Explain how to produce an ideal precipitate in the analysis of sodium fluoride, NaF with silver nitrate, AgNO3 as precipitant using precipitation gravimetry

If a student combines specific amount CaCl2. 9H2O and Na2CO3 and obtained a solid precipitate. The student dissolve 1.37 gram of CaCl2. 9H2O in 25.0 mL of water and 0.984 g of Na2CO3 in 25.0 mL of water.  The student is then combining the two solutions and observed the formation of a solid precipitate. The student filter the solution and recovered the precipitate. The following data were obtained for the experiment.   Initial Mass of CaCl2. 9H2O 1.37 g    Initial Mass of Na2CO3 0.984 g % yield of this experiment 87.4% 1. What is the balanced equation for this experiment?

Hydroxyapatite, Ca₁(PO)(OH)₂, Ca₁(PO4)(OH)₂ (s) ⇒ 10 Ca² ¹(aq) + 6PO³(aq) + 2OH(aq) has a solubility constant of Ksp = 2.34 × 10-5⁹, and dissociates according to 10 Solid hydroxyapatite is dissolved in water to form a saturated solution. What is the concentration of Ca²+in this solution if [OH-] is fixed at 6.20 x 10-4 M?

15). If Ca(NO3) (aq) is slowly added to solution containing CO32– and SO42– what compound would precipitate out first given the solubility products (Ksp (CaSO4) = 2.4 x 10–5 and Ksp (CaCO3) = 8.7 x 10–9)? CaCO3 would precipitate first because it is least soluble. CaSO4 would precipitate first because it is least soluble. CaCO3 would precipitate first because it is more soluble. CaSO4 would precipitate first because it is more soluble.

The value of the thermodynamic solubility product of silver bromide in pure water is Ksp = 5.0x10-13. Calculate the value of the concentration solubility product of silver bromide in a 0.10 M NaNO3 solution. Let's assume the temperature is the same.

1. Explain what is meant by the term Precipitate. 2. Calculate the solubility of Fe(OH)2 at 298 K in 1.0 mol dm³ NaOH given the solubility product constant (Ksp) of Fe(OH)2 at this temperature is 7.9 x 10-16 mol³ dmº.

Consider the following mixtures of chemicals. Complete the table by writing balanced equations and calculating the value of Q. Hence indicate whethe precipitation will occur.  Mixture Balanced equation Ksp Q Precipitation occurs (yes or no) 100mL 0.5 molL-1 Ca(NO3)2 mixed with 100 mL 0.2 molL-1 Na2SO4         20 mL 0.01 molL-1 AgNO3 mixed with 80 mL 0.05 molL-1 K2CrO4

Consider a solution that contains 0.10 M AsO43 and 0.15 M CO32. Solid Co(NO3)2 is added to separate these two anions. Ksp of Co3(AsO4)2 = 6.8 x 1029 and Ksp of COCO3 = 1.0 x 10 %3D 10 Assume the volume change is negligible. As solid Co(NO3)2 is added to this solution, which solid will precipitate first and what is the [Co2*] needed to maintain the maximum separation of AsO43 and CO32? COCO3 precipitates first and [Co2+]max = 9.1 x 10-7M COCO3 precipitates fırst and [Co2+]max = 1.9 x 10-9 M Co3(AsO4)2 precipitates first and [Co2+]max = 1.9 x 10-9 M None of these Co3(AsO4)2 precipitates first and [Co2*]max = 9.1 x 10-7M Co3(AsO4)2 precipitates first and [Co2*]max = 6.7 x 10-10 M COCO3 precipitates first and [Co2*]max = 6.7 x 10-10M

To determine the solubility product constant of Al(OH)3 at a specific temperature, a saturated solution of Al(OH)3 at the required temperature was titrated with 0.2M HCl via the reaction: 3HCl + Al(OH)3  → AlCl3 + 3H2O.  Based on the following data, determine the Ksp of Al(OH)3 at the specified temperature:                Volume of Al(OH)3 titrated: Volume of 0.2M HCl required: 9.5 mL 3.44 mL Your answer should follow the format: a) mols of HCl added b) mols of Al(OH)3 c) Molarity of Al(OH)3 d) Ksp of Al(OH)3 (2 marks)