subners before submitting.The titration of 25.0 mL of an unknown concentration of HCI solution requires 139.9 mL of 0.23 MNAOH solution. What is the concentration of the HCI solution (in Molarity)?uestion 30(Hint - Carefully balance the equation first!)Next* PreviousSubmitNot savedMacBook Air80888F5F7F8F9F6F2F3F4F1#3&$4*36.789.QRTY UAFHJKVw/

Titration: Titration is a common laboratory method of quantative chemical analysis to determine the…

ers before submitti nestion 30 The titration of 25.0 mL of an unknown concentration of HCI solution requires 139.9 mL of 0.23 M NAOH solution. What is the concentration of the HCI solution (in Molarity)? (Hint- Carefully balance the equation first!!) Next

ers before submitti nestion 30 The titration of 25.0 mL of an unknown concentration of HCI solution requires 139.9 mL of 0.23 M NAOH solution. What is the concentration of the HCI solution (in Molarity)? (Hint- Carefully balance the equation first!!) Next

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.30QAP

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Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

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ers before submitting.
The titration of 25.0 mL of an unknown concentration of HCI solution requires 139.9 mL of 0.23 M
NAOH solution. What is the concentration of the HCI solution (in Molarity)?
uestion 30
(Hint - Carefully balance the equation first!)
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Consider the following two acids: In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results. (See Exercise 113.)
Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong acid HA with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: (a) After a very small volume of titrant has been added to the initial HA solution? (b) Halfway to the equivalence point? (c) When enough titrant has been added to take the solution just past the equivalence point? (d) At the equivalence point? Nanoscale representations for Question 111.
What acid-base indicators, shown in Figure 18.24 would be suitable for the neutralization reaction whose titration curve is shown in Figure 18.30?Why?
Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
If 55 mg of lead(II) sulfate is placed in 250 mL of pure water, does all of it dissolve? If not, how much dissolves?
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a strong acid.
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?