentration of silver ions is
The cell voltage is 
queen_honey_blossom answered 2 years agoRelated Solutions
A 10.0 mL solution of 0.030 M AgNO3 was titrated with 0.015 M NaBr in the...
A 10.0 mL solution of 0.030 M AgNO3 was titrated with 0.015 M
NaBr in the cell. S.C.E. || titration solution | Ag(s) Find the
cell voltage for 0.4, 10.0, 20.0, and 27.0 mL of titrant. (The Ksp
of AgBr = 5.0 ✕ 10−13.) 0.4 V 10.0 V 20.0 V 27.0 V
A solution containing 10.00 mL of 0.0500 M metal ion buffered to pH = 10.00 was...
A solution containing 10.00 mL of 0.0500 M metal ion buffered to
pH = 10.00 was titrated with 0.0400 M EDTA. Calculate the fraction
(αY4-) of free EDTA in the form Y4−. Keep 2 significant
figures.
A 25.00 mL of 0.0500 M imidazole (B) solution was titrated with 0.1250 M HNO3. The...
A 25.00 mL of 0.0500 M imidazole (B) solution was titrated with
0.1250 M HNO3. The pKa of the imidazolium chloride (BH+) is
6.993.
(a) what is the pH of the solution before adding any HNO3?
(b) What is the pH of the solution after adding 5.00 mL of
HNO3?
(c) What is the pH of the solution after adding 10.00 mL of
HNO3?
(d) What is the pH of the solution after adding 12.00 mL of
HNO3?
A solution containing 45.00 ml of 0.0500 M metal ion buffered to pH = 10.00 was...
A solution containing 45.00 ml of 0.0500 M metal ion buffered to
pH = 10.00 was titrated with 0.0400 M EDTA. Answer the following
questions and enter your results with numerical value only.
Calculate the equivalence volume, Ve, in
milliliters.
Calculate the concentration (M) of free metal ion at V = 1/2
Ve.
Calculate the fraction (αY4-) of free EDTA
in the form Y4-. Keep 2 significant figures.
If the formation constant (Kf) is 1012.00.
Calculate the value of the...
A 83.0 mL sample of 0.0500 M HNO3 is titrated with 0.100 M KOH solution. Calculate...
A 83.0 mL sample of 0.0500 M HNO3 is titrated
with 0.100 M KOH solution. Calculate the pH after the following
volumes of base have been added.
(a) 11.2 mL
pH = _________
(b) 39.8 mL
pH = __________
(c) 41.5 mL
pH = ___________
(d) 41.9 mL
pH = ____________
(e) 79.3 mL
pH = _____________
35 mL of a 0.0250 M pyridine is titrated with 0.00 mL, 10.00mL 15.00mL 20.00 mL...
35 mL of a 0.0250 M pyridine is titrated with 0.00 mL, 10.00mL
15.00mL 20.00 mL and 25.00mL of a 0.0438 M HCl solution. Calulate
the pH of the solution after each addition and sketch the resulting
graph
Titration of a 15.0 mL solution of KOH requires 17.0 mL of 0.0250 M H2SO4 solution....
Titration of a 15.0 mL solution of KOH requires 17.0 mL of
0.0250 M H2SO4 solution.
What is the molarity of the KOH solution?
M=?
1. a. 0.0500 M of AgNO3 is used to titrate a 25.00-mL containing 0.1000 M sodium...
1. a. 0.0500 M of AgNO3 is used to titrate a 25.00-mL containing
0.1000 M sodium chloride (NaCl) and 0.05000 M potassium iodide
(KI), what is the pAg of the solution after 15.00 mL of AgNO3 is
added to the solution? Ksp, AgCl (s) = 1.82 x 10-10; Ksp, AgI(s) =
8.3*10-17.
b. Same titration as in (a), what is the pAg of the solution
after 25.00 mL of AgNO3 is added to the above solution?
c. Same titration as...
Assume that 40.0 mL of a 0.0250 M solution of the protonated form of the amino...
Assume that 40.0 mL of a 0.0250 M solution of the protonated
form of the amino acid valine (H2A+) (Figure 1) is titrated with
0.100 M NaOH.
Part A
Calculate the pH after addition of 10.0 mL of 0.100 M NaOH.
Express your answer using three significant figures.
Part B
Calculate the pH after addition of 15.0 mL of 0.100 M NaOH.
Express your answer using three significant figures.
Part C
Calculate the pH after addition of 20.0 mL of...
In the experiement, each flask containing a water sample, pipette 10.00 mL of the AgNO3 solution....
In the experiement, each flask containing a water sample,
pipette 10.00 mL of the AgNO3 solution. Using a small graduated
cylinder, carefully add 3.0 mL of Fe(NO3)3 solution and 2.0 mL of
6M HNO3 to each water sample. the trial is now ready for titration.
Obtain approximately 120 mL of stock KSCN solution. Rinse out a
clean buret with about 10 mL of KSCN at least twice, and discard
the washing solution into a waste beaker. From the
calculation , number...
ADVERTISEMENT
ADVERTISEMENT
Latest Questions
- An investor is considering purchasing a Treasury bond with a 20 year maturity, an 8% coupon...
- Write a program that copies the contents of one file to a destination file. This program...
- how to conduct a marketing mix for 3d crest white strips
- Is big data analytics used for service innovation at Amazon? If so, please write a brief...
- A shrink-fit process has been used to enhance the pressure carrying capacity of a cylinder. During...
- Ten-year zero coupon bonds issued by the U.S. Treasury have a face value of $1,000 and...
- The Blossom Department of Transportation has issued 25-year bonds that make semiannual coupon payments at a...
ADVERTISEMENT