Why does the titration curve of a strong acid and strong base appear to have a...
Why does the titration curve of a strong acid and strong base appear to have a buffer region, if strong acids and bases cannot act as buffers?
Homework Answers
Strong acids and bases ionise completely. That's why the concentration of H+ ions (if you are titrating an acid against a base) is high. When you add base drop by drop H+ ion concentration decreases but the decrease is not that significant compared to the H+ ion concentration originally. So, the change in pH is very little.
Same is the case when you titrate a strong base against a strong acid.
That's why it appears to have a buffer region.
Comment if any problem
Add Answer to:
Why does the titration curve of a strong acid and strong base
appear to have a...
Question: In the figure below, titration curves for strong acid with strong base and weak acid...
Question: In the figure below, titration curves for strong acid
with strong base and weak acid with strong base are shown. Compare
the shapes of these curves early in the titration for three
different cases: titration of a strong acid, titration of a weak
acid with a lower pKa, and titration of a weak acid with a higher
pKa. Discuss with the class why the titration curve for weak acids
increase more rapidly early in the titration than do stronger...
In figure 14.5, each curve the concentration or acid and base are the same, e.g., the...
In figure 14.5, each curve the concentration or acid and base are
the same, e.g., the curve labeled 1M is for the titration of 5
drops of 1M weak acid with 1M NaOH.
Why are the titration curves for the different reagent
concentrations so similar in the buffer region? Are these solutions
all buffers? please explain me with details thanks!
Computer-Simulated Titration Curves for 5 Drops of Weak Acids with Strong Base 14.00 1M 1x 10 M 12.00 1x 102...
Consider Figure 14.5. For each curve the concentration of acid and base are the same, e.g.,...
Consider Figure 14.5. For each curve the concentration of acid and base are the same, e.g., the curve labeled 1 M is for the titration of 5 drops of 1 M weak acid with 1 M NaOH. Why are the titration curves for the different reagent concentrations so similar in the buffer region? Are these solutions all buffers? Explain. 1 2 Computer-Simulated Titration Curves for 5 Drops of Weak Acids with S 14.00 12.00 0.00 0.00 2.00 8.00 10.00 4.00...
Classify each titration curve as representing a strong acid titrated with a strong base, a...
Classify each titration curve as representing a strong acid titrated with a strong base, a strong base titrated with a strong acid, a weak acid titrated with a Strong base, a weak base titrated with a strong acid, or a polyprotic acid titrated with a strong base.
Consider the following titration curve for the titration of a generic weak base B with a strong a...
Consider the following titration curve for the titration of a generic weak base B with a strong acid. The titration reaction is 5 10 5 2025 mL acid On the curve, indicate the points or regions that correspond to each of the following conditions. (a) pH depends only on the amount of excess strong aoid added ) the region with maximum bueing (e) pHi depends only on [8 (d) the sholhmrk (equivalence) point e)ph depends only om 1H
Consider the...
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Part 3: Working with the Titration Curve for a Polyprotic Acid and Strong Base Consider carbonic...
Part 3: Working with the Titration Curve for a Polyprotic Acid and Strong Base Consider carbonic acid, H.CO, (which is polyprotic) - a) Write the multi-step dissociation equilibrium for this acid in water (ie, there should be three chemical dissociation stages connected by two equilibrium arrows, given below): b) Below is an idealized titration curve showing the exhibited pH for 25.00 mL of a 0.100 M aqueous carbonic acid solution as a function of added 0.100 M NaOH in units...
why is the pH at end point for a titration of a weak acid with a strong base is greater than 7, yet that of the titration of a strong acid with a strong base is equal to 7?
why is the pH at end point for a titration of a weak acid with a strong base is greater than 7, yet that of the titration of a strong acid with a strong base is equal to 7?
Use the titration curve of a weak acid with a strong base below to answer the...
Use the titration curve of a weak acid with a strong base below to answer the following questions. Identify the Equivalence Point of Titration and label it on the titration curve below. (ii) What is the Titrant (iii) From the graph, what is the [H^+] and the volume of NaOH used to reach the equivalence point. (iv) Calculate the [OH^-] at the equivalence point (v) What is the pKa of the acid used for titration? (vi) Calculate the Ka of...
