Reference no: EM131173177
You had learnt about "solubility product" (Ksp) in First Year Chemistry (see page 124 of textbook by Harris). Given the Ksp of calcium phosphate is 1.2 × 10-29,
(i) write down an appropriate chemical equation that shows the solubility of calcium phosphate.
(ii) write down an expression for Ksp of calcium phosphate based on your answer in
(iii) calculate the solubility of calcium phosphate.
(iv) if the standard deviation of this Ksp is 0.1 × 10-29, what is the standard deviation of the solubility of calcium phosphate calculated in (iii)?
(b) The Nernst equation, applied in potentiometric analysis, is expressed as
E=Eo +RTlogeC nF
where E is the measured potential of the electrode, E° is the standard electrode potential for the ion to be determine, T is the absolute temperature, n is the number of electrons involved in the half-cell concerned, C is the concentration of the ion, R is the gas constant and F is the Faraday constant.
Obtain an expression for the relative standard deviation of the concentration, assuming that T = 298 K and is without error. Then, calculate the value of the relative standard deviation if n = 1 and the standard deviation of E is 0.001 V. You can also assume E° is error free.
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