Homework Answers
explanation :
the indicators which have pH range 6.4 to 8.4 can be best for these titration.
in the image given the selected indicators only the pH range 6.4 to 8.4 . so those three only suitable
phenol red red indicator is best indicator at that range of end-point.
phenol red pH range is 6.8 to 8.4
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The titration shown here has an equivalence point at pH = 7.4. Using this table, identify...
The titration shown here has an equivalence point at pH = 4.3. Using this table, identify...
The titration shown here has an equivalence point at pH = 4.3. Using this table, identify which of the following indicators would be appropriate for this titration. Check all that apply. ethyl orange methyl orange bromocresol purple bromothymol blue bromophenol blue phenolphthalein
Which one of the following indicators would be appropriate to determine the equivalence point in the...
Which one of the following indicators would be appropriate to determine the equivalence point in the titration of 0.25 M HClO with 0.25 M NaOH? thymol blue bromocresol purple bromocresol green thymolphthalein
The titration shown in the plot has an equivalence point at pH = 3.2. Titration Data...
The titration shown in the plot has an equivalence point at pH = 3.2. Identify which of the indicators would be appropriate for this titration.
Section B ANALYTICAL CHEMISTRY 3. Answer ALL parts. (a) Answer each of the following i) ii)...
Section B ANALYTICAL CHEMISTRY 3. Answer ALL parts. (a) Answer each of the following i) ii) Define buffer capacity. (b) A solution was prepared by dissolving 1.572 grams of NaB (Relative Molecular Mass 169), the sodium salt of a weak base, in 100 0 cm of water. pK, for the weak acid HB is 6.3. Calculate the pi of the solution, K.-1 x 1014 (c) 20.0 cm' of the basic solution is titrated with 0.134 mol dm HCL. Calculate: i)...
The following graph shows the pH curve for the titration of 25 mL of a 0.1...
The following graph shows the pH curve for the titration of 25
mL of a 0.1 M monoprotic acid solution with a 0.1 M solution of a
monoprotic base.
mL of 0.1 M base added
(1) The pH curve represents the titration of a
_______(weak/strong) acid with a _______(weak/strong)base.
(2) Choose a suitable indicator for the endpoint
of the titration from the following pulldown list
__________.(bromocresol green / methyl red / bromothymol blue /
cresol red / thymol blue /...
Consider the titration of 25.00 mL of 0.115M NH3 (ka= 5.70e-10 ; kb= 1.75e-5) with 0.0920...
Consider the titration of 25.00 mL of 0.115M NH3 (ka= 5.70e-10 ;
kb= 1.75e-5) with 0.0920 M HCl.
a) calculate the pH of the solution for the following volume of
HCl: 6.25 mL
b) calculate the pH of the solution for the following volume of
HCl: 31.25 mL
c) calculate the pH of the solution for the following volume of
HCl: 50.0 mL
d) Which indicator from the table minimizes the titration error
and why?
blue Indicator thymol blue bromophenol...
An unknown solution gives the following sequential results for color when indicators are 3. added (shown...
An unknown solution gives the following sequential results for color when indicators are 3. added (shown below). Using the corresponding color ranges from the table on page 2, estimate the approximate pH range of this unknown solution. Explain. नी (cnge 3.0-46 Bluish purple Bromphenol blue: 4.2-6.8 Yellow Methyl Red: 60-76 Blue Bromothymol Blue: 2.3-10-0 Colorless Phenolpthalein: 2. Sketch a titration curve for the titration of 50 mL of 0.10 M NaOH as 0.1 M HCl is added to it. Label...
Based on the following information... please answer A. B. and C. TITRATION OF A WEAK ACID...
Based on the following information...
please answer A. B. and C.
TITRATION OF A WEAK ACID TRIAL #1 equivalence point halfway point 25 VOLUME OF BASE ADDED 30 35 40 TITRATION OF A WEAK ACID TRIAL #2 1 equivalence point Hd half-way point s 10 15 30 35 40 45 20 25 VOLUME OF BASE ADDED Trial 1 Trial 2 Mass of oxalic acid 0.2039 pH at equivalence point a Mass of oxalic acid 0.2099 at equivalence point nt 8,5...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is to indicate the of the titration. Use Table 10.2 for the following question. If an acidic solution is titrated with a basic solution and methyl violet is used as an indicator, the solution color will change from to QUESTION 2 3 points Save Answer The molarity of a solution prepared by dissolving 17.0 g of hydrochloric acid (HCI (aq) in 133 mL of water...
