The hydrochloric acid concentration in a solution is determined by titration with NaOH. A 25.00 mL aliquot of the sample requires 20.98 mL of NaOH solution. The NaOH is standardized against oxalic acid (H2C204).A 0.2351 g sample of the acid requires 24.06 mL of NaOH (the acid is diprotic). What is the formality of the HCI in the sample?Formality of HCI (use 4 significant digits):Only a number required. Computer reads units of "F". Tries 1/3 Previous TriesSubmit AnswerIf a 25.00 mL pipet can be used with a precision of ±0.02 mL, a balance with ±0.2 mg, and a buret with ±0.02 mL, what is the expected absolute precision of the formality? Remember that each mass is the resultof two weighings and each volume from a buret is the result of two readings.Absolute SD in formality (use 2 ignificant digits):Submit AnswerTries 0/3

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The hydrochloric acid concentration in a solution is determined by titration with NaOH. A 25.00 mL aliquot of the sample requires 20.98 mL of NaOH solution. The NaOH is standardized against oxalic acid (H2C204). A 0.2351 g sample of the acid requires 24.06 mL of NaOH (the acid is diprotic). What is the formality of the HCI in the sample? Formality of HCI (use 4 significant digits):

The hydrochloric acid concentration in a solution is determined by titration with NaOH. A 25.00 mL aliquot of the sample requires 20.98 mL of NaOH solution. The NaOH is standardized against oxalic acid (H2C204). A 0.2351 g sample of the acid requires 24.06 mL of NaOH (the acid is diprotic). What is the formality of the HCI in the sample? Formality of HCI (use 4 significant digits):

Chemistry

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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 128CP: Consider the titration curve in Exercise 115 for the titration of Na2Cr3 with HCl. a. If a mixture...

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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.
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?
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.
Consider the titration curve in Exercise 115 for the titration of Na2Cr3 with HCl. a. If a mixture of NaHCO3 and Na2CO3 was titrated, what would be the relative sizes of V1, and V2? b. If a mixture of NaOH and Na2CO3 was titrated, what would be the relative sizes of V1 and V2? c. A sample contains a mixture of NaHCO3 and Na2CO3. When this sample was titrated with 0.100 M HCl, it took 18.9 mL to reach the first stoichiometric point and an additional 36.7 mL to reach the second stoichiometric point. What is the composition in mass percent of the sample?
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?
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.
Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
A 5.36-g sample of NH4Cl was added to 25.0 mL of 1.00 M NaOH and the resulting solution diluted to 0.100 L.. (a) What is the pH of this buffer solution?. (b) Is the solution acidic or basic?. (c) What is the pH of a solution that results when 3.00 mL of 0.034 M HCl is added to the solution?
Consider 1.0 L of an aqueous solution that contains 0.10 M sulfuric acid to which 0.30 mole of barium nitrate is added. Assuming no change in volume of the solution, determine the pH, the concentration of barium ions in the final solution, and the mass of solid formed.
Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a strong acid.
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 student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.

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