An unknown acid is titrated with a strong base (NaOH) to produce the above titration curve....
An unknown acid is titrated with a strong base (NaOH) to produce
the above titration curve. Key points on this graph reveal
important information about the substance and the solution created
with it.
What volume of NaOH is needed to reach the equivalence point
(the point where you added equal moles of NaOH to the
acid)? Select one of the following : ["10 mL", "5
mL", "20 mL", "30 mL", "40 mL", "25 mL", "15 mL", "35 mL"]
...
Question: In the figure below, titration curves for strong acid
with strong base and weak acid with strong base are shown. Compare
the shapes of these curves early in the titration for three
different cases: titration of a strong acid, titration of a weak
acid with a lower pKa, and titration of a weak acid with a higher
pKa. Discuss with the class why the titration curve for weak acids
increase more rapidly early in the titration than do stronger...
In figure 14.5, each curve the concentration or acid and base are
the same, e.g., the curve labeled 1M is for the titration of 5
drops of 1M weak acid with 1M NaOH.
Why are the titration curves for the different reagent
concentrations so similar in the buffer region? Are these solutions
all buffers? please explain me with details thanks!
Computer-Simulated Titration Curves for 5 Drops of Weak Acids with Strong Base 14.00 1M 1x 10 M 12.00 1x 102...
Consider Figure 14.5. For each curve the concentration of acid and base are the same, e.g., the curve labeled 1 M is for the titration of 5 drops of 1 M weak acid with 1 M NaOH. Why are the titration curves for the different reagent concentrations so similar in the buffer region? Are these solutions all buffers? Explain. 1 2 Computer-Simulated Titration Curves for 5 Drops of Weak Acids with S 14.00 12.00 0.00 0.00 2.00 8.00 10.00 4.00...
Classify each titration curve as representing a strong acid titrated with a strong base, a strong base titrated with a strong acid, a weak acid titrated with a Strong base, a weak base titrated with a strong acid, or a polyprotic acid titrated with a strong base.
Consider the following titration curve for the titration of a generic weak base B with a strong acid. The titration reaction is 5 10 5 2025 mL acid On the curve, indicate the points or regions that correspond to each of the following conditions. (a) pH depends only on the amount of excess strong aoid added ) the region with maximum bueing (e) pHi depends only on [8 (d) the sholhmrk (equivalence) point e)ph depends only om 1H
Consider the...
0/1 point Question 3 Which calculated titration curve only has 3 distinc strong acid/strong base reaction weak acid/strong base reaction strong acid/weak base reaction weak base/strong acid reaction 0/1 point Question 4 When a weak acid is titrated with a strong base. there are a total of 3 distinct regions of the titration curve that can be calculated the pH is high little titrant is present, but decreases as more of it is added. at no point during the titration,...
Part 3: Working with the Titration Curve for a Polyprotic Acid and Strong Base Consider carbonic acid, H.CO, (which is polyprotic) - a) Write the multi-step dissociation equilibrium for this acid in water (ie, there should be three chemical dissociation stages connected by two equilibrium arrows, given below): b) Below is an idealized titration curve showing the exhibited pH for 25.00 mL of a 0.100 M aqueous carbonic acid solution as a function of added 0.100 M NaOH in units...
Use the titration curve of a weak acid with a strong base below to answer the following questions. Identify the Equivalence Point of Titration and label it on the titration curve below. (ii) What is the Titrant (iii) From the graph, what is the [H^+] and the volume of NaOH used to reach the equivalence point. (iv) Calculate the [OH^-] at the equivalence point (v) What is the pKa of the acid used for titration? (vi) Calculate the Ka of...
An unknown acid is titrated with a strong base (NaOH) to produce
the above titration curve. Key points on this graph reveal
important information about the substance and the solution created
with it.
What volume of NaOH is needed to reach the equivalence point
(the point where you added equal moles of NaOH to the
acid)? Select one of the following : ["10 mL", "5
mL", "20 mL", "30 mL", "40 mL", "25 mL", "15 mL", "35 mL"]
...
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