Home
Class 11
CHEMISTRY
When 0.10 mol of ammonia NH3 is dissolve...

When 0.10 mol of ammonia `NH_3` is dissolved in sufficient water to make 1.0L of solution, the solution is found to have a hydroxide ion concentration of `1.34 xx 10^(-3)`. Calculate `k_b` for Ammonia.

Promotional Banner

Topper's Solved these Questions

  • ENVIRONMENTAL CHEMISTRY

    PATHFINDER|Exercise QUESTION BANK|157 Videos

  • GOC-II & III

    PATHFINDER|Exercise QUESTION BANK|144 Videos

Similar Questions

Explore conceptually related problems

Calculate k_a for a dibasic acid if its concentration is 0.05 N and hydrogen ion concentration is 1 xx 10^(-3) mol L^(-1)

K_a for HCN is 1.4 xx 10^(-9) . Calculate for 0.01 N KCN solution. pH

When 50 mL 0.1 NH_3 is mixed with 10mL of 0.1 M HCl when what is the pH of resultant solution? (pK_b=4.75) -

Calculate the volume of 14.3m NH3, solution needed to prepare 1L of 0.1M solution.

If 1 mol of an electrolyte is dissolved in V cm^(3) of a solution, then molar conductivity of the solution is Lambda_(m) = conductivity of the solution xx V. If the concentration of the solution is (M)/(10), then find the value of V.

Calculate the pH of the following solution: 0.3g of NaOH dissolved in water to give 200 mL of solution.

Determine the pH of an aqueous solution of ammonia if the concentration of the solution is 3(M). K_(b) (ammonia) =1.8xx10^(-5) .

800mL 0.l(M) HCl solution is mixed with 200mL 0.5(M) CH_3NH_2 solution. In the resulting solution , concentration of H_3O^(+) ions is [K_b(CH_3NH_2)=5xx10^(-4)] is

An aqueous solution of 0.1 molal concentration of sucrose should have freezing point (k_f = 1.86 k mol^(-1) kg)

PATHFINDER-EQUILIBRIUM-QUESTION BANK
  1. The species : H2O, HCO3-, HSO4-, and NH3 can act both as bronsted aci...

    Text Solution

    |

  2. Calculate the H^+ ion concentration of a 0.01N weak monobasic acid. Th...

    Text Solution

    |

  3. When 0.10 mol of ammonia NH3 is dissolved in sufficient water to make ...

    Text Solution

    |

  4. What is the pH of the solution when 0.2 mol of HCI is added to one lit...

    Text Solution

    |

  5. Calculate the pH of 0.08M solution of hypochlorous acid, HOCI. The ion...

    Text Solution

    |

  6. The pH of a buffer is 4.745. When 0.01 mol of NaOH is added to 1 litre...

    Text Solution

    |

  7. Calculate the pH of the solution in which 0.2M NH4CI and 0.1 M NH3 are...

    Text Solution

    |

  8. Calculate pH of 1 M PO4^-3) (aq) solution. pkb(PO4^-3) = 1.62

    Text Solution

    |

  9. Hydrolysis constant of NH4^+ is 5.55 xx 10^(-10). What is ionisation c...

    Text Solution

    |

  10. A weak acid HX has the dissociation constant 1xx10^-5M. It forms a sal...

    Text Solution

    |

  11. The solubility product of Mg (OH)2 is 1×10^(−11). At what pH, precipit...

    Text Solution

    |

  12. If a saturated solution is prepared by dissolving Ag2CO3 in water has ...

    Text Solution

    |

  13. Calculate the solubility of A2X3 in pure water, assuming that neither ...

    Text Solution

    |

  14. Calculate the molar solubility of Ni(OH)2 in 0.10 M NaOH. The solubili...

    Text Solution

    |

  15. An indicator has pkin = 5.3. In a certain solution, this indicator is ...

    Text Solution

    |

  16. An indicator has pkin = 5.3. In a certain solution, this indicator is ...

    Text Solution

    |

  17. The ionization constant of an acid-base indicator (a weak acid) is 1.0...

    Text Solution

    |

  18. Calculate the degree of ionization of 0.1 M acetic acid. The dissociat...

    Text Solution

    |

  19. Calculate the concentration of OH^ ions of 0.01 M NH4OH : Kb = 1.58 xx...

    Text Solution

    |

  20. At 15^@C 0.05 N solution of a weak monobasic acid is 3.5% ionised. Cal...

    Text Solution

    |