Concept explainers
(a)
Interpretation: The titration curve of
Concept introduction: Titration is a quantitative chemical analysis method that is used for the determination of concentration of an unknown solution. In
To determine: The size of
(b)
Interpretation: The titration curve of
Concept introduction: Titration is a quantitative chemical analysis method that is used for the determination of concentration of an unknown solution. In acid base titration, the neutralization of either acid or base is done with a base or acid respectively of known concentration. This helps to determine the unknown concentration of acid or base.
To determine: The size of
(c)
Interpretation: The titration curve of
Concept introduction: Titration is a quantitative chemical analysis method that is used for the determination of concentration of an unknown solution. In acid base titration, the neutralization of either acid or base is done with a base or acid respectively of known concentration. This helps to determine the unknown concentration of acid or base.
To determine: The mass percentage of
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Chemistry: An Atoms First Approach
- 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.arrow_forwardA 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?arrow_forwardwhat is the Molarity of the NaOH solution? Mass of H2C2O4·2H2O=1.32191 g Volume of the H2C2O4·2H2O solution=250.0 mL Volume of NaOH solution used in titration=21.45 mLarrow_forward
- 0.3174 g sample of an unknown acid requires 26.23 mL of 0.1056 M NaOH for neutralization to a phenolphthalein end point. There are 0.27 mL of 0.1096 M HCl used for back-titration. a. How many moles of OH− are used? How many moles of H+ from HCl? b. How many moles of H+ are there in the solid acid? c. What is the molar mass of the unknown acid?arrow_forward1.exactly 25 ml of 0.01M HCL was taken diluted with sufficient quantity of water to measure 250ml and titrated with 0.025N NaOH A. write the equilibrium reaction B. normality of the resulting solution of HCL C. pH before the titrant is added D. pH after 5 ml of titrant is added E. pH after 9 ml of titrant is added F. pH after 14 ml of titrant is added G. pH after 18 ml of titrant is added H. volume of the titrant that would produce the stoichiometric point I. pH at stoichiometric point J. illustrate how the titration curve would look likearrow_forward(a.) Titration of a 12.0 mL solution of HCl requires 22.4 mL of 0.12 M NaOH. What is the molarity of the HCl solution? (b.) Titration of a 10.0 mL solution of NH3 requires 15.0 mL of 0.0250 M H2SO4. What is the molarity of the NH3 solution?arrow_forward
- A titration of 25.00 mL of an unknown HCl solution with 0.1240 M NaOH starts at a buret reading for NaOH of 0.53 mL. The phenolphthalein indicator turns light pink in the acid solution for over 30 seconds at a buret reading of 27.30 mL. 5. What was the volume of NaOH dispensed? 6. How many moles of NaOH were dispensed? 7. Write the balanced molecular equation for the neutralization reaction: 8. How many moles of HCl are present in the acid solution? 9. What is the molarity of the unknown HCl solution?arrow_forward36.78 mL of 0.0105 M HCl is required to reach the equivalence point in the titration of 25.0 mL of an ammonia solution. Kb(NH3) = 1.8x10-5. What was the original concentration of NH3 before the titration began?arrow_forward1. How many mL of 3 M NaOH are required to make a 1 L solution of 0.1 M NaOH? 2. A student placed 10.00 mL of a hydrochloric acid solution in an Erlenmeyer flask. She then added 16.6 mL DI water and 2 drops 0.2% phenolphthalein solution. During the titration, a faint, pale pink color was observed when 18.50 mL of 0.262 M barium hydroxide had been added. Calculate the concentration (in M) of the original hydrochloric acid solution.arrow_forward
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