1.A solution has a pH of 5.5. What would be the color of the solution if...
1.A solution has a pH of 5.5. What would be the color of the solution if each of the following indicators were added? (i) bromophenol blue(ii) bromothymol blue(iii) methyl red (iv) phenolphthalein 2.Calculate the pH at the equivalence point when 50.0 mL of a 0.100 M HN3 acid (a weak monoprotic acid having a Ka = 1.90x10-5) is titrated with 0.100 M NaOH. The titration reaction can be represented as HA + NaOH --- > NaA + H2O Hint: At...
The titration shown here has an equivalence point at pH = 4.3. Using this table, identify which of the following indicators would be appropriate for this titration. Check all that apply. ethyl orange methyl orange bromocresol purple bromothymol blue bromophenol blue phenolphthalein
The titration shown in the plot has an equivalence point at pH = 3.2. Identify which of the indicators would be appropriate for this titration.
Section B ANALYTICAL CHEMISTRY 3. Answer ALL parts. (a) Answer each of the following i) ii) Define buffer capacity. (b) A solution was prepared by dissolving 1.572 grams of NaB (Relative Molecular Mass 169), the sodium salt of a weak base, in 100 0 cm of water. pK, for the weak acid HB is 6.3. Calculate the pi of the solution, K.-1 x 1014 (c) 20.0 cm' of the basic solution is titrated with 0.134 mol dm HCL. Calculate: i)...
The following graph shows the pH curve for the titration of 25
mL of a 0.1 M monoprotic acid solution with a 0.1 M solution of a
monoprotic base.
mL of 0.1 M base added
(1) The pH curve represents the titration of a
_______(weak/strong) acid with a _______(weak/strong)base.
(2) Choose a suitable indicator for the endpoint
of the titration from the following pulldown list
__________.(bromocresol green / methyl red / bromothymol blue /
cresol red / thymol blue /...
Consider the titration of 25.00 mL of 0.115M NH3 (ka= 5.70e-10 ;
kb= 1.75e-5) with 0.0920 M HCl.
a) calculate the pH of the solution for the following volume of
HCl: 6.25 mL
b) calculate the pH of the solution for the following volume of
HCl: 31.25 mL
c) calculate the pH of the solution for the following volume of
HCl: 50.0 mL
d) Which indicator from the table minimizes the titration error
and why?
blue Indicator thymol blue bromophenol...
An unknown solution gives the following sequential results for color when indicators are 3. added (shown below). Using the corresponding color ranges from the table on page 2, estimate the approximate pH range of this unknown solution. Explain. नी (cnge 3.0-46 Bluish purple Bromphenol blue: 4.2-6.8 Yellow Methyl Red: 60-76 Blue Bromothymol Blue: 2.3-10-0 Colorless Phenolpthalein: 2. Sketch a titration curve for the titration of 50 mL of 0.10 M NaOH as 0.1 M HCl is added to it. Label...
Based on the following information...
please answer A. B. and C.
TITRATION OF A WEAK ACID TRIAL #1 equivalence point halfway point 25 VOLUME OF BASE ADDED 30 35 40 TITRATION OF A WEAK ACID TRIAL #2 1 equivalence point Hd half-way point s 10 15 30 35 40 45 20 25 VOLUME OF BASE ADDED Trial 1 Trial 2 Mass of oxalic acid 0.2039 pH at equivalence point a Mass of oxalic acid 0.2099 at equivalence point nt 8,5...
QUESTION 1 6 points Save Answer The purpose of an indicator in an acid-base titration is to indicate the of the titration. Use Table 10.2 for the following question. If an acidic solution is titrated with a basic solution and methyl violet is used as an indicator, the solution color will change from to QUESTION 2 3 points Save Answer The molarity of a solution prepared by dissolving 17.0 g of hydrochloric acid (HCI (aq) in 133 mL of water...
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