8th Edition

ISBN: 9781305856745

Author: DECOSTE

Publisher: CENGAGE LEARNING - CONSIGNMENT

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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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Textbook Question

Chapter 8, Problem 36E

How many moles of NaOH must be added to 1.0 L of 2.0 M HC 2 H 3 O 2 to produce a solution buffered at each pH?

a. pH = p K a

b. pH = 4.00

c. pH = 5 .00

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Chapter 8, Problem 35E

Chapter 8, Problem 37E

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Answer the following questions by circling the correct response. a. A0.100 M solution of NaOH has a higher pH than a 0.100 M solution of Ba(OH)2. TRUE / FALSE b. What is the pH of a solution made by dissolving Fe(NO:)2 in water? ACIDIC / NEUTRAL / BASIC c. If you have a buffer solution made from 1 parts ammonia and 2 parts ammonium ions, what is the pH of that solution? 8.95 / 9.55 d. You have a saturated solution of NH,CI with a small amount of undissolved NH,CI sitting at the bottom of the container. Adding which of the following would cause the solid NHẠCI to dissolve? Naci / HCI / NaOH e. The entropy of the universe increases when NaOH is dissolved into water. TRUE / FALSE

4. Formic acid, HFor, has a K, value equal to about 1.8 × 10-4. A student is asked to prepare a buffer having a pH of 3.55 from a solution of formic acid and a solution of sodium formate having the same molarity. How many milliliters of the NaFor solution should she add to 20. mL of the HFO solution to make the buffer? (See discussion of buffers.) -4 ka =18x10 pH= 355 pHs pka +1og ( conjugate base) (aud) 3.55= 3.744 + log () Pka= -logka = -log ( 1.0x104) =D 3.744 0.6397=/0.02 V= 0.0312 L V: 31.2 mL 31.2 mL 5. How many mL of 0.10 M NAOH should the student add to 20 mL 0.10 M HFor if she wished to prepare a buffer with a pH of 3.55, the same as in Problem 4? Ka= mL

Fill in the blanks: A buffer solution is consists of 0.100 M HCN and 0.200 M NaCN. HCN + H₂0 H30* + CN K₂ = 6.2 x 10-10 1. What is the pH of this solution? pH = 2. Calculate the pH if 0.025 M HCI is added to the solution. pH = 3. Calculate the pH 0.020 M NaOH is added to the solution (original). pH = Note: Type only your answer, expressed in 3 significant figures.

Chapter 8 Solutions

EBK CHEMICAL PRINCIPLES

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How many moles of NaOH must be added to 1.0 L of 2.0 M HC 2 H 3 O 2 to produce a solution buffered at each pH? a. pH = p K a b. pH = 4.00 c. pH = 5 .00

Solution Summary: The author explains how the Henderson-Hasselbalch equation is used to calculate the pH of a buffer solution.

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