Concept explainers
(a)
Interpretation:
The equation for reaction when
Concept Introduction:
On addition of limited amount of an acid or base, if a solution does not change the pH, it is known as buffer solution. For example: aqueous solution of weak acid and its conjugate base. This property of buffer to resist the pH is known as buffer action.
For an effective buffer, the value of pH is equal to the
(b)
Interpretation:
The equation for reaction when
Concept Introduction:
On addition of limited amount of an acid or base, if a solution does not change the pH, it is known as buffer solution. For example: aqueous solution of weak acid and its conjugate base. This property of buffer to resist the pH is known as buffer action.
For an effective buffer, the value of pH is equal to the
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Check out a sample textbook solutionChapter 8 Solutions
Introduction to General, Organic and Biochemistry
- 8-53 Write equations to show what happens when, to a buffer solution containing equimolar amounts of CH3COOH and CH3COO-, we add: (a) H3O (b) OH-arrow_forward8-96 Suppose you want to make a CH3COOH/CH3COO- buffer solution with a pH of 5.60. The acetic acid concentration is to be 0.10 M. What should the acetate ion concentration be?arrow_forward8-54 Write equations to show what happens when, to a buffer solution containing equimolar amounts of HPO42- and H2PO4-, we add (a) H3O+ (b) OH-arrow_forward
- 8-110 A concentrated hydrochloric acid solution contains 36.0% HCI (density 1.18 = g/mL). How many liters are required to produce 10.0 L of a solution that has a pH of 2.05?arrow_forward8-103 Suppose you have a phosphate buffer (H2PO4-/HPO42-) of pH 7.21. If you add more solid NaH2PO4 to this buffer, would you expect the pH of the buffer to increase, decrease, or remain unchanged? Explain.arrow_forward8-107 Following are pH ranges for several human biological materials. From the pH at the midpoint of each range, calculate the corresponding [H3O+]. Which materials are acidic, which are basic, and which are neutral? (a) Milk, pH 6.6-7.6 (b) Gastric contents, pH 1.0-3.0 (c) Spinal fluid, pH 7.3-7.5 (d) Saliva, pH 6.5-7.5 (e) Urine, pH 4.8-8.4 (f) Blood plasma, pH 7.35-7.45 (g) Feces, pH 4.6-8.4 (h) Bile, pH 6.8-7.0arrow_forward
- 8-44 What is the molarity of a solution made by dissolving 3.4 g of Ba(OH)2 in enough water to make 450 mL of solution? Assume that Ba(OH)2 ionizes completely in water to Ba2+ and OH- ions. What is the pH of the solution?arrow_forward8-41 What is the [OH-] and pOH of each solution? (a) 0.10 M KOH, (b) 0.10 M Na2CO3, (c) 0.10 M Na3PO4, (d) 0.10 M NaHCO3,arrow_forward8-50 The usual concentration of HCO3- ions in blood plasma is approximately 24 millimoles per liter (mmol/L). How would you make up 1.00 L of a solution containing this concentration of HCO3- ions?arrow_forward
- 8-33 Write an equation for the reaction of HCI with each compound. Which are acid—base reactions? Which are redox reactions? (a) Na2CO3 (b) Mg (c) NaOH (d) Fe2O3 (e) NH3 (f) CH3NH2 (g) NaHCO3 (h) AIarrow_forward8-51 What is the end point of a titration?arrow_forward8-112 Consider an initial 0.040 M hypobromous acid (HOBr) solution at a certain temperature. At equilibrium after partial dissociation, its pH is found to be 5.05. What is the acid ionization constant, Ka, for hypobromous acid at this temperature?arrow_forward
- Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning