BIOCHEMISTRY BOOKS ALC&MOD MST/ET PKG
1st Edition
ISBN: 9780134172507
Author: APPLING
Publisher: Pearson Education
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Chapter 2, Problem 6P
The weak acid HA is 2% ionized (dissociated) in a 0.20 M solution.
a. What is Ka for this acid?
b. What is the pH of this solution?
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Chapter 2 Solutions
BIOCHEMISTRY BOOKS ALC&MOD MST/ET PKG
Ch. 2 - Suppose a chloride ion and a sodium ion are...Ch. 2 - Draw two different possible hydrogen-bonding...Ch. 2 - Prob. 3PCh. 2 - 4. What is the pH of each of the following...Ch. 2 - Prob. 5PCh. 2 - The weak acid HA is 2% ionized (dissociated) in a...Ch. 2 - 7. Calculate the pH values and draw the titration...Ch. 2 - What is the pH of the following buffer mixtures?...Ch. 2 - a. Suppose you wanted to make a buffer of exactly...Ch. 2 - Prob. 10P
Ch. 2 - You need to make a buffer whose pH is 7.0, and you...Ch. 2 - Describe the preparation of 2.00 L of 100 glycine...Ch. 2 - Carbon dioxide is dissolved in blood (pH 7.4) to...Ch. 2 - What is the molecular basis for the observation...Ch. 2 - The anno acid arginine ionizes according to the...Ch. 2 - It is possible to make a buffer that functions...Ch. 2 - A student is carrying out a biological preparation...Ch. 2 - Histidine is an amino acid with three titratable...Ch. 2 - Prob. 19PCh. 2 - Prob. 20PCh. 2 - Prob. 21P
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- A solution with a density of 0.876 g>mL contains 5.0 g of toluene 1C7H82 and 225 g of benzene. Calculate the molarity of the solution.arrow_forwardThe weak acid HA is 2% ionized (dissociated) in a 0.20 M solution. (a) What is Ka for this acid? (b) What is the pH of this solution?arrow_forwardTomato juice has a OH- concentration equal to 1 X 10 -10, what is the pH of this solution?arrow_forward
- A 0.10 M solution of the deadly poison hydrogen cyanide, HCN, has a pH of 5.2. Calculate the [H3O+] of the solution. Is HCN a strong or a weak acid?arrow_forwardConsider a buffer solution that contains 0.55 M NH2CH2CO2H and 0.35 M NH2CH2CO2Na. pKa(NH2CH2CO2H)=9.88. a. Calculate its pH. b. Calculate the change in pH if 0.155 g of solid NaOH is added to 250 mL of this solution. c. If the acceptable buffer range of the solution is ±0.10 pH units, calculate how many moles of H3O+ can be neutralized by 250 mL of the initial buffer.arrow_forwardThe ionization of p-nitrophenol is shown below (pKa = 7.0): a. Identify the weak acid and conjugate base. b. At pH 7, what are the relative concentrations of ionized and un-ionized p-nitrophenol? c. If enough concentrated hydrochloric acid is added to a solution of p-nitrophenol to lower the pH from 7 to 5, what will happen to the relative concentrations of the ionized and un-ionized forms? d. Ionized p-nitrophenol has a yellow color, while the un-ionized form is colorless. The yellow color can be measured using a spectrophotometer at 400nm. In order to determine the total amount of p-nitrophenol in a solution, would you perform the spectrophotometer reading at an acidic or basic pH? Clearly explain why? e. A solution of p-nitrophenol at pH 7.95 was found to have an A400 of 0.255 . What is the total concentration (in µM) of p-nitrophenol (ionized plus un-ionized) in the solution? The molar extinction coefficient of p-nitrophenol is 18,500 M-1cm-1 and the pKa is 7.arrow_forward
- The liquids butan-1-ol and butanal have similar molar masses. Which is expected to have the higher boiling point? Explain your choices.arrow_forwardThe empirical formula of the sugar glucose is C6H12O6. (a) How many moles are there in 270 g of glucose? (b) Calculate the molarity of a solution of 324 g of glucose dissolved in 2.0 l of water.arrow_forwardIn an experiment, what happens to the calculated molar mass after waiting an hour between thawing the frozen cyclohexane and adding the unknown compound, during which time some of the cyclohexane evaporated. Will the molar mass be too large, too small, or unaffected? Explain.|arrow_forward
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