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2 marksSolubility Product

CAPE Chemistry Unit 1 · 2011 · Paper 2 · Question 2(c)(ii)

Kidney stones can form from calcium phosphate (Ca3(PO4)2), which has a Ksp of 1.3 × 10⁻³² at 25 °C. A patient's urine sample contains 1.2 × 10⁻⁴ mol dm⁻³ calcium ions and 1.1 × 10⁻⁸ mol dm⁻³ phosphate ions.

Write the expression for the solubility product constant for calcium phosphate.

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Other parts of this question

  1. 2(a)(i)List the factor which affects the solubility product constant, Ksp.[1 mark]
  2. 2(a)(ii)List ONE factor (except that in (i) above) which influences the solubility of a salt.[1 mark]
  3. 2(b)Describe the 'common ion effect' as it relates to the solubility of salts.[2 marks]
  4. 2(c)(i)Write a balanced equation for the formation of calcium and phosphate ions from calcium phosphate.[2 marks]
  5. 2(c)(iii)Calculate the ionic product of calcium phosphate in the patient's urine.[1 mark]
  6. 2(c)(iv)State why kidney stones are likely to form in the patient's urine.[1 mark]
  7. 2(d)Outline an experimental procedure for the determination of the solubility product constant of barium hydroxide Ba(OH)2.[5 marks]

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