Interpretation:
The compound listed in Table 8-6 that is most effective for making a buffer at pH 7.0 should be identified.
Concept Introduction:
The buffer consists of zwitter ions molecules which have both positive and negative charges. They are concentration and temperature change resistant. To understand the buffer it is not important to know its structure only the
Here, pH is negative log of hydrogen ion,
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- 8-93 Do a 1.0 M CH3COOH solution and a 1.0 M HCI solution require the same amount of 1.0 M NaOH to hit a titration end point? Explain.arrow_forward8-60 How is the buffer capacity affected by the ratio of the conjugate base to the conjugate acid?arrow_forward8-94 Suppose you wish to make a buffer whose pH is 8.21. You have available 1 L of 0.100 M NaH2PO4 and solid Na2HPO4. How many grams of the solid Na2HPO4 must be added to the stock solution to accomplish this task? (Assume that the volume remains 1 L.)arrow_forward
- 8-71 Explain why you do not need to know the chemical formula of a buffer compound to use it.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_forward8-55 We commonly refer to a buffer as consisting of approximately equal molar amounts of a weak acid and its conjugate base—for example, CH3COOH and CH3COO-. Is it also possible to have a buffer consisting of approximately equal molar amounts of a weak base and its conjugate acid? Explain.arrow_forward
- 8-101 Suppose you have an aqueous solution prepared by dissolving 0.050 mol of NaH2PO4 in 1 L of water. This solution is not a buffer, but suppose you want to make it into one. How many moles of solid Na2HPO4 must you add to this aqueous solution to make it into: (a) A buffer of pH 7.21 (b) A buffer of pH 6.21 (c) A buffer of pH 8.21arrow_forward8-53 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_forward8-68 If you have 100 mL of a 0.1 M buffer made of NaH2PO4 and Na2HPO4 that is at pH 6.8 and you add 10 mL of 1 M HCI, will you still have a usable buffer? Why or why not?arrow_forward
- 8-63 The pH of a solution made by dissolving 1.0 mol of propanoic acid and 1.0 mol of sodium propanoate in 1.0 L of water is 4.85. (a) What would the pH be if we used 0.10 mol of each (in 1 L of water) instead of 1.0 mol? (b) With respect to buffer capacity, how would the two solutions differ?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_forward8-115 When a solution prepared by dissolving 0.125 g of an unknown diprotic acid in 25.0 mL of water is titrated with 0.200 M NaOH, 30.0 ml, of the NaOH solution is needed to neutralize the acid. Determine the molarity of the acid solution. What is the molar mass of the unknown diprotic acid?arrow_forward
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