CHEM 1004 Chapter Notes - Chapter 15: Omeprazole, Histamine Receptor, Esomeprazole

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1 May 2014

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Antacid medications - mostly otc, but prescription needed for acid reflux drugs. Ph - the symbol for acidity, represents the "power of the hydrogen (or hydronium) ion" The ph of a solution is a measure of the acidity of that solution. [h3o+] or [h+] = 0. 0000001m = 1 x 10-7 m ph = - log. Express concentration. as power of 10 = - log(10-7) The ph of an acidic solution is less than 7. The ph of a neutral solution equals 7. The ph of a basic solution is greater than 7. Ph of 1 is 10 times more acidic than a ph of 2 and 100 times more acidic than a ph of 3. A ph of 14 is 10 times more basic than a ph of 13 and 100 times more acidic than a ph of 12. Alka seltzer - effervescent antacid and pain reliever!

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Exp 25. pH Measurements- Buffers and Their Properties

I need help with finding kPa in the calculations part C for 1,2, and 3 Thanks!

Experiment 25 pH Measurements- Buffers and Their Properties ne of the more important propertics of an aqucous solution is its concentration of hydrogen ion. The H ion (or, more precisely, the HO ion) has a great effect on the solubility of many inorganic and organic species, on the nature of complex mctallic cations found in solutions, and on the rales of many chemical reac- tions. It is important that we know how to measure the concentration of hydrogen ion and understand its effect on solution properties. For convenience, the concentration of H' ion is frequendly expressed as the pH of the solution rather than as molarity. The pH of a solution is defined by the following equation: pH =-log where the logarithm is taken to the base 10. If [H] is I x 10-*moles per liter, the pH of the solution is, by the equation, 4. If the [H'1 is 5 x 10 M, the pH is 1.3, Basic solutions can also be described in terms of pH. In aqucous solutions the following equilibrium rela- tion will always be obeyed: In distilled water url equals [ OHÂ·], s, by Equation 2, [HÂ·l must be l x 10" M. Therefore, the pH of distilled water is 7. Solutions in which [H.] > 10é¨are sad to be acidic and will have a pH 7. A solution with a pH of 10 will have a [H"] of 1 x 10 0 M and a (OH] of I x 10M We measure the pH of a solution experimentally in two ways. In the first of these we use a chemical called an indicator, which is sensitive to pH. These substances have colors that change over a relatively short pH range (about two pH units) and can, when properly chosen, be used to delermine roughly the pH of a solu tion. Two very common indicators are litmus, usually used on paper, and phenolphthalein, the most common indicator in acid-base titrations. Litmus changes from red to blue as the pH of a solution goes from about 6 to about 8. Phenolphthalein changes from colorless to red as the pH goes from 8 to 10. A given indicator is useful for determining pH only in the region in which it changes color. Indicators are available for measure- ment of pH in all the important ranges of acidity and basicity. By matching the color of a suitable indicator in a solution of known pH with that in an unknown solution, one can determine the pH of the unknown to within about 0.3 pH units. The other method for finding pH is with a device called a pH meter. In this device two electrodes, one of which is sensitive to [H']. are immersed in a solution. The potential between the two electrodes is related to the pH. The pH meter is designed so that the scale will directly furnish the pH of the solution. A pH meter gives much more precise measurement of pH than does a typical indicator and is ordinarily used when an accurate determination of pH is needed Some acids and bases undergo substantial ionization in water, and are called strong because of their essentially complete ionization in reasonably dilute solutions. Other acids and bases, because of incomplete ionization (often far less than even 1% in 0.1 M solution), are called weak. Hydrochloric acid, HC, and sodium hydroxide, NaOH, are typical examples of a strong acid and a strong base. Acetic acid, HC,H,0, and ammonia, NH, are classic examples of a weak acid and a weak base. A weak acid will ionize according to the Law of Chemical Equilibrium: HBlaq)--H'(aq) + B-(aq)

x.Hm1. Which chemical equation shows the dissociation of 2 protonsfrom trihydrogen phosphate (phosphoric acid)? (Points: 1)
H₃PO₄Â®H₂⁺ + HPO₄Â¯
H₃PO₄Â®H₂²⁺ + PO₄²Â¯
H₃PO₄Â®2H⁺ + HPO₄²Â¯
H₃PO₄Â®H₃³⁺ + PO₄³Â¯

2. When dissolved in water, hydrogen bromide(HBr)forms hydrobromic acid. Determine the hydroxide ion concentrationina 4,500 mL solution containing 3.78 g hydrogen bromide;K_w = 1.00 Â´ 10Â¯¹⁴. (Points: 1)
[OHÂ¯] = 9.63 Â´ 10Â¯¹³M
[OHÂ¯] = 2.14 Â´ 10Â¯¹³M
[OHÂ¯] = 4.67 Â´ 10Â¯²M
[OHÂ¯] = 0.0104 M

3. The hydronium ion concentration in asolutionwith pH 10 is __________ than the hydronium ion concentrationin asolution with pH 13. (Points: 1)
1,000 times less
3 times greater
1,000 times greater
100 times less

4. Which reaction most accurately represents thedissociation of nitrous acid (HNO₂) in water? (Points:1)
HNO₂ +H₂O Â® H₃O⁺ + NO₂Â¯
HNO₂ +H₂O Â® H₃O₂⁺ + NOÂ¯
HNO₂ +H₂O Â® HN + HO⁺ + HO₂Â¯
HNO₂ +H₂O Â® H₃O⁺ + N +O₂Â¯

5. The acid neutralizing capacity of a lakeorstream most often derives from the presence of _______ inthesurrounding soil or rock. (Points: 1)
CaCO₃
HNO₃
NaCl
Sr(OH)₂

6. Bases produce which ions in aqueous solution?(Points: 1)
OHÂ¯
NO₂Â¯
ClÂ¯
SO₃Â¯

7. The primary product of the combustion of sulfuris: (Points: 1)
H₂S
H₂SO₄
H₂SO₃
SO₂

8. Which solution is acidic? (Points: 1)
M_OHÂ¯ = 0.0065M
M_H+ = 1.27 Â´10Â¯⁹ M
M_H+ = 5.79 Â´10Â¯¹⁰ M
M_OHÂ¯ = 1.77 Â´10Â¯¹⁰ M

9. An acidic fog in Pasadena was found to have apH of 2.50. Which expression represents this pH measurement?(Points: 1)
M_OHÂ¯ = 3.2 Â´10Â¯¹² M
M_OHÂ¯ = 3.2 Â´10Â¯⁹ M
M_H+ = 9.7 Â´10Â¯³ M

CHEM 1004 Chapter Notes - Chapter 15: Omeprazole, Histamine Receptor, Esomeprazole

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