ilibria re (C,H5COOH) and any amount you need of sodium benzo- ate (CH5COONA). (a) What is the pH of the benzoic acid solution prior to adding sodium benzoate? (b) How many grams of sodium benzoate should be added to prepare the buffer? Neglect the small volume change that occurs when t. mmo- ade by 0.20 M t. i pH of ONa) nat is ium oт- L of the sodium benzoate is added. 17.27 A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.02 mol of KOH? (c) What is the pH of the buffer after the addi- 17.35 tion of 0.02 mol of HNO3? 17.28 A buffer contains 0.15 mol of propionic acid (C2H5COOH) and 0.10 mol of sodium propionate (C2H5COONa) in 1.20L. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.01 mol of NaOH? (c) What is the pH of the buffer after the addition of 0.01 mol of HI2 oic za- ng id of 17.29 (a) What is the ratio of HCO3 to H2CO3 in blood of pH 7 42 (b) What is the ratio of HCO3 to H2CO3 in an exhausted marathon runner whose blood pH is 7.1? 17.30 A buffer, consisting of H2PO4 and HPO,2-, helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. What is the pH of a soft drink in which the major buffer ingredients are 6.5 g of NaH2PO4 and 8.0 g of Na HPO4 per 355 mL of solution? 17.31 You have to prepare a pH = 3.50 buffer, and you have the v following 0.10 M solutions available: HCOOH, CH3COOH, H3PO4, HCOONa, CH3COONA, and NaH,PO4. Which solu- tions would you use? How many milliliters of each solution would you use to make approximately 1 L of the buffer? 25.0 ml %3D 17.32 You have to prepare a pH = 5.00 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONG; CH3COOH, CH;COONA, HCN, and NaCN. Which solu- tions would you use? How many milliliters of each solution would you use to make approximately 1 L of the buffer? 17.36 Acid-Base Titrations (Section 17 1)
Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
17.28 (a) use H-H equation
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