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(a) Explain in terms of ionic equilibria why the aqueous solution of a salt derived from a weak acid and a strong base (e.g. sodium phenolate) has a pH greater than 7.
(b) By considering the equilibrium constant (Ka) of a weak acid, and the effect on Ka when a salt of that acid is added to the solution, derive the Henderson-Hasselbalch equation for buffer solution pH.
(c) Explain why the Henderson-Hasselbalch equation sometimes features a term written as + log10 gA- where gA- represents the activity coefficient of the common anion, and hence describe the effect of increasing the concentration of both the acid and salt in the buffer formulation on buffer performance.
(d) An aqueous buffer solution is formulated containing 0.010 mol dm-3 sodium phenolate to which phenol is added. Given that the pKa of phenol is 9.98, calculate the concentration of phenol required to produce a pH of exactly 9.65 (you may assume that gA- = 1).
20ml of water sample requires 15ml of 0.1mg/l sodium carbonate using phenolphthalein indicator. state the type of acidity and calculate the acidity
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Q. Significant figures of the number of digits? Significant figures of the number of digits reported in a measurement signify how precise the measurement is. The further di
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The de-Broglie wavelength associated with a material particle is: (1) Directly proportional to its energy (2) Directly proportional to momentum (3) Inversely proportiona
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Q. How to evaluate mass number? An isotope of an element is recognized by its mass number which is the sum of the number of protons and neutrons in the atom's nucleus. Mas
Determine the alcoholic acidity of the given sample of flour. After undertaking this activity, you will be able to: • assess the acidity the given sample of flour, and •
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