Home
Class 11
CHEMISTRY
Calculate ka for a dibasic acid if its c...

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)`

Text Solution

Verified by Experts

`2 xx 10^(-8) M^2`
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

Dissociation constant of a weak acid is K_a and its concentration is C, the concentration of hydrogen ion is

When pH of a solution is 2, the hydrogen ion concentration in moles "litre"^(-1) is .............

The concentration of hydrogen ion in a sample of soft drink is 3.8xx10^(-3)(M) , what is its pH?

Consider a certain reaction Ararr products with k=2.0xx10^(-2)s^(-1) .Calculate the concentration of a A remaining after 100s if the initial concentration of A is 1.0"mol .L"^(-1) .

Calculate the H^+ ion concentration of a 0.01N weak monobasic acid. The value of dissociation constant is 4.0 xx 10^(-10) .

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.

Calculate ionisation constant for pyridinium hydrogen Chloride. (given that H^+ ion concentration is 3.6xx10^(-4) M and its concentration is 0.02 M)-

Calculate the conductivity of a semiconductor having electron concentration 5xx10^(12)"cm"^(-3) and hole concentration 8xx10^(13)"cm"^(-3) [mu_(e)=2.3"V"^(-1).s^(-1)."m"^(2)" ""and"" " mu_(h)=0.1"V"^(-1).s^(-1)."m"^(2)]

Consider the reaction 2Ararr4B+C taking place in a closed container. If the concentration of B increases to 5xx10^(-3)"mol".L^(-1) in 10s , then find the reaction -rate in the given interval.

Consider the reaction 2Ararr4B+C taking place in a closed container. If the concentration of B increases to 5xx10^(-3)"mol".L^(-1) in 10s , then find the rate of formation of B

PATHFINDER-EQUILIBRIUM-QUESTION BANK
  1. Calculate the concentration of OH^ ions of 0.01 M NH4OH : Kb = 1.58 xx...

    Text Solution

    |

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

    Text Solution

    |

  3. Calculate ka for a dibasic acid if its concentration is 0.05 N and hyd...

    Text Solution

    |

  4. Calculate the approximate pH of 0.1 M aqueous H2S solution. K1 and k2 ...

    Text Solution

    |

  5. 9.8 g of H2SO4 is present in 500 mL of the solution. Calculate the pH ...

    Text Solution

    |

  6. Find the concentration of H^+, HCO3^-, and CO3^(2-) in a 0.01 M soluti...

    Text Solution

    |

  7. The degree of dissociation of water is 1.8 xx 10^(-9) at 298 K. Calcul...

    Text Solution

    |

  8. The pH of a solution of B(OH)2 is 10.6. Calculate the solubility and s...

    Text Solution

    |

  9. What happens to the pH of 500 mL of a solution that is 0.1 molar in so...

    Text Solution

    |

  10. The concentration of HCN and NaCN in a solution is 0.01 M each. Calcul...

    Text Solution

    |

  11. One litre of a buffer solution is prepared by dissolving 0.6 mole. of ...

    Text Solution

    |

  12. One litre of a buffer solution is prepared by dissolving 0.6 mole. of ...

    Text Solution

    |

  13. Calculate the ratio of pH of a solution containing 1 mole CH3COONa + 1...

    Text Solution

    |

  14. Ka for HCN is 1.4 xx 10^(-9). Calculate for 0.01 N KCN solution. Degre...

    Text Solution

    |

  15. Ka for HCN is 1.4 xx 10^(-9). Calculate for 0.01 N KCN solution: [OH^...

    Text Solution

    |

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

    Text Solution

    |

  17. Calculate the degree of hydrolysis of 0.10 M solution of KCN. Dissocia...

    Text Solution

    |

  18. The solubility of CaSO4 at 25^@C is 2.036 g L^(-1) and degree of disso...

    Text Solution

    |

  19. A solution is saturated with respect to strontium fluoride and stronti...

    Text Solution

    |

  20. The solubility product of AgCI is 1.5 xx 10^-10). Predict whether ther...

    Text Solution

    |