Home
Class 12
CHEMISTRY
Calculate the concentrations of Ca^(2+) ...

Calculate the concentrations of `Ca^(2+)` and `PO_4^(3-)` ions in a saturated `[Ca_3(PO_4)_2]` solution. Given:
`K_(sp)[Ca_3(PO_4)_2]=2.0xx10^(-29)` (at `25^(@)C`)

Text Solution

Verified by Experts

`Ca_3(PO_4)_2(s) `K_(sp)=(3s)^3xx(2s)^2`
[S= solubility of `Ca_3(PO_4)_2]=108s^5`
or `108s^5=2xx10^(-29):.S=7.137xx10^(-7)(M)`
`:.[Ca^(2+)]=2S=3xx7.137xx10^(-7)=2.14xx10^(-6)(M)`
`[PO_4^(3-)]=2S=2xx7.137xx10^(-7)(M)=1.42xx10^(-6)(M)`
Promotional Banner

Topper's Solved these Questions

  • EQUILIBRIUM

    CHHAYA PUBLICATION|Exercise PRACTICE TEST 7|14 Videos

  • EQUILIBRIUM

    CHHAYA PUBLICATION|Exercise SHORT TYPE QUESTIONS|25 Videos

  • ENVIRONMENTAL CHEMISTRY

    CHHAYA PUBLICATION|Exercise PRACTICE SET 14(Answer the following questions)|6 Videos

  • GENERAL PRINCIPLES AND PROCESSES OF ISOLATION OF ELEMENTS

    CHHAYA PUBLICATION|Exercise PRACTICE SET 6|10 Videos

Similar Questions

Explore conceptually related problems

At what concentration of PO_(4)^(3-) ions in 0.1(M) aqueous solution of AgNO_(3), will Ag_(3)PO_(4) start to precipitate?Given: K_(sp)(Ag_(3)PO_(4))=1.3xx10^(-20) .

The bond order between P and O in PO_4^(3-) is

Charge carried by 1 mole PO_4^(3-) ions is.

A solution contains Ag^+,Ca^(2+) and Al^(3+) each having a concentration of 0.1(M). Na_3PO_4 is added to the solution. Which will be precipitated first when the concentration of PO_4^(-3) in the solution is the lowest ? [ Given : K_(sp) values of Ag_3PO_4,Ca_3(PO_4)_2 and AlPO_4 and 10^(-16) , 10^(-33) and 10^(-20) respectively]

What is the percentage of P_(2)O_(5) in calcium phosphate [Ca_(3)(PO_(4))_(2)] ?

Concentration of the Ag^(+) ions in a saturated solution of Ag_(2) C_(2) O_(4) is 2.2 xx 10^(-4)M ). Calculate Ksp

What is the amount of charge carried by 1 mol PO_(4)^(3-) ion?

The concentration of Ca^(2+) ions in a saturated CaF_2 solution is 8.4 mg*L^(-1) at 25^(@) C. Calculate the solubility product of CaF_2 at that temperature.

Freshly precipitated aluminium and magnesium hydroxides are stirred vigorously in a buffer solution containing 0.25 mol L^(-1) of NH_4Cl and 0.05(M) of ammonium hydroxide. Calculate the concentration of aluminium and magnesium ions in solution. K_b(NH_4OH)=1.8xx10^(-5),K_(sp)[Al(OH)_3]=6xx10^(-32) K_(sp)[Mg(OH)_2)]=8.9xx10^(-12)

CHHAYA PUBLICATION-EQUILIBRIUM-LONG TYPE QUESTIONS
  1. Calculate (i) pH of the solution, (ii) degree of hydrolysis of NaCN...

    Text Solution

    |

  2. Calculate (i) pH of the solution, (ii) degree of hydrolysis of NaCN...

    Text Solution

    |

  3. Find the degree of hydrolysis, pH of the solution and hydrolysis const...

    Text Solution

    |

  4. The concentration of Ca^(2+) ions in a saturated CaF2 solution is 8.4m...

    Text Solution

    |

  5. Calculate the concentrations of Ca^(2+) and PO4^(3-) ions in a saturat...

    Text Solution

    |

  6. What will be the solubility of Pb(OH)2 in buffer of pH=9 at 25^(@)C pr...

    Text Solution

    |

  7. A solution contains Ag^+,Ca^(2+) and Al^(3+) each having a concentrati...

    Text Solution

    |

  8. If equal volumes of 0.02(M) CaCl2 and 0.0003(M) Na2SO4 solutions are m...

    Text Solution

    |

  9. What will be the value of pH at which Mg(OH)2 starts to precipitate fr...

    Text Solution

    |

  10. if K(sp)(CaF2)=4xx10^(-11) at 25^(@)C then find the molar solubility o...

    Text Solution

    |

  11. if K(sp)(CaF2)=4xx10^(-11) at 25^(@)C then find the molar solubility o...

    Text Solution

    |

  12. if K(sp)(CaF2)=4xx10^(-11) at 25^(@)C then find the molar solubility o...

    Text Solution

    |

  13. 10^(-4) mol Pb(NO3)2,10^(-4) mol Ca(NO3)2 and 10^(-3) mol Na2CO3 are a...

    Text Solution

    |

  14. A solution contains a mixture of Ag^+(0.1M) and Hg^(2+) (0.1M) which a...

    Text Solution

    |

  15. The solubility product (Ksp) of Ca(OH)2 at 25^(@)C is 4.42xx10^(-5). A...

    Text Solution

    |

  16. An aqueous solution of a metal bromide MBr2 (0.05M) is saturated withH...

    Text Solution

    |

  17. The molar concentration of an aqueous CH3COONa solution is 0.01(M). Ca...

    Text Solution

    |

  18. The molar concentration of an aqueous CH3COONa solution is 0.01(M). Ca...

    Text Solution

    |

  19. The molar concentration of an aqueous CH3COONa solution is 0.01(M). Ca...

    Text Solution

    |

  20. Determine the hydrolysis constant and pH of an aqueous 1.0(M) ammonium...

    Text Solution

    |