Microbiology With Diseases By Taxonomy (6th Edition)
6th Edition
ISBN: 9780134832302
Author: Robert W. Bauman Ph.D.
Publisher: PEARSON
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What determines a molecule’s solubility or lack of solubility inwater?
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- pH expresses the molar concentration of hydronium ions in an aqueous solution on a logarithmic scale. (Note that it is common to use the hydrogen ion, H*, to represent the hydronium ion, H3O+.) pH = -log[H3O+] [H3O+] = 10-PH As pH decreases, acidity increases. As pH increases, acidity decreases. • Acidic solution: pH 7 Part A - Calculating pH Submit [H₂0+] 1 Acidic pH 01 10¹ 102 103 104 105 106 107 108 109 10-10 10-11 10-12 10-13 10-14 stomach acid 3 wine lemon tomatoes juice vinegar, black soft drinks, coffee beer 6 Neutral urine milk 7 human blood pure water sea- water baking soda 10 11 12 13 14 milk of magnesia house- hold ammonia oven cleaner Basic household bleach Adapted from Biological Science by Freeman ©2008 Pearson Education, Inc. What is the pH of an aqueous solution with the hydronium ion concentration [H3O+] = 2 x 10-14 M? Make sure that your answer has the correct number of significant figures. For help determining the correct number of significant figures, see Hint 3. ►…arrow_forwardIbuprofen, widely used as a pain reliever, has limited solubility in water, less than 1 mg>mL. Which part of the molecule’s structure (gray, white, red) contributes to its water solubility? Which part of the molecule (gray, white, red) contributes to its water insolubility?arrow_forwardHow is the molality of a solution different from its molarity?arrow_forward
- Why can amino acids act as buffers in certain pH range? Refer to the structure of amino acids in your answer.arrow_forwardWhat is NOT TRUE about buffers ?arrow_forwardWhat is the pH of the solution given the following information? Methyl orange = yellow Methyl red = yellow Bromothymol blue = green Note: use the provided reference table for color indicators below as a guide pH 5 pH 8 pH 7 pH 6arrow_forward
- What is the effect of adding a small amount of a strong acid or strong base to the acidity of a buffer? How would this compare to an unbuffered solution of the same acidity?arrow_forwardYou have a buffer with a pH of 10. You add a little bit of weak acid. What most likely will happen? a) The pH goes to 7 b) The pH should stay at 10 c) The pH goes up to 11 d) The pH goes down to 9arrow_forwardI want to make a buffer solution containing 1 M glycene pH = 10 (Na+), 1 mM ZnCl2 , 1 mM MgCl2. I have the stock solutions 1 M glycene, 1 M MgCl2, 1 M ZnCl2, and 10 M NaOH. My final volume of buffer solution needs to be 250ml. how much (in ml) of each solution should i put into my buffer?arrow_forward
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