(a)
Interpretation:
The strongest acid should be identified.
Concept introduction:
Titration is a process that determines the concentration of solution by known volume to react with a standard solution of another substance.
titration curve is a plot of pH of solution versus volume of titrant. The shape of titration curve identifies the equivalence point in titration.
The point at which equivalent quantity of acid and base have been mixed together is called equivalent point. at equivalence point depends upon the relative strength of acids or bases.
is defined as the acid dissociation constant in conjugate acid-base pairs. is defined as the base ionization constant in acid-base pairs. is the equilibrium constant for water. At is equal to
The expression for relation between and is as follows:
Rearrange above equation for
Rearrange above equation for
At is equal to the equation will be modified as follows:
(b)
Interpretation:
The weakest acid should be identified.
Concept introduction:
Titration is a process that determines the concentration of solution by known volume to react with a standard solution of another substance.
titration curve is a plot of pH of solution versus volume of titrant. The shape of titration curve identifies the equivalence point in titration.
The point at which equivalent quantity of acid and base have been mixed together is called equivalent point. at equivalence point depends upon the relative strength of acids or bases.
is defined as the acid dissociation constant in conjugate acid-base pairs. is defined as the base ionization constant in acid-base pairs. is the equilibrium constant for water. At is equal to
The expression for relation between and is as follows:
Rearrange above equation for
Rearrange above equation for
At is equal to the equation will be modified as follows:
Want to see the full answer?
Check out a sample textbook solutionChapter 17 Solutions
CHEMISTRY-MOD.MASTERING (18W)
- Consider the titration of HF (K a=6.7104) with NaOH. What is the pH when a third of the acid has been neutralized?arrow_forwardThe major component of vinegar is acetic acid, CH3COOH. Its Ka is 1.8 × 10-5 . One student used 1.000 M NaOH to titrate 25.00 mL vinegar. At the end point, 21.82 mL NaOH was used. (a) What is the concentration of CH3COOH in vinegar? (b) What is the pH of the solution at the end point? (c) What indicator(s) the student should use in this titration? Explainarrow_forward2.0 g of NaOH is dissolved in distilled water to prepare 100 mL solution. 20.0 mL of this solution reaches to the equivalence point when 25 mL of an acid solution containing 1.22 monoprotic weak acid is added. (a) Calculate the molar mass of the unknown acid. (b) After 15.0 mL of NaOH solution had been added during the titration, the pH was determined to be 4.7. What is the Ka of the unknown acid? (NaOH = 40.0 g/mol) unknownarrow_forward
- Consider the titration of 36.0 mL of 0.117 M ammonia with 0.0752 M HCl. (See the Acid-Base Table.) (a) How many mL of HCl are required to reach the equivalence point?5.60 mL(b) What is the pH at the equivalence point? 5.30(c) What is the pH of the solution after the addition of 15.7 mL of acid? (d) What is the pH of the solution after the addition of 82.9 mL of acid? only need part c and d pleasearrow_forwardConsider the titration of 36.0 mL of 0.123 M ammonia with 0.0766 M HCl. (See the Acid-Base Table attached.) (a) How many mL of HCl are required to reach the equivalence point?57.8 mL(b) What is the pH at the equivalence point? 5.29(c) What is the pH of the solution after the addition of 17.2 mL of acid? (d) What is the pH of the solution after the addition of 84.3 mL of acid? (only need help witn c and d)arrow_forward4) A highly toxic hydrogen cyanide (HCN) is a weak acid. A chemical engineer plans to determine pH of a 50 mL sample of HCN (0.10 M) in a titration process. To this end, she used 0.20 M NaOH as a titrant in varying volumes. Calculate the pH of the solution at the following points: (Ka for HCN=6.2×10-¹0) (a) Before addition of NaOH (initial pH), (b) After 10.00 mL of titrant addition, (c) After 25.00 mL of titrant addition, (d) After 50.00 mL of titrant addition.arrow_forward
- In each of the following questions, assume that there is no volume change when HCl is added to water in part (a) or the phosphate buffer in part (c). (a) Calculate the pH when 0.091 moles of HCl are added to 1.000 liter of water. (b) What is the difference between the pH of pure water (pH 7.00) and the pH of the solution after HCl was added? (c) Calculate the pH when 0.091 moles of HCl are added to 1.000 liters of a buffer containing 0.352M KH2PO4 and 0.321 M K2HPO4. (d) The pH before the HCl was added is equal to 7.168. What is the difference between the pH before adding the HCl and after adding the HCl?arrow_forwardA mixture of 100 ml of 0.025 M NH3 and 150 mL of 0.025 M NH4Cl was made. For this problem you need to show your calculation for each number. (A) What is the resulting concentration of the two solutes after mixing the solutions?(B) What is the pH of the solution produced?(C) What will happen if additional 100 mL water is added to the mixture?arrow_forwardA 0.018 M solution of salicylic acid, HOC6H4CO2H, has the same pH as 0.0038 M HNO3solution. (a) Write an equation for the ionization of salicylic acid in aqueous solution. (Assume only the –CO2H portion of the molecule ionizes.) (b) What is the pH of solution containing 0.018 M salicylic acid? (c) Calculate the Ka of salicylic acid.arrow_forward
- For the titration of 10.0 mL of 0.200 M acetic acid with 0.150 M sodium hydroxide, determine the pH when: (a) 10.0 mL of base has been added.(b) 13.3 mL of base has been added. (c) 16.6 mL of base has been added.arrow_forward6. (a) Consider the pH of a solution containing a weak acid, HA , and a soluble salt of the weak acid, such as NaAarrow_forwarda.) A student titrated 50.0mL of a 0.10M solution of a certain weak acid with NaOH(aq). The results are given in the graph attached. (i) What is the approximate pKa of the acid? (ii) What specific value from the graph is needed, in addition to the information in part (a) above, to calculate the molar concentration of the NaOH(aq) ? (iii) Identify a pH value between 2.5 and 7.5 at which the concentration of the weak acid being titrated is less than the concentration of its conjugate base.arrow_forward
- Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage LearningChemistry for Today: General, Organic, and Bioche...ChemistryISBN:9781305960060Author:Spencer L. Seager, Michael R. Slabaugh, Maren S. HansenPublisher:Cengage Learning
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage Learning