1. Obtain the actual molarity of the HCI solUlUII ITUIIInclude in your formal lab report this value and possible sources of error for your experiment.2. Why is it important that the color change occurs by the addition of a single drop? Explain in terms ofits effect on the calculated molarity of the acid.3. Why is an Erlenmeyer flask preferred over a beaker when performing a titration?4. Suppose calcium hydroxide was used in this experiment instead of sodium hydroxide. Assuming allexperimental data was the same, what would be the molarity of the acid? Explain.5. Suppose there was a large air bubble in the tip of the acid burette during the titration and it wasdislodged toward the end of your titration. Explain the effect that this would have on the calculatedvalue of the acid's molarity.6. A student titrated 30.00 mL of a hydrochloric acid solution with 1.00 M sodium hydroxide. Thesodium hydroxide was initially filled to the 2.30 mL mark on the burette. Once the level in the burettereached 50.00 mL, the student was forced to refill the burette and did so to the 5.06 mL mark. Theendpoint was finally reached when the sodium hydroxide level dropped to 32.09 mL on theburette. What is the molarity of the acid solution? Show work.7. How many milliliters of a 0.250 M sulfuric acid solution would be required to completely react with2.398gramsof solid aluminum hydroxide? Work must be shown.

In the question 3 we have to tell that why erlenmeyer flask preferred over beaker while performing…

2. Why is it important that the color change occurs by the addition 8f a single ulUp! its effect on the calculated molarity of the acid. 3. Why is an Erlenmeyer flask preferred over a beaker when performing a titration? hydroxide was used in this experiment instead of sodium hydroxide. Assuming all

2. Why is it important that the color change occurs by the addition 8f a single ulUp! its effect on the calculated molarity of the acid. 3. Why is an Erlenmeyer flask preferred over a beaker when performing a titration? hydroxide was used in this experiment instead of sodium hydroxide. Assuming all

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 15Q: An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker...

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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?
Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a strong acid.
Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
A 2.500-g sample of a mixture of sodium carbonate and sodium chloride is dissolved in 25.00 mL of 0.798 M HCl. Some acid remains after the treatment of the sample. a Write the net ionic equation for the complete reaction of sodium carbonate with hydrochloric acid b If 28.7 mL of 0.108 M NaOH were required to titrate the excess hydrochloric acid, how many moles of sodium carbonate were present in the original sample? c What is the percent composition of the original sample?
Explain why the hydrolysis of salts makes it necessary to have available in a laboratory more than one acid-base indicator for use in titrations.
. 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.
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.
You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.
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.
When might a pH meter be better than an indicator to determine the end point of an acid-base titration?
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?
An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.