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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).
classification of gels
a sample of CaCo3 and MgCo3 weighing 192g is ignited to constanr weight of 104 gm . what is the composition of mixture ?
Calculate the molarmass of a nonelectrolyte that lowers the freezing point of 25.00g of water to -3.9 degrees C when 4.27 g of the substance is dissolved in the water.
What is mole?
Scale up At this phase, sensory analysis consists of tests that compare the production samples with the optimized product. Depending on the resources available, either consume
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write the structures of the major product (saytzeff elimination) when the following alcohols are dehydrated with hot,concentrated sulphuric acid. 1. 3-methyl-2-butanol 2. 2-pentano
What property command to water soluble vitamins permits water solubility Ans) Because of 1]OH bond between them 2] polar componets 3] Availibility of in nature
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