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pH is a measure of how acidic or basic a substance is. It is measured on a scale from 0 to 14, with 7 being neutral. A pH less than 7 is acidic and a pH greater than 7 is basic.
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Solved in 2 steps
- 1. Calculate the pH of a buffer solution made from 0.20 M CH3COOH and 0.50 M CH3COO- that has an acid dissociation constant for CH3COOH of 1.8 x 10-5.2. Calculate the pH of a buffer containing 0.1 M sodium acetate and 0.2 M acetic acid (pKa = 4.76).2. Four unidentified solutions of equal concentration (0.1 mol/L) were prepared by chemistry students who were investigating the properties of acids and bases. Solution Red litmus Blue litmus pH Conductivit Blue No change 13.2 Very high 2 No change Red 3.5 Weak 3 No change Red 1.8 Very high 4 Blue No change 10.7 Weak Identify the acids and the bases in the list above. b. Classify the acids and the bases as being weak or strong with supporting information. Suggest another test that could be used to determine the relative strengths of the acids.
- 4. A 100-mL buffer solution with pH of 4.80 is prepared as a stock solution. Using this stock buffer solution, three buffers are prepared by diluting a given volume of the stock buffer (as shown below) to 100 mL with water. Volume used from Buffer Final volume, mL original solution, mL 1 5 100 2 10 100 20 100 a. Do they have the same pH? Check the box corresponding your answer. O Yes O No HY 47.1 Basic Biochemistry, Laboratory b. Which is true about their absolute concentrations? Check the box corresponding your answer. [Buffer 1] > [Buffer 2] > [Buffer 3] [Buffer 3] > [Buffer 2] > [Buffer 1] [Buffer 3] = [Buffer 2] = [Buffer 1] [Buffer 3] = [Buffer 2] > [Buffer 1] [Buffer 3] > [Buffer 2] = [Buffer 1] c. Which is true about their concentration ratios? Check the box corresponding your answer. [Buffer 1] > [Buffer 2] > [Buffer 3] [Buffer 3] > [Buffer 2] > [Buffer 1] [Buffer 3] = [Buffer 2] = [Buffer 1] [Buffer 3] = [Buffer 2] > [Buffer 1] [Buffer 3] > [Buffer 2] = [Buffer 1] %3! %3D d.…2. You are given 575mL of a .200M solution of NaOH and are adding 600mL of water What is the new concentration?1.Write the equation for the dissociation and re-formation of water
- 1. What volumes of 50 mM CH3COOH and 30 mM NaCH3CO0 solutions are needed to prepare 2L of 20 mM acetate buffer pH 3.6? (pka for acetic acid is 4.74)4. In a solution, the medium in which atoms/ions/molecules are dispersed is the and the dispersed substances are called the pH Scale4. A buffer can protect against changes in pH when hydrogen ion or hydroxide ion is added to a reaction mixture. Explain the reason.
