Lecture_Notes_091809b

Lecture_Notes_091809b - The [H+] of a certain solution is...

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Unformatted text preview: The [H+] of a certain solution is 0.00345 M. What is the pOH of this solution? 2.46 2. 11.53 3. 1.46 4. Cannot be determined 1. 7% .5 3 2. 46 89% 3% 1. 46 1% m in e d 11 C an n ot be de te r Using pH Given the following pH’s for various biological fluids, calculate the concentration of H+ and OH- present: Gastric Juice: pH = 2.0 Spinal Fluid: pH = 7.4 Bile: pH = 6.9 Using pH The pH of 0.040 M hypobromous acid (HOBr) is 5.05. Set up the equilibrium equation for the dissociation of HOBr, and calculate the value of the acid dissociation constant. Calculating pH Phenol (C6H5OH) is a weak acid used as a general disinfectant and in the manufacture of plastics. Calculate the pH and the concentrations of all species present in a 0.10 M solution of phenol, Ka = 1.3 x 10-10. Percent Dissociation One way to describe to what extent an acid has dissociated is with percent dissociation. Percent Dissociation Calculate the pH and the percent dissociation in 1.5 M HNO2, Ka = 4.5 x 10-4. Steps for Solving a Acid Equilibrium Problem 1. 2. 3. 4. 5. 6. Choose the species that can produce H+ and write the balanced equations. Using the values for the Ka for the acids decide which reaction dominates producing the most H+. Write the equilibrium expression for the dominant reaction. Make ICE table. Solve for x, making any possible assumptions. Calculate [H+], pH or % dissociation, whatever you are asked for. A Solution Containing 2 or more Weak Acids Find the pH of a mixture that contains 0.150 M HF (Ka = 3.5 x 10-4) and 0.100 M HClO (Ka = 2.9 x 10-8). What is the hypochlorite ion concentration at equilibrium? A Solution Containing 2 or more Weak Acids Bases Strong Bases – soluble hydroxide salts, such as NaOH, Ca(OH)2, KOH, etc. Weak Bases – molecules or ions that accept an H+ ion from water leaving behind an OH- ion. ...
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Lecture_Notes_091809b - The [H+] of a certain solution is...

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