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The pH scale is used as a measure of acidity in the environment. In this lab you will learn to measure pH with a pH meter, determine the pH of some solutions, and investigate the properties of buffers.

The symbol pH is derived from the French for "hydrogen power." The numbers in the pH scale stand for negative logarithms (10^-n) of the concentration of hydronium ions (H₃O⁺), here verbally simplified to hydrogen ions (H⁺) expressed in moles per liter of water. To obtain a mole of any substance, you simply measure out its molecular weight in grams. One gram of hydrogen atoms is a mole; 44 grams of CO₂ is a mole; the atomic weight of C = 12, that of O = 16, and 12 + 2(16) = 44. A mole of any substance contains the same number of particles—Avogadro’s number, 6.02 x 10²³. The liter is a particular volume of water.

Thus a pH of 0 means a hydrogen ion concentration of 10⁰ molar or moles per liter, which is one mole.

Since normal dissociation of water molecules into H⁺ and OH^- yields 10^-7 moles of H⁺, pure water has a pH of 7, the neutral point in the scale. Since the pH scale is logarithmic, a difference in 1 unit is a 10-fold increase or decrease in concentration of hydrogen ions.

I. Measuring pH

Your instructor will demonstrate the use of the pH meter and of litmus paper. pH meters have been calibrated—DO NOT CHANGE ANY OF THE CONTROL SETTINGS.

Pour about 15 ml (enough to cover the pH meter electrode) of each solution into a small beaker.

• Lift electrode arm out fo the standard pH 7 buffer (yellow solution).
• Rinse electrode thoroughly using blue capped distilled water wash bottle.
• Dry electrode completely from top to bottom and in groove using Kimwipes.
• Lower electrode into test solution.
• Read pH from meter.
• Raise electrode and repeat rinsing procedure.
• Go on to next test solution.

Put a drop of each solution on pink and on blue litmus paper in a watch glass and record the color change. What is the effect of an acid and of a base on each color?

* clean the tip of the electrode thoroughly; detergent and soapy water both leave a film.

What would be the resulting pH if you mix equal amounts of an acid and a base that are the same numerical distance from neutrality (e.g., pH 5 + pH 9)?

II. Investigating the Properties of Buffers

Constant pH is maintained with buffers, which are solutions of weak acids or bases that either donate or accept hydrogen ions. Thus excess H+ is removed, and, when the addition of OH- uses up the H+ to form water, the H+ is replaced. In this exercise you will compare several solutions. Be sure to use equal volumes of liquid (water or buffer) in each beaker.

• Add acid (lemon juice) one drop at a time to an aqueous solution.
• Swirl the solution well to mix it after each drop is added; you can do this gently by moving the beaker with the pH meter electrode in the solution.
• Record the change in pH of the solution.

When you add acid, you expect the pH to decrease. For the first 20 drops of lemon juice you have added, using graph paper, plot the pH (on the y-axis) as a function of the number of drops of added lemon juice (on the x-axis). Compare the rate of the decrease in pH in the different solutions (water or buffer). Did the pH change at a uniform rate with each drop by drop addition of lemon juice?

Buffers act to resist changes in pH (either additions of acid or base). Buffers, however, have a limited capacity, and when you exceed that capacity, the pH changes rapidly. Organisms depend on the buffering capacity of their environment and on buffered solutions within their own bodies in order to tolerate fluctuations in acidity. Changes that exceed the capacity of the buffers will often kill the organisms. Almost all cellular chemistry takes place at pH's between 6 and 8.

When finished with the lab exercise, clean up:

• Rinse electrode of pH meter thoroughly, dry cmpletely and place back into standard pH 7 buffer (yellow solution).
• Dispose of all test solutions in the sink (they are household products). Do not discard the yellow standard buffer solution!
• Remove labels from all glassware.
• Rinse glassware thoroughly and return it to its original place.
• Wipe up any spills in your area.
• Leave the lab as it was when you began.

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